CHEM 1201 Borill LSUE Exam 4

Given w = 0, an endothermic reaction has the following. A) +ΔH and -ΔE B) - ΔH and +ΔE C) + ΔH and +ΔE D) - ΔH and -ΔE

+ ΔH and +ΔE

Calculate the change in internal energy (ΔE) for a system that is absorbing 35.8 kJ of heat and is expanding from 8.00 to 24.0 L in volume at 1.00 atm. (Remember that 101.3 J = 1 L∙atm) A) +51.8 kJ B) -15.8 kJ C) -16.6 kJ D) -29.3 kJ E) +34.2 kJ

+34.2 kJ

The temperature rises from 25.00°C to 29.00°C in a bomb calorimeter when 3.50 g of sucrose undergoes combustion in a bomb calorimeter. Calculate ΔErxn for the combustion of sucrose in kJ/mol sucrose. The heat capacity of the calorimeter is 4.90 kJ/°C. The molar mass of sugar is 342.3 g/mol. A) - 1.92 × 103 kJ/mole B) 1.92 × 103 kJ/mole C) - 1.23 × 103 kJ/mole D) 2.35 × 104 kJ/mole

- 1.92 × 103 kJ/mole

A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature rose from 35.0 to 76.0°C and the heat capacity of the calorimeter is 23.3 kJ/°C, what is the value of DH°rxn? The molar mass of ethanol is 46.07 g/mol. C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(g) ΔH°rxn = ? A) -1.24 × 103 kJ/mol B) +1.24 × 103 kJ/mol C) -8.09 × 103 kJ/mol D) -9.55 × 103 kJ/mol E) +9.55 × 103 kJ/mol

-1.24 × 103 kJ/mol

At constant pressure, the combustion of 6.00 g of C4H10(g) releases 297 kJ of heat. What is ΔH for the reaction given below? 2 C4H10(g) + 13 O2(g) → 8 CO2(g) + 10 H2O(l) A) -54.2 kJ B) -779 kJ C) -6024 kJ D) -11508 kJ

-6024 kJ

For ΔEsys to always be -, what must be TRUE? A) q = w B) +q > -w C) +w > -q D) -w > +q

-w > +q

How many moles of Ar are contained in a 5.00 L tank at 155°C and 2.80 atm? A) 0.399 moles B) 1.10 moles C) 2.51 moles D) 0.455 moles E) 0.289 moles

0.399 moles

Determine the density of NH3 gas at 435 K and 1.00 atm. A) 2.10 g/L B) 0.477 g/L C) 0.321 g/L D) 2.24 g/L E) 0.851 g/L

0.477 g/L

Zinc reacts with aqueous sulfuric acid to form hydrogen gas: Zn(s) + H2SO4(aq) → ZnSO4 (aq) + H2(g) In an experiment, 225 mL of wet H2 is collected over water at 27°C and a barometric pressure of 748 torr How many grams of Zn have been consumed? The vapor pressure of water at 27°C is 26.74 torr A) 4.79 × 10^6 B) 0.567 C) 567 D) 431 E) 4.31 × 10^5

0.567

A 9.50L cylinder contains a mixture of 138 g Ne and 403 g Cl2 at 325 K. What is the partial pressure of Cl2? A) 16.0 atm B) 19.5 atm C) 6.53 atm D) 35.5 atm

16.0 atm

A gas occupies 4.23 L at 2.25 atm. What is the volume at 3.46 atm? A) 6.50 L B) 1.84 L C) 2.75 L D) 32.9 L E) 0.364 L

2.75 L

How many liters of oxygen are needed to exactly react with 19.8 g of methane at STP? CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) A) 13.9 L B) 27.8 L C) 55.5 L D) 60.5 L

55.5 L

How many molecules of N2 are in a 400.0 mL container at 780 mm Hg and 135°C? A) 7.01 × 1021 molecules B) 7.38 × 1021 molecules C) 2.12 × 1022 molecules D) 2.23 × 1022 molecules

7.38 × 1021 molecules

A syringe initially holds a sample of gas with a volume of 285 mL at 355 K and 1.88 atm. To what temperature must the gas in the syringe be heated/cooled in order to have a volume of 435 mL at 2.50 atm? A) 139 K B) 572 K C) 175 K D) 466 K E) 721 K

721 K

Energy that is associated with the relative positions of electrons and nuclei in atoms and molecules is called A) kinetic energy. B) thermal energy. C) gravitational energy. D) chemical energy

chemical energy

Identify what a coffee cup calorimeter measures. A) measures ΔH for aqueous solutions B) measures ΔE for hydrolysis reactions C) measures ΔH for reduction solutions D) measures ΔT for combustion solutions E) measures ΔE for oxidation reactions

measures ΔH for aqueous solutions

All of the following statements concerning real cases is correct EXCEPT A) molecules of real gases are attracted to each other. B) molecules of real gases occupy no volume. C) the pressure of a real gas at low temperatures is lower than for ideal gases. D) the pressure of a real gas is due to collisions with the container. E) nonideal gas behavior is described by the Van der Waals Equation.

molecules of real gases occupy no volume.

The rate of effusion of argon to an unknown gas is 1.194. What is the other gas? A) oxygen B) nitrogen C) neon D) krypton E) hydrogen

nitrogen

Define hypoxia. A) oxygen starvation B) increased oxygen concentration in body tissues C) increased nitrogen concentration in body tissues and fluids D) nitrogen starvation

oxygen starvation

Define vapor pressure. A) partial pressure of water in a liquid mixture B) partial pressure of water in a gaseous mixture C) condensation of water D) water dissolved in a liquid E) water molecules

partial pressure of water in a gaseous mixture

All the following are state functions EXCEPT A) ∆E. B) PV. C) ∆H. D) q. E) all of the above are state functions.

q.

An instrument used to measure blood pressure is called a A) barometer. B) manometer. C) sphygmomanometer. D) spectrophotometer. E) spectrometer

sphygmomanometer.

Which of the following processes are endothermic? A) the reaction associated with the lattice energy of LiCl B) the reaction associated with the ionization energy of potassium C) the reaction associated with the heat of formation of CaS D) the formation of F2 from its elements in their standard states E) None of the above are endothermic.

the reaction associated with the ionization energy of potassium

Which of the following processes is endothermic? A) the freezing of water B) the combustion of butane C) a hot cup of coffee (system) cools on a countertop D) the chemical reaction in a "hot pack" often used to treat sore muscles E) the vaporization of rubbing alcohol

the vaporization of rubbing alcohol

The combustion of titanium with oxygen produces titanium dioxide: Ti(s) + O2(g) → TiO2(s) When 2.060 g of titanium is combusted in a bomb calorimeter, the temperature of the calorimeter increases from 25.00°C to 91.60°C. In a separate experiment, the heat capacity of the calorimeter is measured to be 9.84 kJ/K. The heat of reaction for the combustion of a mole of Ti in this calorimeter is ________ kJ/mol. A) 14.3 B) 19.6 C) -311 D) -0.154 E) -1.52 ×10^4

-1.52 ×10^4

Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2H2O2(l) → 2H2O(l) + O2(g) ΔH = -196 kJ Calculate the value of q (kJ) in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pressure? A) -23.1 kJ B) -11.5 kJ C) -0.0217 kJ D) 1.44 kJ E) -2.31 × 104 kJ

-11.5 kJ

Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction 2 NO(g) + O2(g) → 2 NO2(g) ΔH°rxn = ? Given: N2(g) + O2(g) → 2 NO(g) ΔH°rxn = +183 kJ 1/2 N2(g) + O2(g) → NO2(g) ΔH°rxn = +33 kJ A) -150. kJ B) -117 kJ C) -333 kJ D) +115 kJ E) +238 k

-117 kJ

Use the bond energies provided to estimate ΔH°rxn for the reaction below. C2H4(g) + H2(g) → C2H6(g) ΔH°rxn = ? Bond Bond Energy (kJ/mol) C-C 347 C-H 414 C=C 611 C≡C 837 H-H 436 A) -128 kJ B) +98 kJ C) +700 kJ D) -102 kJ E) -166 kJ

-128 kJ

When 1.50 mol of CH4(g) reacts with excess Cl2(g) at constant pressure according to the chemical equation shown below, 1062 kJ of heat are released. Calculate the value of ΔH for this reaction, as written. 2 CH4(g) + 3 Cl2(g) → 2 CHCl3(l) + 3 H2(g) ΔH = ? A) -1420 kJ B) -708 kJ C) +708 kJ D) +1420 kJ

-1420 kJ

The volume of 350. mL of gas at 25°C is decreased to 135 mL at constant pressure. What is the final temperature of the gas? A) -158°C B) 9.6°C C) 65°C D) 500°C

-158°C

Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction P4(g) + 10 Cl2(g) → 4PCl5(s) ΔH°rxn = ? Given: PCl5(s) → PCl3(g) + Cl2(g) ΔH°rxn = +157 kJ P4(g) + 6 Cl2(g) → 4 PCl3(g) ΔH°rxn = -1207 kJ A) -1835 kJ B) -1364 kJ C) -1050. kJ D) -1786 kJ E) -2100. kJ

-1835 kJ

Use the bond energies provided to estimate ΔH°rxn for the reaction below. 2 Br2(l) + C2H2(g) → C2H2Br4(l) ΔH°rxn = ? Bond Bond Energy (kJ/mol) Br-Br 193 C≡C 837 C-C 347 C-Br 276 C-H 414 A) +407 kJ B) -324 kJ C) -228 kJ D) +573 kJ E) -648 kJ

-228 kJ

Calculate the change in internal energy (ΔE) for a system that is giving off 25.0 kJ of heat and is changing from 12.00 L to 6.00 L in volume at 1.50 atm pressure. (Remember that 101.3 J = 1 L∙atm) A) +25.9 kJ B) -16.0 kJ C) -25.9 kJ D) -24.1 kJ E) 937 kJ

-24.1 kJ

Calculate the change in internal energy (ΔE) for a system that is giving off 25.0 kJ of heat and is changing from 18.00 L to 15.00 L in volume at 1.50 atm pressure. (Remember that 101.3 J = 1 L∙atm) A) +25.5 kJ B) -16.0 kJ C) -25.5 kJ D) -24.5 kJ E) 456 kJ

-24.5 kJ

Use the bond energies provided to estimate ΔH°rxn for the reaction below. XeF2 + 2 F2 → XeF6 ΔH°rxn = ? Bond Bond Energy (kJ/mol) Xe-F 147 F-F 159 A) -429 kJ B) +159 kJ C) -660 kJ D) +176 kJ E) -270 kJ

-270 kJ

A 4.98 g sample of aniline (C6H5NH2, molar mass = 93.13 g/mol) was combusted in a bomb calorimeter with a heat capacity of 4.25 kJ/°C. If the temperature rose from 29.5°C to 69.8°C, determine the value of ΔH°comb for aniline. A) +7.81 × 103 kJ/mol B) -3.20 × 103 kJ/mol C) +1.71 × 103 kJ/mol D) -1.71 × 103 kJ/mol E) -7.81 × 103 kJ/mol

-3.20 × 103 kJ/mol

Calculate the work, w, gained or lost by the system when a gas expands from 15 L to 40 L against a constant external pressure of 1.5 atm. 1 L ∙ atm = 101 J A) -6.1 kJ B) -3.8 kJ C) +3.8 kJ D) +6.1 kJ

-3.8 kJ

At constant pressure, the combustion of 15.0 g of C2H6(g) releases 777 kJ of heat. What is ΔH for the reaction given below? 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(l) A) -129 kJ B) -779 kJ C) -1560 kJ D) -3120 kJ

-3120 kJ

Use the information provided to determine ΔH°rxn for the following reaction ΔH°f (kJ/mol) CH4(g) + 3 Cl2(g) → CHCl3(l) + 3 HCl(g) ΔH°rxn = ? CH4(g) -75 CHCl3(l) -134 HCl(g) -92 A) -151 kJ B) -335 kJ C) +662 kJ D) +117 kJ E) -217 kJ

-335 kJ

Sodium metal reacts with water to produce hydrogen gas and sodium hydroxide according to the chemical equation shown below. When 0.0 25 mol of Na is added to 100.00 g of water, the temperature of the resulting solution rises from 25.00°C to 35.75°C. If the specific heat of the solution is 4.18 J/(g ∙ °C), calculate ΔH for the reaction, as written. 2 Na(s) + 2 H2O(l) → 2 NaOH(aq) + H2(g) ΔH = ? A) -5.41 kJ B) -90.0 kJ C) -180 kJ D) -360 kJ

-360 kJ

Use the information provided to determine ΔH°rxn for the following reaction ΔH°f (kJ/mol) CH4(g) + 4 Cl2(g) → CCl4(g) + 4 HCl(g) ΔH°rxn = ? CH4(g) -75 CCl4(g) -96 HCl(g) -92 A) -389 kJ B) -113 kJ C) +113 kJ D) -71 kJ E) +79 kJ

-389 kJ

Use the bond energies provided to estimate ΔH°rxn for the reaction below. CH3OH(l) + 2 O2(g) → CO2(g) + 2 H2O(g) ΔH°rxn = ? Bond Bond Energy (kJ/mol) C-H 414 C-O 360 C=O 799 O=O 498 O-H 464 A) +473 kJ B) -91 kJ C) -486 kJ D) -392 kJ E) +206 kJ

-392 kJ

A balloon is inflated from 0.0100 L to 0.400 L against an external pressure of 10.00 atm. How much work is done in joules? 101.3 J = 1 L × atm A) -39.5 J B) 39.5 J C) 0. 395 J D) -0. 395 J E) -395 J

-395 J

Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for SO3(g) ΔH°f (kJ/mol) 2 SO2(g) + O2(g) → 2 SO3(g) ΔH°rxn = -198 kJ SO2(g) -297 A) -792 kJ/mol B) -248 kJ/mol C) -495 kJ/mol D) -578 kJ/mol E) -396 kJ/mol

-396 kJ/mol

Use the bond energies provided to estimate ΔH°rxn for the reaction below. PCl3(g) + Cl2(g) → PCl5(l) ΔH°rxn = ? Bond Bond Energy (kJ/mol) Cl-Cl 243 P-Cl 331 A) -243 kJ B) -419 kJ C) -662 kJ D) -67 kJ E) -905 kJ

-419 kJ

A sample of NI3 is contained in a piston and cylinder. The samples rapidly decomposes to form nitrogen gas and iodine gas, and releases 3.30 kJ of heat and does 950 J of work. What is ∆E? A) -953.3 J B) +953.3 J C) -4250 J D) -946.7 J E) +4250 J

-4250 J

When 1.50 g of Ba(s) is added to 100.00 g of water in a container open to the atmosphere, the reaction shown below occurs and the temperature of the resulting solution rises from 22.00°C to 33.10°C. If the specific heat of the solution is 4.18 J/(g ∙ °C), calculate for the reaction, as written. Ba(s) + 2 H2O(l) → Ba(OH)2(aq) + H2(g) = ? A) -431 kJ B) -3.14 kJ C) +3.14 kJ D) +431 kJ

-431 kJ

Use the information provided to determine ΔH°rxn for the following reaction ΔH°f (kJ/mol) 3 Fe2O3(s) + CO(g) → 2 Fe3O4(s) + CO2(g) ΔH°rxn = ? Fe2O3(s) -824 Fe3O4(s) -1118 CO(g) -111 CO2(g) -394 A) +277 kJ B) -577 kJ C) -47 kJ D) +144 kJ E) -111 kJ

-47 kJ

A 100.0 mL sample of 0.300 M NaOH is mixed with a 100.0 mL sample of 0.300 M HNO3 in a coffee cup calorimeter. If both solutions were initially at 35.00°C and the temperature of the resulting solution was recorded as 37.00°C, determine the ΔH°rxn (in units of kJ/mol NaOH) for the neutralization reaction between aqueous NaOH and HCl. Assume 1) that no heat is lost to the calorimeter or the surroundings, and 2) that the density and the heat capacity of the resulting solution are the same as water. A) -55.7 kJ/mol NaOH B) -169 kJ/mol NaOH C) -16.7 kJ/mol NaOH D) -27.9 kJ/mol NaOH E) - 34.4 kJ/mol NaOH

-55.7 kJ/mol NaOH

Use the ΔH°f information provided to calculate ΔH°rxn for the following ΔH°f (kJ/mol) SO2Cl2(g) + 2 H2O(l) → 2 HCl(g) + H2SO4(l) ΔH°rxn = ? SO2Cl2(g) -364 H2O(l) -286 HCl(g) -92 H2SO4(l) -814 A) -256 kJ B) +161 kJ C) -62 kJ D) +800. kJ E) -422 kJ

-62 kJ

Two solutions, initially at 24.69°C, are mixed in a coffee cup calorimeter (Ccal = 105.5 J/°C). When a 200.0 mL volume of 0.100 M AgNO3 solution is mixed with a 100.0 mL sample of 0.100 M NaCl solution, the temperature in the calorimeter rises to 25.16°C. Determine the DH°rxn, in units of kJ/mol AgCl. Assume that the density and heat capacity of the solutions is the same as that of water. Hint: Write a balanced reaction for the process. A) -32 kJ/mol AgCl B) -78 kJ/mol AgCl C) -64 kJ/mol AgCl D) -25 kJ/mol AgCl E) -59 kJ/mol AgCl

-64 kJ/mol AgCl

Calculate the change internal energy (ΔE) for a system that is giving off 65.0 kJ of heat and is performing 855 J of work on the surroundings. A) 64.1 kJ B) -64.1 kJ C) -65.9 kJ D) 9.00 × 102 kJ E) -9.00 × 102 kJ

-65.9 kJ

Two solutions, initially at 24.60°C, are mixed in a coffee cup calorimeter (Ccal = 15.5 J/°C). When a 100.0 mL volume of 0.100 M AgNO3 solution is mixed with a 100.0 mL sample of 0.200 M NaCl solution, the temperature in the calorimeter rises to 25.30°C. Determine the DH°rxn for the reaction as written below. Assume that the density and heat capacity of the solutions is the same as that of water. NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) DH°rxn = ? A) -35 kJ B) -69 kJ C) -250 kJ D) -16 kJ E) -140 kJ

-69 kJ

When 0.455 g of anthracene, C14H10, is combusted in a bomb calorimeter that has a water jacket containing 500.0 g of water, the temperature of the water increases by 8.63°C. Assuming that the specific heat of water is 4.18 J/(g ∙ °C), and that the heat absorption by the calorimeter is negligible, estimate the enthalpy of combustion per mole of anthracene. A) +39.7 kJ/mol B) -39.7 kJ/mol C) -7060 kJ/mol D) -8120 kJ/mol

-7060 kJ/mol

Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction 2 S(s) + 3 O2(g) → 2 SO3(g) ΔH°rxn = ? Given: SO2(g) → S(s) + O2(g) ΔH°rxn = +296.8 kJ 2 SO2(g) + O2(g) → 2 SO3(g) ΔH°rxn = -197.8 kJ A) -494.6 kJ B) -692.4 kJ C) -791.4 kJ D) 1583 kJ E) -293.0 kJ

-791.4 kJ

What is the enthalpy change (in kJ) of a chemical reaction that raises the temperature of 250.0 mL of solution having a density of 1.25 g/ml by 7.80°C? (The specific heat of the solution is 3.74 J/g∙K.) A) -7.43 kJ B) -12.51 kJ C) 8.20 kJ D) -9.12 kJ E) 6.51 kJ

-9.12 kJ

In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH4(g) +2O2 (g) → CO2(g) + 2H2O(l) ΔH = -890.0 kJ Calculate the value of q (kJ) in this exothermic reaction when 1.70 g of methane is combusted at constant pressure. A) -94.6 kJ B) 0.0306 kJ C) -0.0106 kJ D) 32.7 kJ E) -9.46 × 104 kJ

-94.6 kJ

Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for IF ΔH°f (kJ/mol) IF7(g) + I2(g) → IF5(g) + 2 IF(g) ΔH°rxn = -89 kJ IF7(g) 941 IF5(g) 840 A) 101 kJ/mol B) -146 kJ/mol C) -190. kJ/mol D) -95 kJ/mol E) 24 kJ/mol

-95 kJ/mol

A piece of metal weighing 57.3 g is heated to a temperature of 88.0°C and is then immersed in 155 g of water at a temperature of 21.53°C. After equilibration the temperature is 24.72°C. If CH2O = 4.184 J/g°C, what is Cmetal? A) .370 J/g°C B) .164 J/g°C C) 1.00 J/g°C D) 2.11 J/g°C E) .571 J/g°C

.571 J/g°C

A gas bottle contains 0. 250 mol of gas at 730 mm Hg pressure. If the final pressure is 1.15 atm, how many moles of gas were added to the bottle? A) 0.0 262 mol B) 0. 0493 mol C) 0. 276 mol D) 0. 299 mol

0. 0493 mol

How many grams of KCl(s) are produced from the thermal decomposition of KClO3(s) which produces 50.0 mL of O2(g) at 25°C and 1.00 atm pressure according to the chemical equation shown below? 2 KClO3(s) → 2 KCl(s) + 3 O2(g)? A) 0. 102 g B) 0. 152 g C) 0. 167 g D) 0. 304 g

0. 102 g

A balloon filled with helium gas at 20°C occupies 4.91 L at 1.00 atm. The balloon is immersed in liquid nitrogen at -196°C, while the pressure is raised to 5.20 atm. What is the volume of the balloon in the liquid nitrogen? A) 0. 25 L B) 3.6 L C) 6.7 L D) 97 L

0. 25 L

A 2.75-L container filled with CO2 gas at 25°C and 225 kPa pressure springs a leak. When the container is re-sealed, the pressure is 185 kPa and the temperature is 10°C. How many moles of gas were lost? A) 0.0 335 mol B) 0. 728 mol C) 0. 882 mol D) 3.39 mol

0.0 335 mol

A gas occupies 22.4 L at STP and 19.0 L at 100°C and 1.50 atm pressure. How many moles of gas did the system gain or lose? A) 0.08 moles gained B) 0.01 moles gained C) 0.01 moles lost D) 0.0 7 moles lost

0.0 7 moles lost

How many moles of nitrogen will react with 380 mL of hydrogen at -30°C and 200 mm Hg? N2(g) + 3 H2(g)→ 2 NH3(g) A) 0.0150 mol B) 0.00782 mol C) 0.00501 mol D) 0.00167 mol E) 0.0382 mol

0.00167 mol

The following reaction is used to generate hydrogen gas in the laboratory. If 243 mL of gas is collected at 25°C and has a total pressure of 745 mm Hg, what mass of hydrogen is produced? A possibly useful table of water vapor pressures is provided below. Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) T (°C) P (mm Hg) 20 17.55 25 23.78 30 31.86 A) 0.0196 g H2 B) 0.0717 g H2 C) 0.0190 g H2 D) 0.0144 g H2 E) 0.0449 g H2

0.0190 g H2

The mole fraction of carbon dioxide in dry air near sea level is 0.000375, where the molar mass of carbon dioxide is 44.010. The partial pressure of carbon dioxide when the total atmospheric pressure (dry air) is 97.5 kPa is A) 2.63 × 10^5 B) 5.97 × 10^3 C) 0.0370 D) 1.63 E) 8.40 × 10^-4

0.0370

What is the density of hydrogen gas at STP? A) 11.1 g/L B) 0.0450 g/L C) 0.0823 g/L D) 0.0899 g/L

0.0899 g/L

In a container containing CO, H2, and O2, what is the mole fraction of CO if the H2 mole fraction is 0.22 and the O2 mole fraction is 0.58? A) 0.20 B) 0.30 C) 0.10 D) 0.50

0.20

A mixture of 0.220 moles CO, 0.350 moles N2 and 0.640 moles Ne has a total pressure of 2.95 atm. What is the pressure of CO? A) 1.86 atm B) 0.649 atm C) 0.536 atm D) 1.54 atm E) 0.955 atm

0.536 atm

A sample of 0.200 moles of nitrogen occupies 0.400 L. Under the same conditions, what number of moles occupies 1.200 L? A) 0.600 moles B) 0.0667 moles C) 2.40 moles D) 0.0960 moles

0.600 moles

Calculate the ratio of effusion rates of Cl2 to O2. A) 47.7 B) 0.451 C) 2.22 D) 1.49 E) 0.671

0.671

A sample of neon at 30.5°C exerts a pressure of 701 mm Hg? What is its density? A) 0.747 g/mL B) 563 g/mL C) 7.42 g/mL D) 1.38 g/mL E) 0.482 g/mL

0.747 g/mL

What is the volume of 5.60 g of O2 at 7.78 atm and 415K? A) 1.53 L B) 565 L C) 24.5 L D) 25.0 L E) 0.766 L

0.766 L

A mixture of 0.220 moles CO, 0.350 moles H2 and 0.640 moles He has a total pressure of 2.95 atm. What is the pressure of H2? A) 1.17 atm B) 0.853 atm C) 1.03 atm D) 0.969 atm E) 0.649 atm

0.853 atm

Zinc reacts with aqueous sulfuric acid to form hydrogen gas: Zn(s) +H2SO4 (aq) → ZnSO4 (aq) + H2(g) In an experiment, 201 mL of wet H2 is collected over water at 27°C and a barometric pressure of 733 torr The vapor pressure of water at 27°C is 26.74 torr. The partial pressure of hydrogen in this experiment is ________ atm. A) 0.929 B) 706 C) 0.964 D) 760 E) 1.00

0.929

A mixture of N2, O2 and He have mole fractions of 0.25, 0.65, and 0.10, respectively. What is the pressure of N2 if the total pressure of the mixture is 3.9 atm? A) 2.5 atm B) 0.39 atm C) 0.67 atm D) 0.98 atm E) 1.33 atm

0.98 atm

Give the temperature and pressure at STP. A) 0°C and 1.00 atm B) 0K and 1.00 atm C) 25°C and 1.00 in Hg D) 32K and 1 torr Hg E) 0°C and 1 mm Hg

0°C and 1.00 atm

A steel bottle contains argon gas at STP. What is the final pressure if the temperature is changed to 145°C? A) 0. 653 atm B) 0. 713 atm C) 1. 40 atm D) 1. 53 atm

1. 53 atm

A basketball is inflated to a pressure of 1. 90 atm in a 24.0°C garage. What is the pressure of the basketball outside where the temperature is -1.00°C? A) 1. 74 atm B) 1. 80 atm C) 2.00 atm D) 2.08 atm

1. 74 atm

Which one of these will diffuse the fastest at 25°C? A) 2.0 M Ar B) 1.0 M H2 C) 2.0 M N2 D) 0.5 M Ne E) 2.0 M O2

1.0 M H2

What is the temperature of NO2 gas if the average speed (actually the root-mean-square speed) of the molecules is 750 m/s? A) 1.38 K B) 1.04 × 10^3 K C) 1.38 × 10^3 K D) 1.04 × 10^6 K

1.04 × 10^3 K

A 4.00-L flask contains nitrogen gas at 25°C and 1.00 atm pressure. What is the final pressure in the flask if an additional 2.00 g of N2 gas is added to the flask and the flask cooled to -55°C? A) 0.319 atm B) 1.05 atm C) 1.44 atm D) 1.96 atm

1.05 atm

A mixture of 10.0 g of Ne and 10.0 g Ar have a total pressure of 1.6 atm. What is the partial pressure of Ne? A) 1.1 atm B) 0.80 atm C) 0.54 atm D) 0.40 atm E) 1.3 atm

1.1 atm

Calculate the kinetic energy of a 150 g baseball moving at a speed of 39. m/s ( 87 mph). A) 5.8 J B) 1.1 × 102 J C) 5.8 × 103 J D) 1.1 × 105 J

1.1 × 102 J

How many molecules of He are contained in a 10.0 L tank at 7.53 atm and 485 K? A) 1.89 × 1024 molecules B) 1.14 × 1024 molecules C) 8.32 × 1024 molecules D) 4.89 × 1024 molecules E) 3.63 × 1024 molecules

1.14 × 1024 molecules

Using the following thermochemical equation, determine the amount of heat produced per kg of CO2 formed during the combustion of benzene (C6H6). 2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(g) ΔH°rxn = -6278 kJ A) 1.43 × 105 kJ/kg CO2 B) 2.30 × 104 kJ/kg CO2 C) 4.34 × 104 kJ/kg CO2 D) 1.19 × 104 kJ/kg CO2 E) 8.40 × 105 kJ/kg CO2

1.19 × 104 kJ/kg CO2

A syringe contains 0.65 moles of He gas that occupy 750.0 mL. What volume (in L) of gas will the syringe hold if 0.35 moles of Ne is added? A) 0.87 L B) 4.9 L C) 1.2 L D) 2.1 L E) 1.9 L

1.2 L

The concentration of water vapor in a sample of air that has a partial pressure of water of 0.91 torr and a total pressure of air of 735 torr is ________ ppm. A) 1.2 × 10^3 B) 1.2 C) 0.12 D) 8.1 × 10^-4 E) 0.81

1.2 × 10^3

If NO and NH3 are allowed to effuse through a porous membrane under identical conditions, the rate of effusion for NH3 will be ________ times that of NO . A) 0.57 B) 0.75 C) 1.3 D) 1.8

1.3

How much energy is required to decompose 612 g of PCl3, according to the reaction below? The molar mass of PCl3 is 137.32 g/mol and may be useful. 4 PCl3(g) → P4(s) + 6 Cl2(g) ΔH°rxn = +1207 kJ A) 1.85 × 103 kJ B) 3.46 × 103 kJ C) 5.38 × 103 kJ D) 1.34 × 103 kJ E) 4.76 × 103 kJ

1.34 × 103 kJ

The density of nitric oxide (NO) gas at 1.21 atm and 54.1°C is ________ g/L. A) 0.0451 B) 0.740 C) 1.35 D) 0.273 E) 8.2

1.35

In the laboratory, hydrogen gas is usually made by the following reaction: Zn(s) + 2 HCl(aq) → H2(g) + ZnCl2(aq) How many liters of H2 gas, collected over water at an atmospheric pressure of 752 mm Hg and a temperature of 21.0°C, can be made from 3.566 g of Zn and excess HCl? The partial pressure of water vapor is 18.65 mm Hg at 21.0°C. A) 0. 0975 L B) 1.30 L C) 1.33 L D) 1.36 L

1.36 L

A gas mixture contains CO, Ar and H2. What is the total pressure of the mixture, if the mole fraction of H2 is 0.350 and the pressure of H2 is 0.480 atm? A) 1.37 atm B) 0.168 atm C) 5.95 atm D) 0.729 atm E) 2.1 atm

1.37 atm

A sample of copper absorbs 43.6 kJ of heat, resulting in a temperature rise of 75.0°C, determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J/g°C. A) 1.51 kg B) 6.62 kg C) 1.26 kg D) 7.94 kg E) 3.64 kg

1.51 kg

How much energy is evolved during the formation of 197 g of Fe, according to the reaction below? Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn = -852 kJ A) 1.52 × 103 kJ B) 3.02 × 103 kJ C) 8.40 × 103 kJ D) 964 kJ E) 482 k

1.52 × 103 kJ

What is the total pressure in a 6.00-L flask which contains 0.127 mol of H2(g) and 0.288 mol of N2(g) at 20.0°C? A) 0. 510 atm B) 0.681 atm C) 1.16 atm D) 1.66 atm

1.66 atm

How much energy is required to decompose 765 g of PCl3, according to the reaction below? The molar mass of PCl3 is 137.32 g/mol and may be useful. 4 PCl3(g) → P4(s) + 6 Cl2(g) ΔH°rxn = +1207 kJ A) 2.31 × 103 kJ B) 4.33 × 103 kJ C) 6.72 × 103 kJ D) 1.68 × 103 kJ E) 5.95 × 103 kJ

1.68 × 103 kJ

A syringe contains 589 mL of CO at 325 K and 1.2 atm pressure. A second syringe contains 473 mL of N2 at 298 K and 2.6 atm. What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at 273 K? A) 0.59 atm B) 1.1 atm C) 1.7 atm D) 1.9 atm E) 3.8 atm

1.7 atm

It takes 11.2 kJ of energy to raise the temperature of 145 g of benzene from 23.0°C to 68.0°C. What is the specific heat of benzene? A) 1. 14 J/(g ∙ °C) B) 1.72 J/(g ∙ °C) C) 3.48 J/(g ∙ °C) D) 5. 25 J/(g ∙ °C)

1.72 J/(g ∙ °C)

What volume will 4.91 × 1022 atoms of Ar occupy at STP? A) 1.10 L B) 2.00 L C) 2.24 L D) 3.11 L E) 1.83 L

1.83 L

A sample of CO2 gas fills a container with a volume of 44.5 L. When the volume is decreased to 13.8 L at a constant temperature, the pressure inside the container is 6.25 atm. What was the pressure inside the container originally? A) 0.035 atm B) 0.51 atm C) 1.94 atm D) 3.84 atm E) 6.25 atm

1.94 atm

Determine the density of CO2 gas at STP. A) 1.96 g/L B) 1.80 g/L C) 2.24 g/L D) 4.46 g/L E) 5.10 g/L

1.96 g/L

Which of the following substances (with specific heat capacity provided) would show the greatest temperature change upon absorbing 100.0 J of heat? A) 10.0 g Cu, CCu = 0.385 J/g°C B) 10.0 g H2O, = 4.18 J/g°C C) 10.0 g ethanol, Cethanol = 2.42 J/g°C D) 10.0 g Al, CAl = 0.903 J/g°C E) 10.0 g Pb, CPb= 0.128 J/g°C

10.0 g Pb, CPb= 0.128 J/g°C

A sample of gas initially has a volume of 859 mL at 565 K and 2.20 atm. What pressure will the sample have if the volume changes to 268 mL while the temperature is increased to 815 K? A) 10.2 atm B) 9.83 atm C) 15.3 atm D) 6.53 atm E) 1.05 atm

10.2 atm

Using the following equation for the combustion of octane, calculate the amount of moles of oxygen that reacts with 100.0 g of octane. The molar mass of octane is 114.33 g/mole. The molar mass of carbon dioxide is 44.0095 g/mole. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ A) 18.18 moles B) 6.997 moles C) 14.00 moles D) 8.000 moles E) 10.93 moles

10.93 moles

What is the volume of 30.0 g of argon gas at 157°C and 2.50 kPa pressure? A) 3.87 L B) 10.6 L C) 393 L D) 1070 L

1070 L

How many grams of XeF6 are required to react with 0.579 L of hydrogen gas at 6.46 atm and 45°C in the reaction shown below? XeF6(s) + 3 H2(g) → Xe(g) + 6 HF(g) A) 9.58 g B) 11.7 g C) 35.2 g D) 106 g

11.7 g

Convert 1.50 atm to mm Hg. A) 760 mm Hg B) 875 mm Hg C) 1140 mm Hg D) 1000 mm Hg E) 1520 mm Hg

1140 mm Hg

Convert 1.50 atm to torr. A) 760 torr B) 875 torr C) 1140 torr D) 1000 torr E) 1520 torr

1140 torr

A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 629 torr. Use Charles's law to calculate the volume (L) the gas will occupy when the temperature is increased to while maintaining the pressure at 629 torr. A) 10.9 L B) 13.2 L C) 2.07 L D) 7.56 L E) 48.4 L

13.2 L

A cylinder filled with nitrogen gas at 80°C occupies 6.82 L at 12.00 atm. It is then quickly cooled to 5°C, and the pressure is measured at 4.82 atm. What is the new volume of the cylinder? A) 6.42 L B) 17.3 L C) 3.38 L D) 13.4 L

13.4 L

Determine the volume of O2 (at STP) formed when 50.0 g of KClO3 decomposes according to the following reaction. The molar mass for KClO3 is 122.55 g/mol. 2 KClO3(s) → 2 KCl(s) + 3 O2(g) A) 9.14 L B) 8.22 L C) 12.3 L D) 13.7 L E) 14.6 L

13.7 L

How many liters of hydrogen gas are needed to produce 100.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below? 2 H2(g) + O2(g) → 2 H2O(l) A) 67.9 L B) 136 L C) 203 L D) 407 L

136 L

A balloon contains 0.76 mol N2, 0.18 mol O2, 0.031 mol He and 0.026 mol H2 at 7 49 mm Hg. What is the partial pressure of O2? A) 20 mm Hg B) 23 mm Hg C) 140 mm Hg D) 570 mm Hg

140 mm Hg

For the reaction: NO(g) + 1/2 O2(g) → NO2(g) ΔH°rxn is -114.14 kJ/mol. Calculate ΔH°f of gaseous nitrogen monoxide, given that ΔH°f of NO2(g) is 33.90 kJ/mol. A) 148.0 kJ/mol B) 91.04 kJ/mol C) -114.1 kJ/mol D) 181.9 kJ/mol E) -35.64 kJ/mol

148.0 kJ/mol

The specific heat capacity of liquid mercury is 0.14 J/gK. How many joules of heat are needed to raise the temperature of 5.00 g of mercury from 15.0°C to 36.5°C? A) 7.7 × 102 J B) 15 J C) 36 J D) 0.0013 J E) 1.7 J

15 J

Which of the following samples will have the lowest pressure if they are all at the same temperature and in identical containers (same volume)? A) 15 g H2 B) 15 g Ar C) 15 g Kr D) 15 g CO2 E) All of these samples will have the same pressure.

15 g Kr

A 21.8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature rises from 25.0 to 62.3°C, determine the heat capacity of the calorimeter. The molar mass of ethanol is 46.07 g/mol. C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(g) ΔH°rxn = -1235 kJ A) 4.99 kJ/°C B) 5.65 kJ/°C C) 63.7 kJ/°C D) 33.1 kJ/°C E) 15.7 kJ/°

15.7 kJ/°

According to the following thermochemical equation, what mass of HF (in g) must react in order to produce 345 kJ of energy? Assume excess SiO2. SiO2(s) + 4 HF(g) → SiF4(g) + 2 H2O(l) ΔH°rxn = -184 kJ A) 42.7 g B) 37.5 g C) 150. g D) 107 g E) 173 g

150. g

Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction 4 SO3(g) → 4 S(s) + 6 O2(g) ΔH°rxn = ? Given: SO2(g) → S(s) + O2(g) ΔH°rxn = +296.8 kJ 2 SO2(g) + O2(g) → 2 SO3(g) ΔH°rxn = -197.8 kJ A) -494.6 kJ B) -692.4 kJ C) -791.4 kJ D) 1583 kJ E) -293.0 kJ

1583 kJ

Calculate the amount of heat (in kJ) required to raise the temperature of a 79.0 g sample of ethanol from 298.0 K to 385.0 K. The specific heat capacity of ethanol is 2.42 J/g°C. A) 57.0 kJ B) 16.6 kJ C) 73.6 kJ D) 28.4 kJ E) 12.9 kJ

16.6 kJ

Determine the mass of water formed when 12.5 L NH3 (at 298 K and 1.50 atm) is reacted with 18.9 L of O2 (at 323 K and 1.1 atm). 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) A) 17.0 g H2O B) 20.7 g H2O C) 37.7 g H2O D) 13.8 g H2O E) 27.9 g H2O

17.0 g H2O

What volume will 0.780 moles of Xe occupy at STP? A) 22.4 L B) 70.0 L C) 43.7 atm D) 17.5 L E) 15.6 L

17.5 L

How much heat is absorbed when 45.00 g of C(s) reacts in the presence of excess SO2(g) to produce CS2(l) and CO(g) according to the following chemical equation? 5 C(s) + 2 SO2(g) → CS2(l) + 4 CO(g) ΔH° = 239.9 kJ A) 179.8 kJ B) 239.9 kJ C) 898.5 kJ D) 2158 kJ

179.8 kJ

The mole fraction of argon in dry air near sea level is 1.818 × 10-5 where the molar mass of argon is 39.948. The concentration of argon in the atmosphere is ________ ppm. A) 1.07 × 108 B) 0.934 C) 9.34 × 106 D) 18.18 E) 9.34 × 109

18.18

How many liters of O2 gas at 25°C and 1.00 atm pressure are needed to react with 60.25 grams of potassium hydride according to the chemical equation shown below? 2 KH(s) + O2(g) → H2O(l) + K2O(s) A) 9.19 L B) 18.4 L C) 36.8 L D) 73.5 L

18.4 L

It takes 18.2 kJ of energy to raise the temperature of 55.2g of an unknown liquid from 30.0°C to 47.0°C. What is the specific heat of the unknown liquid A) 1. 17 J/(g ∙ °C) B) 205J/(g ∙ °C) C) 89.0 J/(g ∙ °C) D) 19.4 J/(g ∙ °C)

19.4 J/(g ∙ °C)

Using the following equation for the combustion of octane, calculate the heat of reaction for 400.0 g of octane. The molar mass of octane is 114.33 g/mole. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ A) 19280 kJ B) 19.28 kJ C) 38560 kJ D) 50400 kJ

19280 kJ

Choose the thermochemical equation that illustrates ΔH°f for Li2SO4. A) 2 Li+(aq) + SO42-(aq) → Li2SO4(aq) B) 2 Li(s) + 1/8 S8(s, rhombic) + 2 O2(g) → Li2SO4(s) C) Li2SO4(aq) → 2 Li+(aq) + SO42-(aq) D) 8 Li2SO4(s) → 16 Li(s) + S8(s, rhombic) + 16 O2(g) E) 16 Li(s) + S8(s, rhombic) + 16 O2(g) → 8 Li2SO4(s)

2 Li(s) + 1/8 S8(s, rhombic) + 2 O2(g) → Li2SO4(s)

For a process at constant pressure, 49,600 calories of heat are released. This quantity of heat is equivalent to A) 4.82 × 10-6 J. B) 1.19 × 104 J. C) 1.24 × 104 J. D) 2.08 × 105 J.

2.08 × 105 J.

The concentration of carbon monoxide in a sample of air is 9.2 ppm. There are ________ molecules of CO in 1.00 L of this air at 755 torr and 23°C. A) 3.8 × 10^-7 B) 2.2 × 10^21 C) 2.9 × 10^18 D) 1.7 × 10^20 E) 2.3 × 10^17

2.3 × 10^17

A mixture of Ar, Ne and He has a pressure of 7.85 atm. If the Ne has a mole fraction of 0.47 and He has a mole fraction of 0.23, what is the pressure of Ar? A) 4.2 atm B) 3.7 atm C) 1.8 atm D) 5.5 atm E) 2.4 atm

2.4 atm

The specific heat capacity of solid copper metal is 0.385 J/gK. How many joules of heat are needed to raise the temperature of a 1.55-kg block of copper from 33.0°C to 77.5°C? A) 1.79 × 10^5 J B) 26.6 J C) 2.66 × 10^4 J D) 5.58 × 10^-6 J E) 0.00558 J

2.66 × 10^4 J

A gas mixture consists of N2, O2, and Ne, where the mole fraction of N2 is 0.55 and the mole fraction of Ne is 0.25. If the mixture is at STP in a 5.0 L container, how many molecules of O2 are present? A) 4.5 × 1022 molecules O2 B) 2.7 × 1022 molecules O2 C) 3.7 × 1023 molecules O2 D) 1.1 × 1023 molecules O2 E) 9.3 × 1024 molecules O2

2.7 × 1022 molecules O2

How many molecules of XeF6 are formed from 12.9 L of F2 (at 298 K and 2.60 atm) according to the following reaction? Assume that there is excess Xe. Xe(g) + 3 F2(g) → XeF6(g) A) 1.21 × 1023 molecules XeF6 B) 8.25 × 1023 molecules XeF6 C) 2.75 × 1023 molecules XeF6 D) 7.29 × 1023 molecules XeF6 E) 1.37 × 1023 molecules XeF6

2.75 × 1023 molecules XeF6

A sample of copper absorbs 43.6 kJ of heat, resulting in a temperature rise of 40.0°C, determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J/g°C. A) 2.83 kg B) 9.93 kg C) 1.89 kg D) 11.9 kg E) 5.46 kg

2.83 kg

According to the following reaction, how much energy is required to decompose 59.0 kg of Fe3O4? The molar mass of Fe3O4 is 231.55 g/mol. Fe3O4(s) → 3 Fe(s) + 2 O2(g) ΔH°rxn = +1118 kJ A) 1.42 × 105 kJ B) 1.13 × 104 kJ C) 2.85 × 105 kJ D) 5.70 × 105 kJ E) 8.55 × 105 kJ

2.85 × 105 kJ

Calculate the amount of heat (in kJ) necessary to raise the temperature of 53.8 g benzene by 50.6 K. The specific heat capacity of benzene is 1.05 J/g°C. A) 1.61 kJ B) 16.6 kJ C) 2.59 kJ D) 2.86 kJ E) 3.85 kJ

2.86 kJ

What pressure will 2.6 × 1023 molecules of N2 exert in a 3.9 L container at 45°C? A) 5.7 atm B) 1.7 atm C) 2.9 atm D) 3.4 atm E) 4.6 atm

2.9 atm

Calculate the pressure of 4.55 moles of gas occupying 3.86 L at 213 K A) 15.8 atm B) 3.28 atm C) 20.6 atm D) 12.2 atm

20.6 atm

What is the total volume of hydrogen gas and oxygen gas that can be produced from the thermal decomposition of 0. 0425 grams of H2O2 at 700°C and 755 mm Hg according to the chemical equation shown below? H2O2(l) → H2(g) + O2(g) A) 50.2 mL B) 100 mL C) 151 mL D) 201 mL

201 mL

How many grams of Xe gas are present in a 21.00 L cylinder held at a pressure of 21.00 atm and 67.0°C? A) 2074 g B) 514.7 g C) 7361 g D) 8043 g

2074 g

Which of the following samples will have the greatest volume at STP? A) 22 g Ne B) 22 g He C) 22 g O2 D) 22 g Cl2 E) All of these samples would have the same volume at STP.

22 g He

When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M NaF, CaF2 precipitates, as shown in the net ionic equation below. The initial temperature of both solutions is 22.00°C. Assuming that the reaction goes to completion, and that the resulting solution has a mass of 100.00 g and a specific heat of 4.18 J/(g ∙ °C), calculate the final temperature of the solution. Ca2+(aq) + 2 F-(aq) → CaF2(s) ΔH° = -11.5 kJ A) 21.45°C B) 22.55°C C) 23.10°C D) 23.65°C

22.55°C

What is the total volume of the mixture of hydrogen gas and oxygen gas can be obtained from the electrolysis of 110.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below? 2 H2O(l) → 2 H2(g) + O2(g) A) 74.7 L B) 149 L C) 224 L D) 447 L

224 L

What is the Celsius temperature of 100.0 g of chlorine gas in a 55.0-L container at 800 mm Hg? A) -23°C B) 228°C C) 250°C D) 500°C

228°C

According to the following reaction, how much energy is evolved during the reaction of 32.5 g B2H6 and 72.5 g Cl2? The molar mass of B2H6 is 27.67 g/mol. B2H6(g) + 6 Cl2(g) → 2 BCl3(g) + 6 HCl(g)ΔH°rxn = -1396 kJ A) 1640 kJ B) 238 kJ C) 1430 kJ D) 3070 kJ E) 429 kJ

238 kJ

Convert 1.75 atm to psi. A) 52.4 psi B) 875 psi C) 25.7 psi D) 1000 psi E) 1330 psi

25.7 psi

Determine the theoretical yield and the percent yield if 21.8 g of K2CO3 is produced from reacting 27.9 g KO2 with 29.0 L of CO2 (at STP). The molar mass of KO2 = 71.10 g/mol and K2CO3 = 138.21 g/mol. 4 KO2(s) + 2 CO2(g) → 2 K2CO3(s) + 3 O2(g) A) 27.1 g, 80.4 % yield B) 179 g, 12.2 % yield C) 91.7 g, 23.8 % yield D) 206 g, 10.6 % yield E) 61.0 g, 35.7 % yield

27.1 g, 80.4 % yield

The atmospheric pressure is 700 mm Hg. What is the pressure in inches of Hg? A) 16.0 in Hg B) 0.921 in Hg C) 13.5 in Hg D) 27.6 in Hg E) 32.5 in Hg

27.6 in Hg

What is the volume of 0.700 mol of neon gas at a pressure of 609.5 mm Hg and 117°C? A) 0.0941 L B) 13.5 L C) 2.13 L D) 27.9 L E) 0.138 L

27.9 L

A 5.00-g sample of liquid water at 25.0 C is heated by the addition of 84.0 J of energy. The final temperature of the water is ________°C. The specific heat capacity of liquid water is 4.18J/gK A) 95.2 B) 25.2 C) -21.0 D) 29.0 E) 4.02

29.0

Determine the volume of H2S (at 375 K and 1.20 atm) needed to produce 55.0 g of S. Assume that there is excess SO2 present. 2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(g) A) 44.0 L B) 29.3 L C) 22.7 L D) 34.1 L E) 66.0 L

29.3 L

Determine the final temperature of a gold nugget (mass = 376 g) that starts at 398 K and loses 4.85 kJ of heat to a snowbank when it is lost. The specific heat capacity of gold is 0.128 J/g°C. A) 133 K B) 398 K C) 187 K D) 297 K E) 377 K

297 K

How many liters of hydrogen gas can be generated by reacting 9.25 grams of barium hydride with water at 20°C and 755 mm Hg pressure according to the chemical equation shown below? BaH2(s) + 2 H2O(l) → Ba(OH)2(aq) + 2 H2(g) A) 0. 219 L B) 0. 799 L C) 1.60 L D) 3.21 L

3.21 L

The density of chlorine gas at 1.21 atm and 34.9°C is ________ g/L. A) 0.0479 B) 0.295 C) 0.423 D) 1.70 E) 3.39

3.39

The density of krypton gas at 1.21 atm and 50.0°C is ________ g/L. A) 0.0456 B) 0.262 C) 0.295 D) 3.82 E) 7.65

3.82

How many grams of calcium hydride are required to produce 4.56 L of hydrogen gas at 25.0°C and 0.975 atm pressure according to the chemical equation shown below? CaH2(s) + 2 H2O(l) → Ca(OH)2(aq) + 2 H2(g) A) 3.82 g B) 7.64 g C) 15.3 g D) 45.6 g

3.82 g

Determine the specific heat capacity of an alloy that requires 59.3 kJ to raise the temperature of 150.0 g alloy from 298 K to 398 K. A) 4.38 J/g°C B) 2.29 J/g°C C) 3.95 J/g°C D) 2.53 J/g°C E) 1.87 J/g°

3.95 J/g°C

Using the following equation for the combustion of octane, calculate the amount of grams of carbon dioxide formed from 100.0 g of octane. The molar mass of octane is 114.33 g/mole. The molar mass of carbon dioxide is 44.0095 g/mole. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ A) 800.1 g B) 307.9 g C) 260.1 g D) 792.3 g

307.9 g

A piece of iron (mass = 25.0 g) at 398 K is placed in a styrofoam coffee cup containing 25.0 mL of water at 298 K. Assuming that no heat is lost to the cup or the surroundings, what will the final temperature of the water be? The specific heat capacity of iron = 0.449 J/g°C and water = 4.18 J/g°C. A) 348 K B) 308 K C) 287 K D) 325 K E) 388 K

308 K

A 50.0-g sample of liquid water at 25.0°C is mixed with 29.0 g of water at 45.0°C. The final temperature of the water is ________°C. A) 102 B) 27.6 C) 35.0 D) 142 E) 32.3

32.3

Determine the volume of SO2 (at STP) formed from the reaction of 96.7 g of FeS2 and 55.0 L of O2 (at 398 K and 1.20 atm). The molar mass of FeS2 is 119.99 g/mol. 4 FeS2(s) + 11 O2(g) → 2 Fe2O3(s) + 8 SO2(g) A) 36.1 L B) 45.3 L C) 18.1 L D) 27.6 L E) 32.9 L

32.9 L

At 1 atm pressure, the heat of sublimation of gallium is 277.0kJ/mol and the heat of vaporization is 271.0 kJ/mol. To the correct number of significant figures, how much heat is required to melt 5.50 mol of gallium at 1 atm pressure? A) 6 kJ B) 33 kJ C) 244 kJ D) 274 kJ

33 kJ

A gas is at 35.0°C and 3.50 L. What is the temperature at 7.00 L? A) 343°C B) 70.0°C C) 616°C D) 1.16°C E) 17.5°C

343°C

Calcium hydride (CaH2 ) reacts with water to form hydrogen gas: CaH2 (s) + 2H2O(l) → Ca(OH)2(aq) + 2H2(g) How many grams of CaH2 are needed to generate 48.0 L of H1 gas at a pressure of 0.888 atm and a temperature of 32°C? A) 50.7 B) 0.851 C) 143 D) 35.8 E) 71.7

35.8

A sample of N2 effuses in 220 s. How long will the same size sample of Cl2 take to effuse? A) 350 s B) 138 s C) 558 s D) 86.8 s E) 388 s

350 s

A 0.465 g sample of an unknown compound occupies 245 mL at 298 K and 1.22 atm. What is the molar mass of the unknown compound? A) 26.3 g/mol B) 33.9 g/mol C) 12.2 g/mol D) 38.0 g/mol E) 81.8 g/mol

38.0 g/mol

The specific heat of copper is 0.385 J/(g ∙ °C). If 34.2 g of copper, initially at 24.0°C, absorbs 4.689 kJ, what will be the final temperature of the copper? A) 24.4°C B) 26.8°C C) 356°C D) 380°C

380°C

What volume will a balloon occupy at 1.0 atm, if the balloon has a volume of 8.8 L at 4.4 atm? A) 2.0 L B) 0.50 L C) 39 L D) 13 L E) 4.4 L

39 L

How many grams of water are required to produce 5.50 L of hydrogen gas at 25.0°C and 755 mm Hg pressure according to the chemical equation shown below? BaH2(s) + 2 H2O(l) → Ba(OH)2(aq) + 2 H2(g) A) 2.01 g B) 4.02 g C) 4.07 g D) 8.04 g

4.02 g

What pressure (in atm) will 0.44 moles of CO2 exert in a 2.6 L container at 25°C? A) 0.35 atm B) 4.1 atm C) 4.7 atm D) 8.6 atm E) 3.6 atm

4.1 atm

What pressure will 14.0 g of CO exert in a 3.5 L container at 75°C? A) 4.1 atm B) 5.0 atm C) 6.4 atm D) 1.1 atm E) 2.3 atm

4.1 atm

A sample of air from a home is found to contain 6.2 ppm of carbon monoxide. This means that if the total pressure is 695 torr, then the partial pressure of CO is ________ torr. A) 4.3 × 10^3 B) 4.3 × 10^-3 C) 4.3 D) 8.9 × 10^3 E) 1.1 × 10^8

4.3 × 10^-3

The concentration of ozone in a sample of air that has a partial pressure of of 0.33 torr and a total pressure of air of 735 torr is ________ ppm. A) 4.5 × 10^2 B) 0.45 C) 0.045 D) 2.2 × 10^-3 E) 2.2

4.5 × 10^2

For a given set of conditions, a sample of 0.95 moles of Kr occupies 5.20 L. How many moles of Kr will occupy 24.8 L under the same conditions? A) 7.42 mol B) 0.0221 mol C) 10.5 mol D) 4.53 mol E) 3.58 mol

4.53 mol

When 14.0 g of zinc metal reacts with excess HCl, how many liters of H2 gas are produced at STP? A) 0.2 08 L B) 0. 416 L C) 4.80 L D) 9.60 L

4.80 L

The mole fraction of oxygen in dry air near sea level is 0.20948. The concentration of oxygen is ________ molecules per liter, assuming an atmospheric pressure of 739 torr and a temperature of 29.5°C. A) 6.23 B) 0.00819 C) 4.93 × 10^21 D) 3.75 × 10^24 E) 5.07 × 10^22

4.93 × 10^21

A 43.9-g piece of copper (CCu= 0.385 J/g°C) at 135.0°C is plunged into 254 g of water at 39.0°C. Assuming that no heat is lost to the surroundings, what will the final temperature of the system be? A) 100.0°C B) 40.5°C C) 62.5°C D) 87.0°C E) 53.1°C

40.5°C

How many grams of F2 gas are there in a 5.00-L cylinder at 4.00 × 103 mm Hg and 23°C? A) 19.5 g B) 41.1 g C) 500 g D) 2.96 × 104 g

41.1 g

A 0. 600 g sample containing Ag2O and inert material is heated, causing the silver oxide to decompose according to the following equation: 2 Ag2O(s) → 4 Ag(s) + O2(g) If 13.8 mL of gas are collected over water at 27°C and 1.00 atm external pressure, what is the percentage of silver oxide in the sample? The partial pressure of water is 26.7 mm Hg at 27°C. A) 10.4% B) 20.9% C) 41.8% D) 44.8%

41.8%

What volume of benzene (C6H6, d= 0.88 g/mL, molar mass = 78.11 g/mol) is required to produce 1.5 × 103 kJ of heat according to the following reaction? 2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(g) ΔH°rxn = -6278 kJ A) 75 mL B) 37 mL C) 21 mL D) 19 mL E) 42 mL

42 mL

How much heat is absorbed/released when 25.00 g of NH3(g) reacts in the presence of excess O2(g) to produce NO(g) and H2O(l) according to the following chemical equation? 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(l) ΔH° = 1168 kJ A) 428.6 kJ of heat are absorbed. B) 428.6 kJ of heat are released. C) 1715 kJ of heat are absorbed. D) 1715 kJ of heat are released.

428.6 kJ of heat are absorbed.

The specific heat capacity of methane gas is 2.20 J/g-K. How many joules of heat are needed to raise the temperature of 5.00 g of methane from 36.0°C to 75.0°C? A) 88.6 J B) 429 J C) 1221 J D) 0.0113 J E) 22.9 J

429 J

A large balloon is initially filled to a volume of 25.0 L at 353 K and a pressure of 2575 mm Hg. What volume of gas will the balloon contain at 1.35 atm and 253 K? A) 22.2 L B) 87.5 L C) 11.4 L D) 45.0 L E) 58.6 L

45.0 L

What pressure would a gas mixture in a 10.0 L tank exert if it were composed of 48.5 g He and 94.6 g CO2 at 398 K? A) 39.6 atm B) 7.02 atm C) 32.6 atm D) 46.6 atm E) 58.7 atm

46.6 atm

A 6.55 g sample of aniline (C6H5NH2, molar mass = 93.13 g/mol) was combusted in a bomb calorimeter with a heat capacity of 14.25 kJ/°C. If the initial temperature was 32.9°C, use the information below to determine the value of the final temperature of the calorimeter. 4 C6H5NH2(l) + 35 O2(g) → 24 CO2(g) + 14 H2O(g) + 4 NO2(g) ΔH°rxn = -1.28 × 104 kJ A) 257°C B) 46.6°C C) 48.7°C D) 41.9°C E) 931°C

48.7°C

A container filled with gas is connected to an open-end manometer that is filled with mineral oil. The pressure in the gas container is 753 mm Hg and atmospheric pressure is 724 mm. How high will the level rise in the manometer if the densities of Hg and mineral oil are 13.6 g/mL and 0.822 g/mL respectively? A) 1.75 mm B) 23.8 mm C) 29.0 mm D) 480 mm

480 mm

A 7.82 L gas cylinder contains 28.6 g of O2 and 79.5 g of Xe at 70°C. What is the pressure exerted by the gas? A) 1.10 atm B) 8.63 atm C) 6.92 atm D) 3.28 atm E) 5.41 atm

5.41 atm

What volume (in mL) will a sample of F2 gas occupy in a syringe at 5.5 atm, if the F2 has a volume of 25.0 mL at 1.2 atm? A) 11 mL B) 17 mL C) 3.8 mL D) 5.5 mL E) 7.6 mL

5.5 mL

To what volume will a sample of gas expand if it is heated from 50.0∘C and 2.33 L to 500.0°C? A) 5.58 L B) 23.3 L C) 0.233 L D) 0.97 L E) 0.184 L

5.58 L

How many grams of zinc metal are required to produce 2.00 liters of hydrogen gas at STP according to the chemical equation shown below? Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g) A) 0. 171 g B) 5.83 g C) 11.7 g D) 131 g

5.83 g

Which of the following (with specific heat capacity provided) would show the smallest temperature change upon gaining 200.0 J of heat? A) 50.0 g Al, CAl = 0.903 J/g°C B) 50.0 g Cu, CCu = 0.385 J/g°C C) 25.0 g granite, Cgranite = 0.79 J/g°C D) 25.0 g Au, CAu = 0.128 J/g°C E) 25.0 g Ag, CAg = 0.235 J/g°C

50.0 g Al, CAl = 0.903 J/g°C

Calculate the root mean square velocity of nitrogen molecules at 25°C. A) 729 m/s B) 515 m/s C) 149 m/s D) 297 m/s

515 m/s

What is the temperature of 100.8 g of N2 that exerts a pressure of 23.8 atm in a 6.51 L container? A) 524K B) 489K C) 778K D) 261K E) 340K

524K

A 1.000 kg sample of nitroglycerine, C3H5N3O9, explodes and releases gases with a temperature of 1985°C at 1. 100 atm. What is the volume of gas produced? 4 C3H5N3O9(s) → 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g) A) 742.2 L B) 3525 L C) 4730 L D) 5378 L

5378 L

How many milliliters of ozone gas at at 25.0°C and 1.00 atm pressure are needed to react with 45.00 mL of a 0. 100 M aqueous solution of KI according to the chemical equation shown below? O3(g) + 2 I-(aq) + H2O(l) → O2(g) + I2(s) + 2 OH-(aq) A) 55.0 mL B) 110. mL C) 165 mL D) 220. mL

55.0 mL

Determine the total volume of all gases (at STP) formed when 50.0 mL of TNT (C3H5(NO3)3, d = 1.60 g/mL, molar mass = 227.10 g/mol) reacts according to the following reaction. 4 C3H5(NO3)3(l) → 6 N2(g) + O2(g) + 12 CO2(g) + 10 H2O(g) A) 4.93 L B) 57.2 L C) 29.6 L D) 448 L E) 175 L

57.2 L

What is the temperature of 144.32 g of O2 found in a 5.00L container kept at a pressure of 3.28 atm assuming it behaves as a real gas? A) 44.3 K B) 57.5 K C) 102 K D) 219 K E) 328 K

57.5 K

According to the following reaction, how much energy is evolved during the reaction of 0.111 mol B2H6 and 0.252 mol Cl2 (Both gases are initially at STP)? The molar mass of B2H6 is 27.67 g/mol. B2H6(g) + 6 Cl2(g) → 2 BCl3(g) + 6 HCl(g) ΔH°rxn = -1396 kJ A) 58.7 kJ B) 156 kJ C) 215 kJ D) 352 kJ E) 508 kJ

58.7 kJ

A 6.50-g sample of copper metal at 25.0°C is heated by the addition of 84.0 J of energy. The final temperature of the copper is ________°C. The specific heat capacity of copper is 0.38J/gK A) 29.9 B) 25.0 C) 9.0 D) 59.0 E) 34.0

59.0

A 6.55 g sample of aniline (C6H5NH2, molar mass = 93.13 g/mol) was combusted in a bomb calorimeter. If the temperature rose by 32.9°C, use the information below to determine the heat capacity of the calorimeter. 4 C6H5NH2(l) + 35 O2(g) → 24 CO2(g) + 14 H2O(g) + 4 NO2(g) ΔH°rxn = -1.28 × 104 kJ A) 97.3 kJ/°C B) 38.9 kJ/°C C) 5.94 kJ/°C D) 6.84 kJ/°C E) 12.8 kJ/°C

6.84 kJ/°C

Using the following equation for the combustion of octane, calculate the amount of moles of carbon dioxide formed from 100.0 g of octane. The molar mass of octane is 114.33 g/mole. The molar mass of carbon dioxide is 44.0095 g/mole. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ A) 18.18 moles B) 6.997 moles C) 14.00 moles D) 8.000 moles E) 10.93 moles

6.997 moles

What is the average speed (actually the root-mean-square speed) of a neon atom at 27°C? A) 5.78 m/s B) 19.3 m/s C) 183 m/s D) 609 m/s

609 m/s

Calculate the temperature, in K, of 2.20 moles of gas occupying 3.30 L at 3.50 atm. A) 64.0 K B) -209 K C) 337 K D) 28.0 K

64.0 K

What is the pressure in a gas container that is connected to an open-end U-tube manometer if the pressure of the atmosphere is 742 torr and the level of mercury in the arm connected to the container is 8.60 cm higher than the level of mercury open to the atmosphere? A) 656 mm Hg B) 733 mm Hg C) 751 mm Hg D) 828 mm Hg

656 mm Hg

How many liters of oxygen are needed to react with 2.878 g of octane at STP? 2C8H18(g) + 25O2(g) → 16CO2(g) +18H2O(g) A) 8.21 L B) 7.04 L C) 6.72 L D) 7.68 L

7.04 L

What is the volume of 9.783 × 1023 atoms of Kr at 9.25 atm and 512K? A) 7.38 L B) 3.69 L C) 1.85 L D) 15.4 L E) 30.8 L

7.38 L

The action of some commercial drain cleaners is based on the following reaction: 2 NaOH(s) + 2 Al(s) + 6 H2O(l) → 2 NaAl(OH)4(s) + 3 H2(g) What is the volume of H2 gas formed at STP when 6.32 g of Al reacts with excess NaOH? A) 3.50 L B) 5.25 L C) 7.87 L D) 8.59 L

7.87 L

A 0. 286-g sample of gas occupies 125 mL at 60. cm of Hg and 25°C. What is the molar mass of the gas? A) 5.9 g/mol B) 44 g/mol C) 59 g/mol D) 71 g/mol

71 g/mol

The atmospheric pressure is 715 mm Hg. What is the pressure in torr? A) 715 torr B) 28.1 torr C) 13.8 torr D) 31.8 torr E) 760 torr

715 torr

How much energy is evolved during the formation of 98.7 g of Fe, according to the reaction below? Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn = -852 kJ A) 753 kJ B) 1.51 × 103 kJ C) 4.20 × 103 kJ D) 482 kJ E) 241 kJ

753 kj

How many liters of oxygen gas can be produced at STP from the decomposition of 0.250 L of 3.00 M H2O2 in the reaction according to the chemical equation shown below? 2H2O2(l) -> 2H2O(l) + O2(g) A) 8.41 L B) 11.2 L C) 16.8 L D) 33.6 L

8.41 L

If a sample of 0.29 moles of Ar occupies 3.8 L under certain conditions, what volume will 0.66 moles occupy under the same conditions? A) 12 L B) 8.6 L C) 17 L D) 5.0 L E) 15 L

8.6 L

How much energy is evolved during the reaction of 51.2 g of Al, according to the reaction below? Assume that there is excess Fe2O3. Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn = -852 kJ A) 51.2 kJ B) 448 kJ C) 224 kJ D) 1617 kJ E) 808 kJ

808 kJ

A 55.0-L steel tank at 20.0°C contains acetylene gas, C2H2, at a pressure of 1.39 atm. Assuming ideal behavior, how many grams of acetylene are in the tank? A) 3.17 g B) 8.20 g C) 82.9 g D) 1210 g

82.9 g

The specific heat capacity of liquid water is 4.18 J/g-K. How many joules of heat are needed to raise the temperature of 5.00 g of water from 25.1°C to 65.3°C? A) 48.1 J B) 840 J C) 1.89 × 10^3 J D) 2.08 × 10^-2 J E) 54.4 J

840 J

A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 667 torr. Use Boyle's law to calculate the pressure (torr) when the volume is reduced to 7.88 L at a constant temperature of 25.0°C. A) 846 torr B) 0.118 torr C) 5.26 × torr D) 526 torr E) 1.11 torr

846 torr

A 12.8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity of 5.65 kJ/°C. Using the information below, determine the final temperature of the calorimeter if the initial temperature is 25.0°C. The molar mass of ethanol is 46.07 g/mol. C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(g) ΔH°rxn = -1235 kJ A) 53.4°C B) 28.1°C C) 111°C D) 85.7°C E) 74.2°C

85.7°C

What mass of NO2 is contained in a 13.0 L tank at 4.58 atm and 385 K? A) 18.8 g B) 53.1 g C) 24.4 g D) 86.7 g E) 69.2 g

86.7 g

To what temperature must a balloon, initially at 25°C and 2.00 L, be heated in order to have a volume of 6.00 L? A) 993 K B) 403 K C) 75 K D) 655 K E) 894 K

894 K

How many mL of O2 gas at 25°C and 755 mm Hg pressure can be produced from the thermal decomposition of 0. 300 grams of KClO3(s) according to the chemical equation shown below? 2 KClO3(s) → 2 KCl(s) + 3 O2(g) A) 30.1 mL B) 40.2 mL C) 90.4 mL D) 181 mL

90.4 mL

What volume of water is produced when 38.5 g of ethanol reacts with oxygen at 500°C at 1.75 atm? CH3CH2OH(g) + 3 O2(g)→ 2 CO2(g) + 3 H2O(g) A) 91.0 L B) 58.7 L C) 103 L D) 30.3 L E) 12.5 L

91.0 L

If a block of gold requires 1.42 kJ of energy to raise the temperature from 120.0°C to 240.0°C, what is the mass of the block? The specific heat capacity of gold is 0.129 J/g-K. A) 92.0 g B) 35.3 g C) 186 g D) 55.7 g

92.0 g

According to the following thermochemical equation, what mass of H2O (in g) must form in order to produce 488 kJ of energy? SiO2(s) + 4 HF(g) → SiF4(g) + 2 H2O(l) ΔH°rxn = -184 kJ A) 34.0 g B) 51 g C) 27.1 g D) 95.4 g E) 47.8 g

95.4 g

Using the following thermochemical equation, determine the amount of heat produced from the combustion of 24.3 g benzene (C6H6). The molar mass of benzene is 78.11 g/mole. 2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(g) ΔH°rxn = -6278 kJ A) 3910 kJ B) 1950 kJ C) 977 kJ D) 40.1 kJ E) 0.302 kJ

977 kJ

How much heat energy is required to raise the temperature of 0.298 mole of water from 35.93°C to 79.84°C? The specific heat capacity of water = 4.18 J/g°C. A) 13.1 J B) 54.7 J C) 985 J D) 2105 J E) 3310 J

985 J

A student is preparing to perform a series of calorimetry experiments. She first wishes to determine the calorimeter constant (Ccal) for her coffee cup calorimeter. She pours a 50.0 mL sample of water at 345 K into the calorimeter containing a 50.0 mL sample of water at 298 K. She carefully records the final temperature of the water as 317 K. What is the value of Ccal for the calorimeter? A) 19 J/K B) 28 J/K C) 99 J/K D) 21 J/K E) 76 J/K

99 J/K

Three identical flasks contain three different gases at standard temperature and pressure. Flask A C2H4 contains flask B contains O3, and flask C contains F2. Which flask contains the largest number of molecules? A) flask A B) flask B C) flask C D) All contain same number of molecules.

All contain same number of molecules.

Which of the following statements is TRUE? A) State functions do not depend on the path taken to arrive at a particular state. B) DErxn can be determined using constant volume calorimetry. C) Energy is neither created nor destroyed, excluding nuclear reactions. D) ΔHrxn can be determined using constant pressure calorimetry. E) All of the above are true

All of the above are true

Which of the following gas samples would be most likely to behave ideally under the stated conditions? A) Ar at STP B) CO at 200 atm and 25°C C) SO2 at 2 atm and 0 K D) N2 at 1 atm and -70°C E) H2 at 400 atm and 25°C

Ar at STP

Which of the following statements is TRUE? A) At a given temperature, lighter gas particles travel more slowly than heavier gas particles. B) The smaller a gas particle, the slower it will effuse. C) The higher the temperature, the lower the average kinetic energy of the sample. D) At low temperatures, intermolecular forces become important and the pressure of a gas will be lower than predicted by the ideal gas law. E) None of the above statements are true

At low temperatures, intermolecular forces become important and the pressure of a gas will be lower than predicted by the ideal gas law.

Which of the following statements is TRUE? A) Particles of different masses have the same average speed at a given temperature. B) The larger a molecule, the faster it will effuse. C) At very high pressures, a gas will occupy a larger volume than predicted by the ideal gas law. D) For a given gas, the lower the temperature, the faster it will effuse. E) None of the above statements are true.

At very high pressures, a gas will occupy a larger volume than predicted by the ideal gas law.

The volume of a gas is proportional to number of moles of a gas is known as A) Avogadro's Law. B) Ideal Gas Law. C) Charles's Law. D) Boyle's Law. E) Dalton's Law.

Avogadro's Law.

A mixture of 1.0 mol He and 1.0 mol Ne are at STP in a rigid container. Which of the following statements is TRUE? A) Both gases have the same average kinetic energy. B) Both gases contribute equally to the density of the mixture under these conditions. C) Both gases have the same molecular speed. D) The mixture has a volume of 22.4 L E) All of the above are true.

Both gases have the same average kinetic energy.

The volume of a gas is inversely proportional to the pressure of a gas is known as A) Avogadro's Law. B) Ideal Gas Law. C) Charles's Law. D) Boyle's Law. E) Dalton's Law.

Boyle's Law.

Which of the following processes are exothermic? A) Cl2(g) → 2Cl(g) B) Br(g) + e⁻ → Br⁻(g) C) Li(s) → Li(g) D) NaF(s) → Na⁺(g) + F⁻(g) E) None of the above are exothermic.

Br(g) + e⁻ → Br⁻(g

Identify a substance that is in its standard state. A) N2(l) B) Cu(g) C) Cl D) He2 E) Br(l)

Br(l)

Which one of the following elements is NOT in its standard state? A) Br2(g) B) F2(g) C) Hg(l) D) Na(s) E) Cl2(g)

Br2(g)

The density of an unknown gas at 320K is 3.97 g/L and exerts a pressure of 1.80 atm in a cylinder. What is the gas? A) F2 B) C4H10 C) Cl2 D) C2H2

C4H10

Which of the following samples will have the greatest average speed at 355 K? A) Kr B) C2H4 C) Cl2 D) CH4 E) All of these samples will have the same average speed at the same temperature.

CH4

Identify the gas particle that travels the slowest. A) H2 B) O2 C) Ne D) F2 E) CO

CO

Identify an element that is NOT in its standard state. A) CO(g) B) Ba(s) C) H2(g) D) O2(g) E) Ne(g)

CO(g)

Give the gas that is the lowest percent by volume in dry gas. A) CO2 B) He C) H2 D) N2

CO2

Which of the following processes are endothermic? A) K⁺(g) + I⁻(g) → KI(s) B) 2 Br(g) → Br2(g) C) Ca(s) → Ca(g) D) 2 Na(s) + O2(g) → Na2O(s) E) None of the above are endothermic

Ca(s) → Ca(g)

The volume of a gas is proportional to the temperature of a gas is known as A) Avogadro's Law. B) Ideal Gas Law. C) Charles's Law. D) Boyle's Law. E) Dalton's Law

Charles's Law

A 0.334 g sample of an unknown halogen occupies 109 mL at 398 K and 1.41 atm. What is the identity of the halogen? A) Br2 B) F2 C) Cl2 D) I2 E) Ge

Cl2

The density of a gas is 3.16 g/L at STP. What is the gas? A) H2 B) Br2 C) Kr D) Cl2 E) Ar

Cl2

Choose the reaction that illustrates ΔH°f for CsHCO3. A) Cs(s) + H2(g) + C(s) + O2(g) → CsHCO3(s) B) Cs+(aq) + HCO3 -1(aq) → CsHCO3(s) C) Cs+(aq) + H2O(l) + CO2(g) → CsHCO3(s) D) Cs(s) + 1/2 H2(g) + C(s) + 3/2 O2(g) → CsHCO3(s) E) Cs(s) + 2 H(g) + C(s) + 3 O(g) → CsHCO3(s)

Cs(s) + 1/2 H2(g) + C(s) + 3/2 O2(g) → CsHCO3(s)

The total pressure of a gas mixture is the sum of the partial pressure of its components is known as A) Avogadro's Law. B) Ideal Gas Law. C) Charles's Law. D) Boyle's Law. E) Dalton's Law.

Dalton's Law.

Which of the following gases has the largest density at STP? A) He B) C2H2 C) F2 D) N2 E) H2

F2

Which of the following is NOT a standard state? A) For a liquid, it is 25°F. B) For a solid, it is 25° C. C) For a solid, it is 1 atm. D) For a solution, it is 1 M. E) For a liquid, it is 1 atm.

For a liquid, it is 25°F.

Which of the following is NOT a standard state? A) For a solid, it is 25°F. B) For a liquid, it is 25°C. C) For a gas, it is 1 atm. D) For a solution, it is 1 M. E) For a liquid, it is 1 atm.

For a solid, it is 25°F

Give the definition for diffusion. A) Gas molecules mix equally. B) Gas molecules spread out in a concentration gradient. C) Gas molecules escape from a container into a vacuum through a small hole. D) average distance between collisions E) Gas molecules mix unequally.

Gas molecules spread out in a concentration gradient.

The rate of effusion of two different gases is known as A) Avogadro's Law. B) Graham's Law. C) Charles's Law. D) Boyle's Law. E) Dalton's Law.

Graham's Law

Identify a substance that is NOT in its standard state. A) O2 B) Zn C) H D) O3 E) Xe

H

Identify the gas particle that travels the fastest. A) H2 B) N2 C) Ne D) Cl2 E) CO

H2

Rank the following in order of decreasing rate of effusion. F2 SF6 He Ar A) SF6 > Ar > F2 > He B) Ar > He > SF6 > F2 C) F2 > Ar > He > SF6 D) He > F2 > Ar > SF6 E) He > F2 > SF6 > Ar

He > F2 > Ar > SF6

Give the units of specific heat capacity. A) J/°C B) J/g °C C) Jmole °C D) g/°C E) gmole °C

J/g °C

Give the units of heat capacity. A) J/°C B) J/g °C C) Jmole/°C D) g/°C E) mole/°C

J/°C

Which of the following statements about energy is FALSE? A) Energy can be converted from one type to another. B) The total energy of a system remains constant. C) Kinetic energy is the energy associated with its position or composition. D) Energy is the capacity to do work. E) Systems tend to change in order to lower their potential energy.

Kinetic energy is the energy associated with its position or composition.

Which of the following gases has the lowest average speed at 25°C? A) C3H8 B) Kr C) CH3NH2 D) SO2

Kr

Choose the reaction that illustrates ΔH°f for Mg(NO3)2. A) Mg(s) + N2(g) + 3O2(g) → Mg(NO3)2(s) B) Mg2+(aq) + 2 NO3-(aq) → Mg(NO3)2(aq) C) Mg(s) + 2 N(g) + 6 O(g) → Mg(NO3)2(s) D) Mg(NO3)2(aq) → Mg2+(aq) + 2 NO3-(aq) E) Mg(NO3)2(s) → Mg(s) + N2(g) + 3O2(g)

Mg(s) + N2(g) + 3O2(g) → Mg(NO3)2(s)

Which compound should have the largest lattice energy? A) SrI2 B) CaCl2 C) NaI D) MgO E) KF

MgO

The rate of effusion of oxygen to an unknown gas is 0.935. What is the other gas? A) Ne B) Ar C) F2 D) N2

N2

Which of the following gases has the highest average speed at 400K? A) N2 B) O2 C) F2 D) Cl2

N2

A compound is found to be 30.45% N and 69.55 % O by mass. If 1.63 g of this compound occupy 389 mL at 0.00°C and 775 mm Hg, what is the molecular formula of the compound? A) NO2 B) N2O C) N4O2 D) N2O5 E) N2O4

N2O4

Place the following gases in order of increasing density at STP. F2 NH3 N2O4 Ar A) N2O4 < Ar < F2 < NH3 B) Ar < N2O4 < F2 < NH3 C) F2 < Ar < N2O4 < NH3 D) NH3 < F2 < Ar < N2O4 E) Ar < F2 < NH3 < N2O4

NH3 < F2 < Ar < N2O4

A sample of 1.58 g of an unknown gas has a volume of 0.682 L. The sample is kept at 60°C, and exerts a pressure of 1.38 atm. What is the gas? A) Cl2 B) NO C) NO2 D) SO2 E) C2H6

NO2

Two aqueous solutions are both at room temperature and are then mixed in a coffee cup calorimeter. The reaction causes the temperature of the resulting solution to fall below room temperature. Which of the following statements is TRUE? A) The products have a lower potential energy than the reactants. B) This type of experiment will provide data to calculate ΔErxn. C) The reaction is exothermic. D) Energy is leaving the system during reaction. E) None of the above statements are true.

None of the above statements are true

Which of the following would have a density of 1.37 g/L at 7.0°C and 0.987 atm? A) N2 B) O2 C) Kr D) Rn

O2

If 2.0 mol of gas A is mixed with 1.0 mol of gas B to give a total pressure of 1.6 atm, what is the partial pressure of gas A and B? A) PA = 0.33 atm and PB = 0.67 atm B) PA = 0.67 atm and PB = 0.33 atm C) PA = 1.0 atm and PB = 2.0 atm D) PA = 2.0 atm and PB = 1.0 atm E) PA = 1.06 atm and PB = 0.53 atm

PA = 1.06 atm and PB = 0.53 atm

Which of the following samples has the greatest density at STP? A) NO2 B) Xe C) SO2 D) SF6 E) All of these samples have the same density at STP.

SF6

Which of the following compounds will behave LEAST like an ideal gas at low temperatures? A) He B) SO2 C) H2 D) N2 E) F2

SO2

Arrange the gases according to increasing rate of diffusion at 50°C. A) NO2 < O2 < SO2 B) O2 < NO2 < SO2 C) O2 < SO2 < NO2 D) SO2 < O2 < NO2 E) SO2 < NO2 < O2

SO2 < NO2 < O2

A piece of iron (C=0.449 J/g°C) and a piece of gold (C=0.128 J/g°C) have identical masses. If the iron has an initial temperature of 488 K and the gold has an initial temperature of 308 K, which of the following statements is TRUE of the outcome when the two metals are placed in contact with one another? Assume no heat is lost to the surroundings. A) Since the two metals have the same mass, the final temperature of the two metals will be 398 K, exactly halfway between the two initial temperatures. B) Since the two metals have the same mass, but the specific heat capacity of gold is much smaller than that of iron, the final temperature of the two metals will be closer to 308 K than to 488 K. C) Energy will flow from the gold to the iron until the two metals are at the same temperature. D) Since the two metals have the same mass, the thermal energy contained in each metal after equilibrium will be the same. E) None of the above are true.

Since the two metals have the same mass, the thermal energy contained in each metal after equilibrium will be the same

Which statement is TRUE about kinetic molecular theory? A) A single particle does not move in a straight line. B) The size of the particle is large compared to the volume of the particle. C) The collisions of particles with one another is completely elastic. D) The average kinetic energy of a particle is not proportional to the temperature.

The collisions of particles with one another is completely elastic.

Which one of the following statements is NOT true concerning the equation below? N2(g) + 3 H2(g) → 2 NH3(g) ΔH°rxn = -459.0 kJ A) The production of 1.00 mole of ammonia is accompanied by the production of 229.5 kJ of heat. B) The complete reaction of 1.00 moles of nitrogen requires 459 kJ of heat. C) The complete reaction of 1.00 moles of hydrogen produces 153 kJ of heat. D) The complete reaction of 0.8278 moles of hydrogen requires 0.2759 moles of nitrogen. E) The reaction is exothermic.

The complete reaction of 1.00 moles of nitrogen requires 459 kJ of heat.

Which of the following is TRUE if ΔEsys = - 115 J? A) The system is gaining 115 J, while the surroundings are losing 115 J. B) The system is losing 115 J, while the surroundings are gaining 115 J. C) Both the system and the surroundings are gaining 115 J. D) Both the system and the surroundings are losing 115 J. E) None of the above are true.

The system is losing 115 J, while the surroundings are gaining 115 J.

Which of the following processes is exothermic? A) a candle flame B) baking bread C) the chemical reaction in a "cold pack" often used to treat injuries D) the vaporization of water E) None of the above are exothermic

a candle flame

In a bomb calorimeter, reactions are carried out A) at fixed pressure. B) at fixed volume. C) at fixed temperature. D) with solids only. E) using water as a solvent.

at fixed volume.

An instrument used to measure atmospheric pressure is called a A) barometer. B) manometer. C) sphygmomanometer. D) spectrophotometer. E) spectrometer.

barometer

If the pressure in a gas container that is connected to an open-end U-tube manometer is 116 kPa and the pressure of the atmosphere at the open end of the tube is 752 mm Hg, the level of mercury in the tube will A) be 118 mm higher in the arm open to the atmosphere. B) be 118 mm higher in the arm connected to the gas cylinder. C) be 870 mm higher in the arm open to the atmosphere. D) be 870 mm higher in the arm connected to the gas cylinder.

be 118 mm higher in the arm open to the atmosphere.

Given three cylinders containing O2 gas at the same volume and pressure. Cylinder A is at 15°C, cylinder B is at -5°F, cylinder C is at 255 K. Which cylinder contains the largest mass of oxygen? A) cylinder A B) cylinder B C) cylinder C D) All cylinders contain the same mass of O2.

cylinder B

Define kinetic energy A) energy associated with the temperature of an object B) energy associated with the motion of an object C) energy associated with the force of an object D) energy associated with the gravity of an object E) energy associated with the position or composition of an object

energy associated with the motion of an object

Define potential energy. A) energy associated with the temperature of an object B) energy associated with the motion of an object C) energy associated with the force of an object D) energy associated with the gravity of an object E) energy associated with the position or composition of an object

energy associated with the position or composition of an object

Define thermal energy A) energy associated with the temperature of an object B) energy associated with the motion of an object C) energy associated with the force of an object D) energy associated with the gravity of an object E) energy associated with the position or composition of an object

energy associated with the temperature of an object

A scuba diver experiences ________ as she descends into the ocean water. A) decrease of 1 atm for each 20 m of depth B) decrease of 1 atm for each 10 m of depth C) increase of 1 atm for each 20 m of depth D) increase of 1 atm for each 10 m of depth E) no difference in pressure

increase of 1 atm for each 10 m of depth

A sample of nitrogen gas is placed in a sealed chamber, and the temperature is increased from 25°C to 125°C under constant pressure. The volume of the sample must A) increase. B) decrease. C) remain constant. D) None of these are possible.

increase.

Which of the following will cause the volume of an ideal gas to triple in value? A) raising the temperature from 25°C to 75°C at constant pressure B) lowering the absolute temperature by a factor of 3 at constant pressure C) raising the absolute temperature by a factor of 3 while increasing the pressure by a factor of 3 D) lowering the absolute temperature by a factor of 3 while increasing the pressure by a factor of 3 E) lowering the pressure by a factor of 3 while the temperature stays constant

lowering the pressure by a factor of 3 while the temperature stays constant

An instrument used to measure the pressure of a gas in a laboratory is called a A) barometer. B) manometer. C) sphygmomanometer. D) spectrophotometer. E) spectrometer.

manometer.

Identify what a bomb calorimeter measures. A) measures ΔH for aqueous solutions B) measures ΔE for combustion reactions C) measures ΔH for reduction solutions D) measures ΔT for aqueous solutions E) measures ΔE for oxidation reactions

measures ΔE for combustion reactions

Which of the following processes is endothermic? A) mixing water and acid B) rusting iron C) photosynthesis D) the electron affinity of a fluorine atom E) None of the above processes are endothermic.

photosynthesis

Which of the following signs on q and w represent a system that is doing work on the surroundings, as well as gaining heat from the surroundings? A) q = +, w = - B) q = -, w = + C) q = +, w = + D) q = -, w = - E) None of these represent the system referenced above

q = +, w = -

The law of ________ states that energy that can be neither created or destroyed. A) kinetic energy B) the consecration of energy C) potential energy D) the conservation of energy E) thermochemistry

the conservation of energy

Which of the following processes are exothermic? A) the second ionization energy of Mg B) the sublimation of Li C) the breaking the bond of I2 D) the formation of NaBr from its constituent elements in their standard state E) None of the above are exothermic.

the formation of NaBr from its constituent elements in their standard state

Define heat capacity. A) the quantity of heat required to lower the temperature of 1 mole of a substance by 1°C B) the quantity of heat required to change a system's temperature by 1°C C) the quantity of heat required to lower the temperature of 1 gram of a substance by 1°C D) the quantity of heat required to raise the temperature of 1 g of a substance by 1°F E) the quantity of heat required to lower the temperature of 1 liter of a substance by 1°C

the quantity of heat required to change a system's temperature by 1°C

6) Define specific heat capacity. A) the quantity of heat required to lower the temperature of 1 mole of a substance by 1°C B) the quantity of heat required to change a system's temperature by 1°C C) the quantity of heat required to raise the temperature of 1 gram of a substance by 1°C D) the quantity of heat required to lower the temperature of 1 gram of a substance by 1°F E) the quantity of heat required to lower the temperature of 1 liter of a substance by 1°

the quantity of heat required to raise the temperature of 1 gram of a substance by 1°C

Define molar heat capacity. A) the quantity of heat required to raise the temperature of 1 mole of a substance by 1°C B) the quantity of heat required to change a system's temperature by 1°C C) the quantity of heat required to raise the temperature of 1 gram of a substance by 1°C D) the quantity of heat required to lower the temperature of 1 g of a substance by 1°F E) the quantity of heat required to lower the temperature of 1 liter of a substance by 1°C

the quantity of heat required to raise the temperature of 1 mole of a substance by 1°C

Which of the following processes is exothermic? A) the ionization of a potassium atom B) the breaking of a Br-Br bond C) the sublimation of dry ice (CO2(s)) D) the reaction associated with DH°f for an ionic compound E) All of the above processes are exothermic.

the reaction associated with DH°f for an ionic compound

This equation is used to calculate the properties of a gas under nonideal conditions. A) Charles's Law B) Avogadro's Law C) Boyle's Law D) van der Waals equation E) Dalton's Law

van der Waals equation

A 1.44-g sample of an unknown pure gas occupies a volume of 0.335 L at a pressure of 1.00 atm and a temperature of 100.0°C. The unknown gas is A) argon B) helium C) krypton D) neon E) xenon

xenon

For a particular process that is carried out at constant pressure, q = 145 kJ and w = -35 kJ. Therefore A) ΔE = 110 kJ and ΔH = 145 kJ. B) ΔE = 145 kJ and ΔH = 110 kJ. C) ΔE = 145 kJ and ΔH = 180 kJ. D) ΔE = 180 kJ and ΔH = 145 kJ

ΔE = 110 kJ and ΔH = 145 kJ

When 5.00 mol of benzene is vaporized at a constant pressure of 1.00 atm and at its normal boiling point of 80.1°C, 169.5 kJ are absorbed and PΔV for the vaporization process is equal to 14.5 kJ then A) ΔE = 155.0 kJ and ΔH = 169.5 kJ. B) ΔE = 184.0 kJ and ΔH = 169.5 kJ. C) ΔE = 169.5 kJ and ΔH = 184.0 kJ. D) ΔE = 169.5 kJ and ΔH = 155.0 kJ.

ΔE = 155.0 kJ and ΔH = 169.5 kJ.

Which statement is FALSE? A) An exothermic reaction gives heat off heat to the surroundings. B) Enthalpy is the sum of a system's internal energy and the product of pressure and volume change. C) ΔErxn is a measure of heat. D) ΔHrxn is the heat of reaction. E) Endothermic has a positive ΔH

ΔErxn is a measure of heat.

When 10.00 moles of H2(g) reacts with 5.000 mol of O2(g) to form 10.00 mol of H2O(l) at 25°C and a constant pressure of 1.00 atm. If 683.0 kJ of heat are released during this reaction, and PΔV is equal to -37.00 kJ, then A) ΔH° = +683.0 kJ and ΔE° = +720.0 kJ. B) ΔH° = +683.0 kJ and ΔE° = +646.0 kJ. C) ΔH° = -683.0 kJ and ΔE° = -646.0 kJ. D) ΔH° = -683.0 kJ and ΔE° = -720.0 kJ

ΔH° = -683.0 kJ and ΔE° = -646.0 kJ