CHEM 101 FINal

Use the following information to determine the enthalpy for the reaction shown below. CS2(l) 3O2(g) CO2(g) 2SO2(g) /\H = ? C(graphite) O2(g) CO2(g) /\H =-393.5 kJ S(s) O2(g) SO2(g) /\H =-296.8 kJ C(graphite) 2S(s) CS2(l) /\H= 87.9 kJ a. -1075 kJ d. +778 kJ b. +1075 kJ e. -602 kJ c. -778 kj

A

Water can be separated into its elements according to the following equation. If 20.0 g of water is decomposed by this method, how much oxygen gas is produced? 2H2O(l) 2H2(g) O2(g) a. 17.8 g d. 16.0 g b. 8.9 g e. 10.0 g c. 35.6 g

A

What are the units of molar concentration, M ? a. mol/L d. ppm b. g/L e. mol/mL c. mol/kg

A

What is the molar mass of a gas that has a density of 2.62 g/L at 2.00 atm and 25.0C? a. 32.0 g/mol d. 28.0 g/mol b. 16.0 g/mol e. 2.69 g/mol c. 64.0 g/mol

A

When solid sodium hydroxide (NaOH) pellets are dissolved in water, the temperature of the water and beaker rises. This is an example of ________ a. an exothermic process. d. a thermodynamic cycle. b. an endothermic process. e. all solvation processes. c. a combustion reaction.

A

Which one of the following is a mixture? a. an aqueous solution of sugar d. copper metal b. pure water e. table salt (sodium chloride) c. nitrogen gas

A

Which one of the following is not a physical process or change? a. natural gas burning d. iodine vaporizing b. water boiling e. alcohol evaporating c. ice melting

A

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

E

What is the correct formula for the compound formed between potassium and phosphorus based on their positions in the periodic table? a. K2P d. K2P2 b. KP2 e. K3P c. KP

E

What is the oxidation number of S in H2SO4? a. +2 d. -6 b. -4 e. +6 c. +4

E

What mass of barium sulfate (molar mass = 233 g/mol) is produced when 125 mL of a 0.150 M solution of barium chloride is mixed with 125 mL of a 0.150 M solution of iron(III) sulfate? a. 7.59 g d. 18.8 g b. 3.65 g e. 4.37 g c. 13.1 g

E

What volume of 12 M HCl solution needs to be diluted to produce 275 mL of 2.1 M HCl solution? a. 1.8 mL d. 23 mL b. 9.2 mL e. 48 mL c. 5.7 mL

E

Which of the following compounds is a strong electrolyte? a. methane, CH4 d. hydrofluoric acid, HF b. methanol, CH3OH e. potassium chloride, KCl c. ammonia, NH3

E

Which one of the following statements regarding a strong acid is not correct? a. A strong acid ionizes completely in water. b. A strong acid ionizes in water to produce H+. c. A strong acid neutralizes bases. d. HCl is an example of a strong acid. e. Acids are only strong at a high concentration.

E

Describe the position of electrons around one N atom in the Lewis structure of N2. a. 3 shared electron pairs, 1 lone pair b. 2 shared electron pairs, 2 lone pairs c. 1 shared electron pair, 3 lone pairs d. 3 shared electron pairs e. 2 shared electron pairs, 1 lone pair

A

Determine the oxidation state of P in PO3 3-. A) +3 B) +6 C) +2 D) 0 E) -3

A

How many gold atoms are there in a 1.00 kg bar of gold? a. 3.06 1024 d. 5.08 10-3 mol b. 197 mol e. 5.08 1018 c. 3.06 1021

A

How many gold atoms are there in a 1.00 kg bar of gold? a. 3.06 X 10 24 d. 5.08 X 10-3 mol b. 197 mol e. 5.08 10 18 c. 3.06 X 10 21

A

In one analysis, 3.01 1013 molecules of ozone were found in an air sample. How many moles of ozone is this? a. 5.00 1011 mol d. 5.00 1037 mol b. 1.81 1037 mol e. 6.02 1023 mol c. 1.81 1011 mol

A

Most chloride salts are soluble. Identify an exception to this generalization. a. AgCl d. BaCl2 b. CaCl2 e. NaCl c. MgCl2

A

Silicon is best described as a ________ a. metalloid. d. noble gas. b. metal. e. nonmetal. c. transition metal.

A

The density of iron is 7.9 g/cm3. What is the volume of a 4.5 kg iron block? a. 570 cm3 d. 35.6 cm3 b. 0.570 cm3 e. 1.76 cm3 c. 3.56 104 cm3

A

The mass of 0.25 mol of some element is 8.0 g. What is the element? a. O2 d. Br2 b. N2 e. H2 c. Cl2

A

A gas, initially at 2.50 atm and 3.00 L, expands to a volume of 10.00 L. What is the new pressure of the gas? a. 0.75 atm d. 8.33 atm b. 1.33 atm e. 12.0 atm c. 2.10 atm

A

An orbital's shape is determined by ________ a. the quantum number. d. the n quantum number. b. the ml quantum number. e. both the n and quantum numbers. c. the ms quantum number.

A

Sodium metal easily loses an electron to form the sodium ion. In this process, sodium is ________ a. reduced. d. complexed. b. oxidized. e. both ionized and oxidized. c. ionized.

E

An orbital's orientation in space is determined by ________ a. the quantum number. d. the n quantum number. b. the ml quantum number. e. both the l and ml quantum numbers. c. the ms quantum number.

B

Dialuminum hexachloride, Al2Cl6 (266.66 g/mol), is an inexpensive compound that is used in many industrial processes. It is made by treating scrap aluminum with chlorine gas. If a reaction is run with 270 g of aluminum and 710 grams of chlorine, the limiting reactant is ________, and the theoretical yield is ________ of Al2Cl6. 2Al(s) 3Cl2(g) Al2Cl6(s) a. Al; 890 g d. Cl2; 1,300 g b. Cl2; 890 g e. Cl2; 2,700 g c. Al; 1,300 g

B

During a(n) ________ process, energy is transferred to the system from the surroundings. a. exothermic d. thermochemical b. endothermic e. physical c. thermodynamic

B

How many moles of ammonia are there in a 346 g sample of pure NH3 (17.03 g/mol)? a. 0.0496 mol d. 5,930 mol b. 20.3 mol e. 3.46 mol c. 24.7 mol

B

How many moles of ammonia are there in a 346 g sample of pure NH3 (17.03 g/mol)? a. 0.0496 mol d. 5,930 mol b. 20.3 mol e. 3.46 mol c. 24.7 mol

B

In its reaction with water, ammonia (NH3) ________ a. acts as an acid. b. acts as a base. c. acts neither as an acid nor as a base. d. serves as both an acid and as a base. e. causes a precipitate to form.

B

Sodium nitrite, which is used in meat processing, has been implicated as a possible health hazard because it can react with amines present in meat to form trace quantities of carcinogenic nitrosamines. What is the formula of sodium nitrite? a. Na2NO3 d. Na2NO4 b. NaNO2 e. Na2NO2 c. NaNO3

B

The summit of Mt. Humphreys, the highest point in Arizona, is 12,600 ft. How many meters is this? (1 m 1.0936 yd, 1 yd 3 ft exactly) a. 4,593 m d. 41,338 m b. 3,841 m e. 37,800 m c. 34,565 m

B

What ml quantum numbers are possible when n 2 and l 1? a. 0 and 1 d. 2, 1, 0, 1, and 2 b. 1, 0, and 1 e. 0 c. 0, 1 and, 2

B

Which of the following ionic compounds is insoluble in water? a. BaCl2 d. Ba(NO3)2 b. BaSO4 e. MgCl2 c. NaOH

B

Which of the following is the correct Lewis symbol for the oxide anion (O2)? brooke it would not post pic a. a. c. c. b. b. d. d.

B

Identify a spectator ion in the following acid-base reaction. Ca(CO3)(s) 2HCl(aq) CaCl2(aq) 2H2O(l ) CO2(g) a. H+ d. CO32- b. Ca2+ e. H3O+ c. Cl-

C

If the following operations are carried out, how many significant figures should be reported in the answer? 213-0.32+2.3-57.432 a. 1 d. 4 b. 2 e. 5 c. 3

C

If the following operations are carried out, how would the final answer be reported? (14.1+12.14) X 7.45 a. 195.19 d. 2.00 102 b. 195.2 e. 195.5 c. 195

C

In the following reaction, which element or ion is reduced? Cl2(g) NaBr(aq) NaCl(aq) Br2(g) a. Br2 d. Br - b. Na e. C- c. Cl2

C

Magnesium hydroxide is insoluble. Write the net ionic equation for the reaction that takes place between a solution of magnesium chloride and a solution of sodium hydroxide. a. MgCl2(aq) NaOH(aq) MgOH(s) NaCl2(aq) b. MgCl2(aq) 2NaOH(aq) Mg(OH)2(s) 2NaCl(aq) c. Mg2(aq) 2OH(aq) Mg(OH)2(s) d. Mg2(aq) 2Cl (aq) 2Na(aq) 2OH(aq) Mg(OH)2(s) 2NaCl(s) e. Mg2(aq) OH(aq) MgOH(s)

C

Ozone (O3) reacts with iodide (I-) and water to form iodine (I2), hydroxide (OH-), and oxygen (O2). Balance the following reaction equation and report the sum of the stoichiometric coefficients. O3 I H2O I2 OH O2 a. 10 d. 12 b. 6 e. 14 c. 8

C

What is the change in internal energy (E) of a system when it loses 10 kJ of energy and 5,000 J of work is done on the system? a. +15 kJ d. +5,010 J b. -10 kJ e. +4,990 J c. -5 kJ

C

What is the ground-state electron configuration of a Cl- ion? a. 1s22s22p63s23p4 d. 1s22s22p63s23p2 b. 1s22s22p63s23p5 e. 1s22s22p63s23p8 c. 1s22s22p63s23p6

C

15.00 g of aluminum sulfide and 10.00 g of water react until the limiting reactant is used up. Balance the reaction equation, identify the limiting reactant, and report the mass of H2S that can be produced from these reactants. ________Al2S3 ________H2O ________Al(OH)3 ________H2S a. 13.89 g d. 9.458 g b. 10.00 g e. 1.108 g c. 15.00 g

D

A 35/17 Cl atom has ________ protons, ________ neutrons, and ________ electrons. a. 17; 18; 19 d. 17; 18; 17 b. 17; 20; 17 e. 18; 17; 18 c. 17; 17; 20

D

A hypothetical element has two stable isotopes: one isotope has a mass of 106.9051 amu with an abundance of 48.183%, the other isotope has a mass of 108.9048 amu with an abundance of 51.825%. What is the average atomic mass of this element? a. 107.980 amu d. 107.950 amu b. 107.970 amu e. 107.940 amu c. 107.960 amu

D

A mass of 11.60 g of phosphoric acid was produced from the reaction of 10.00 g of P4O10 with 12.00 g water. What was the percent yield for this reaction? a. 78.62% d. 84.00% b. 101.1% e. 52.70% c. 92.70%

D

Determine the enthalpy for the following reaction, given (NH3(g)) 46.1 kJ/mol, (NO(g)) 90.3 kJ/mol, and (H2O(g)) 241.8 kJ/mol. 4NH3(g) 5O2(g) 4NO(g) 6H2O(g) Hrxn ? kJ a. -1274 kJ/mol d. -905.2 kJ/mol b. -1,996 kJ/mol e. -105.4 kJ/mol c. +1,274 kJ/mol

D

During an exothermic process, ________ for the system. a. q > 0 d. /\H<0 b. w > 0 e. q + w=0 c. /\H>0

D

Extensive properties are ________ a. physical properties and not chemical properties. b. identical for all substances. c. independent of the volume of substance present. d. dependent on the amount of substance. e. dependent on factors external to the substance itself.

D

Fool's Gold is the mineral pyrite (FeS2). What is the mass percent of sulfur in pyrite? a. 36.44% d. 53.41% b. 46.59% e. 63.56% c. 49.09%

D

If there are 0.505 g of NaCl left in a beaker that originally contained 75.0 mL of saltwater, what must have been the concentration of the original solution? a. 0.00647 M d. 0.115 M b. 0.0115 M e. 0.673 M c. 0.0673 M

D

In which one of the following compounds is the oxidation number of phosphorus equal to 5? a. PH3 d. P2O5 b. P4S6 e. P4 c. PO33

D

Molarity, M, is defined as ________ a. moles of solute dissolved in 1 mol of solvent. b. moles of solute dissolved in 1 kg of solvent. c. moles of solute dissolved in 1 L of solvent. d. moles of solute dissolved in 1 L of solution. e. moles of solute dissolved in the solution.

D

The symbol and name corresponding to the factor 10(-6) is ________ a. f, femto. d. u , micro. b. p, pico. e. m, milli. c. n, nano.

D

The symbol and name corresponding to the factor 106 is ________ a. f, femto. d. u , micro. b. p, pico. e. m, milli. c. n, nano.

D

What are the spectator ions in the reaction of barium hydroxide and nitric acid? a. H3O and NO3 d. Ba2 and NO3 b. Ba2 and OH e. Ba2, NO3, H3O, and OH c. H3O and OH

D

What is the electron configuration for sulfur? a. 1s22s22p4 d. [Ne]3s23p4 b. 1s22s22p63s23p5 e. 1s22s22p5 c. [He]2s22p4

D

What is the molar mass of sulfuric acid (H2SO4)? a. 49.0 g/mol d. 98.1 g/mol b. 24.5 g/mol e. 97.0 g/mol c. 101 g/mol

D

What mass of phosphoric acid (H3PO4, 98.00 g/mol) is produced from the reaction of 10.00 g of P4O10 (283.89 g/mol) with 12.00 g water? a. 10.90 g d. 13.81 g b. 0.14 g e. 14.52 g c. 43.52 g

D

Which of the following is most likely to exhibit covalent bonding? a. NaF d. CO2 b. CaCl2 e. NaCl c. Cs2O

D

Which of the following is the ground-state electron configuration of the Mg2 ion? a. 1s22s22p63s2 d. [He]2s22p6 b. [Ne]3s2 e. [He]2s22p8 c. [Ne]3s23p2

D

Which of the following quantities has two significant figures? a. 0.4 d. 0.0092 b. 101 e. 0.520 c. 1.10 103

D

Which one of these formula-name combinations is not correct? a. diphosphorus tetroxide: P2O4 b. tetraphosphorus nonoxide: P4O9 c. diphosphorus pentoxide: P2O5 d. tetraphosphorus heptoxide: P4O6 e. phosphorus monoxide: PO

D

Which statement about isotopes of the same element is not correct? a. They have the same number of protons. b. They have different numbers of neutrons. c. They have essentially the same chemical properties. d. They have the same atomic mass. e. They have the same number of electrons.

D

A sample of Ar gas at 35C occupies a volume of 1.50 L at a pressure of 3.2 atm. How many moles of the gas are present in the sample? a. 3.32 moles d. 1.67 moles b. 0.599 moles e. 0.190 moles c. 5.26 moles

E

In quantum mechanics, an atomic orbital ________ a. provides the position of an electron at any instant of time in the space around an atomic nucleus. b. locates all the electrons in an atom. c. is identical to the orbits Bohr used in his analysis of the hydrogen atom. d. identifies the most probable position of an atomic nucleus. e. provides the probability of finding an electron at any point in the space around an atomic nucleus.

E