Chemistry Final Exam

Which factors listed below will speed up the dissolving of a solid solute in water? I. Cool the solution II. Heat the solution III. Grind up the solute IV. Decrease the surface area of the solute Select one: a. I and III b. III and II c. II and IV d. I and IV

b. III and II

A colorless liquid composed of 46.68% N and 53.32 % O has a molar mass of 60.01 g/mol. Find the molecular formula. Select one: a. N3O2 b. N2O2 c. N4O2 d. N5O2

b. N2O2

Given: H2O, NaOH, HC2H3O2, or CH4, choose the strong base. Select one: a. CH4 b. NaOH c. H2O d. HC2H3O2

b. NaOH

The following reaction :2Hg + O2 --> 2HgO can be classified as what type of reaction? Select one: a. Double Replacement b. Synthesis c. Decomposition d. Single Replacement

b. Synthesis

What is the molarity of an HCl solution if 50.0 mL is neutralized in a titration by 40.0 mL of 0.400 M NaOH? Select one: a. 0.500 M b. 0.200 M c. 0.280 M d. 0.320 M

d. 0.320 M

A sample of gas at 255 K occupies a volume of 1.55 L. If the temperature is raised to 298 K what will be the new volume? Select one: a. 4.81 L b. 2.81 L c. 6.81 L d. 1.81 L

d. 1.81 L

You have 200.0 cm3 of nitrogen(IV) oxide at a temperature of 303.0 K and a pressure of 101.0 kPa. What volume will the NO2 occupy at 255.0 kPa and 371.0 K? Select one: a. 67.99 cm3 b. 88.99 cm3 c. 96.99 cm3 d. 35.99 cm3

c. 96.99 cm3

What is the minimum energy required for an effective collision? Select one: a. Potential Energy b. Kinetic Energy c. Activation Energy d. Collision Energy

c. Activation Energy

What is the net ionic equation for the precipitation reaction between BaCl2 and Na2SO4? Select one: a. BaCl2(aq) + Na2SO4(aq) -> BaSO4(s) + 2NaCl(aq) b. Na+(aq) + Cl-(aq) -> NaCl(s) c. Ba2+(aq) + SO42-(aq) -> BaSO4(s) d. Ba2+(aq) + 2Cl-(aq) + 2 Na+(aq) + SO42-(aq) -> BaSO4(s) + 2Cl-(aq) + 2Na+(aq)

c. Ba2+(aq) + SO42-(aq) -> BaSO4(s)

Coffee has a pH of about 5. What type of solution would it form? Select one: a. Acidic b. Strong c. Basic d. Neutral

c. Basic

Whose acid definition is the broadest? Select one: a. Arrhenius b. Faraday c. Brønsted-Lowry d. Lewis

c. Brønsted-Lowry

What is the empirical formula for a compound that is 27.3 % C and 72.7 % O? Select one: a. CO4 b. CO6 c. CO2 d. CO

c. CO2

What type of solution that contains all of the solute it can hold at a given temperature? Select one: a. Supersaturated b. Unsaturated c. Saturated d. Suspension

c. Saturated

The following reaction : Cr + Fe(NO3)2 à Fe + Cr(NO3)3, can be classified as what type of reaction? Select one: a. Decomosition b. Double Replacement c. Single Replacement d. Synthesis

c. Single Replacement

What type of solution that contains more solute than it can hold at a given temperature? Select one: a. Unsaturated b. Saturated c. Supersaturated d. Suspension

c. Supersaturated

What must occur in order for gas particles to react? Select one: a. They must be at the critical temperature b. They must be the same element c. They must collide d. Activation energy must be applied

c. They must collide

What type of solution that contains less solute than it is able to hold at a given temperature? Select one: a. Saturated b. Supersaturated c. Unsaturated d. Suspension

c. Unsaturated

Acids generally release H2 gas when they react with Select one: a. inactive metals. b. nonmetals. c. active metals. d. semimetals.

c. active metals.

If H3O+ of a solution is less than OH-, the solution Select one: a. is always acidic. b. is always neutral. c. is always basic. d. might be acidic, basic, or neutral.

c. is always basic.

The conjugate of a weak base is a Select one: a. strong base. b. weak base. c. strong acid. d. weak acid.

c. strong acid.

The conjugate of a strong base is a Select one: a. strong base. b. weak base. c. weak acid. d. strong acid.

c. weak acid.

Which compound dissociates to produce the ions SO42-(aq) and NH4+(aq)? Select one: a. (NH4)2SO4(s) b. NH4SO4(s) c. NH4(SO4)2(s) d. (NH4)3(SO4)2(s)

a. (NH4)2SO4(s)

What is the coefficient that belongs in front of oxygen in the equation? ____C3H8 + ___O2 --> ____CO2 + ___H2O Select one: a. 5 b. 4 c. 3 d. 6

a. 5

Which compound dissociates to produce the ions Ca2+(aq) and NO3-(aq)? Select one: a. Ca(NO3)2(s) b. CaNO3(s) c. Ca2(NO3)3 d. Ca2NO3

a. Ca(NO3)2(s)

Find the percent composition of CaC2. Select one: a. 72.5%Ca, 27.5 C b. 62.5%Ca, 37.5 C c. 25.5%Ca, 74.5 C d. 52.5%Ca, 47.5 C

b. 62.5%Ca, 37.5 C

How much heat does it take to warm 16.0 g of pure water from 90°C to 100 °C? The specific heat of water is 4.18 J/g°C Select one: a. 270 J b. 669 J c. 768 J d. 549 J

b. 669 J

A gas at 925.0 mm Hg pressure at 50.00 °C is cooled to -25.00 °C. What is the final pressure in mm Hg? Select one: a. 912.4 mm Hg b. 710.2 mm Hg c. 624.8 mm Hg d. 872.5 mm Hg

b. 710.2 mm Hg

A reaction in which oxygen combines with a substance and releases heat and light can be classified as what type of reaction? Select one: a. Single Replacement Reaction b. Combustion Reaction c. Synthesis Reaction d. Double Replacement Reaction

b. Combustion Reaction

What is the net ionic equation for the precipitation reaction between copper(II) chloride and sodium hydroxide? Select one: a. Cu2+(aq) + 2OH-(aq) + 2Cl-(aq) -> Cu(OH)2(s) + 2Cl-(aq) b. Cu2+(aq) + 2OH-(aq) -> Cu(OH)2(s) c. Cu2+(aq) + 2Cl-(aq) + 2Na+(aq) + 2OH-(aq) -> Cu(OH)2(s) + 2NaCl(s) d. Na+(aq) + Cl-(aq) -> NaCl(s)

b. Cu2+(aq) + 2OH-(aq) -> Cu(OH)2(s)

What combination of pressure and temperature would increase the solubility of a gas in a liquid? Select one: a. Increase pressure and decrease temp b. Decrease pressure and Increase temp c. Keep pressure constant and increase temp d. Increase temp and decrease pressure

b. Decrease pressure and Increase temp

A compound is composed of 82.68% mercury, (Hg), and 17.32% nitrogen, (N). What is the compounds empirical formula? Select one: a. HgN b. HgN3 c. HgN4 d. HgN2

b. HgN3

How does a catalyst increases the rate of a chemical reaction? Select one: a. Requires no activation energy for the reaction to occur b. Raises the activation energy of the reaction c. Enhances the activation energy of the reaction d. Lowers the activation energy of the reaction

a. Requires no activation energy for the reaction to occur

What is the substance that dissolves a solute to form a solution? Select one: a. Solvent b. Aqueous c. Liquid d. Concentrated Solution

a. Solvent

A species that can react as either an acid or a base is Select one: a. amphoteric substance. b. oxyacid. c. Lewis acid. d. salt.

a. amphoteric substance.

A sample of SO2 gas has a volume of 9.50 L at a temperature of 320K. At what temperature will the gas have a volume of 2.55 L? Select one: a. 56 K b. 96 K c. 86 K d. 46 K

c. 86 K

What are the coefficients to correctly balance the formula equation? Al2(SO4)3 + KOH → Al(OH)3 + K2SO4 Select one: a. 1,6,2,3 b. 2,6,3,1 c. 3,2,1,6 d. 1,3,2,6

a. 1,6,2,3

A sample of ammonia gas occupies a volume of 27.4 L at 14.0o C and a pressure of 1.20 atm. What volume will the sample occupy at 3.00 atm and 0 oC? Select one: a. 10.4L b. 23.5L c. 35.8L d. 24.6L

a. 10.4L

Find the percent composition of MgSO4. Select one: a. 20.2%Mg, 26.6%S, 53.2%O b. 20.2%Mg, 36.6%S, 43.2%O c. 30.2%Mg, 16.6%S, 53.2%O d. 10.2%Mg, 36.6%S, 53.2%O

a. 20.2%Mg, 26.6%S, 53.2%O

What is the net ionic equation for the precipitation reaction between silver nitrate solution and sodium sulfide solution? Select one: a. 2Ag+(aq) + S2-(aq) -> Ag2S(s) b. 2Ag+(aq) + 2NO3-(aq) + 2Na+(aq) + S2-(aq) -> Ag2S(s) + 2Na+(aq) + 2NO3-(aq) c. 2Ag+(aq) + 2NO3-(aq) + 2Na+(aq) + S2-(aq) -> Ag2S(s) + 2NaNO3(s) d. Na+(aq) + NO3-(aq) -> NaNO3(s)

a. 2Ag+(aq) + S2-(aq) -> Ag2S(s)

Find the percent composition of MgS. Select one: a. 43.1%Mg , 56.9%S b. 33.1%Mg , 66.9%S c. 73.1%Mg , 36.9%S d. 40.1%Mg , 59.9%S

a. 43.1%Mg , 56.9%S

A compound contains 36.1 g calcium and 63.9 g chlorine. What is the empirical formula of the compound? Select one: a. CaCl2 b. CaCl5 c. CaCl d. CaCl3

a. CaCl2

The following reaction : AgNO3(aq) + NaCl (aq) --> AgCl(s) + NaNO3(aq) , can be classified as what type of reaction? Select one: a. Double Replacement b. Single Replacement c. Decomposition d. Combustion

a. Double Replacement

What are the products of the neutralization reaction between sodium hydroxide and sulfuric acid? Select one: a. Na2SO4 and H2O b. Na2SO3 and H2O c. Na2SO2 and H2O d. Na2SO4 and H3O

a. Na2SO4 and H2O

What is the expression that represents the pH of a solution? Select one: a. -log [H+] b. -log [HO-] c. -log[pOH] d. -log [OH+]

b. -log [HO-]

The molar mass of H2O is 18.015 g/mol. How many moles of water are present in 3.6 g? Select one: a. 0.15 mol b. 0.20 mol c. 0.78 mol d. 0.56 mol

b. 0.20 mol

A sample of gas at 2.50 atm and 6.50 L is compressed to 1.50L at a constant temperature. What is the new pressure? Select one: a. 67.8 atm b. 10.8 atm c. 34.8 atm d. 45.8 atm

b. 10.8 atm

What is the formula mass of (NH4)3PO4 ? Select one: a. 154.7 amu b. 149.0 amu c. 176.9 amu d. 167.9 amu

b. 149.0 amu

The molar mass of CO2 is 44 g/mol. How many moles are present in 110 g? Select one: a. 3.2 mol b. 2.5 mol c. 2.1 mol d. 3.5 mol

b. 2.5 mol

What is the OH- concentration of a solution whose pH is 12.40? Select one: a. 1.0 x 10-1 M b. 2.5 x 10-2 M c. 8.9 x 10-2 M d. 4.4 x 10--2 M

b. 2.5 x 10-2 M

What is the balanced equation when aluminum reacts with copper(II)sulfate? Select one: a. 3Al + 3CuSO4à Al2(SO4)3 + 3Cu b. 2Al + 3CuSO4à Al2(SO4)3 + 3Cu c. Al + CuSO4à Al2(SO4)3 + Cu d. 2Al + 2CuSO4à Al2(SO4)3 + 3Cu

b. 2Al + 3CuSO4à Al2(SO4)3 + 3Cu

The temperature of a sample of water increases from 20.0°C to 46.6°C as it absorbs 5650 J of heat. What is the mass of the sample? The specific heat of water is 4.18 J/g°C. Select one: a. 17.2 g b. 34.6 g c. 50.8 g d. 67.3 g

b. 34.6 g ****

What type of acids and bases produce only a few ions in solution? Select one: a. Miscible b. Weak c. Strong d. Concentrated

b. Weak

If H3O+ of a solution is greater than OH-, the solution Select one: a. is always basic. b. is always acidic. c. is always neutral. d. might be acidic, basic, or neutral.

b. is always acidic.

The temperature of a sample of iron with a mass of 10.0 g changed from 50.4°C to 25.0°C with the release of 114 J of heat. What is the specific heat of iron? Select one: a. 0.219 J/ g oC b. 0.699 J/ g oC c. 0.449 J/ g oC d. 0.359 J/ g oC

c. 0.449 J/ g oC

A sample of an unknown metal has a mass of 120.7 g. As the sample cools from 90.5oC to 25.7oC, it releases 7020 J of energy. What is the specific heat of the sample? Select one: a. 0.789J/g oC b. 0.649 J/g oC c. 0.898 J/g oC d. 0.359 J/g oC

c. 0.898 J/g oC

The specific heat of ethanol is 2.44 J/g°C. How many joules of energy are required to heat 50.0 g of ethanol from -20.0°C to 68.0°C? Select one: a. 14890 J b. 13450 J c. 10700 J d. 11930 J

c. 10700 J

Find the percent composition of KClO4. Select one: a. 58.2%K, 15.6%Cl, 26.2%O b. 18.2%K, 15.6%Cl, 26.2%O c. 28.2%K, 25.6%Cl, 46.2%O d. 38.2%K, 15.6%Cl, 46.2%O

c. 28.2%K, 25.6%Cl, 46.2%O

What is the hydronium ion concentration of a solution whose pH is 7.30? Select one: a. 7.1 x 10-6 M b. 3.8 x 10-8 M c. 5.0 x 10-8 M d. 1.4 x 10-11 M

c. 5.0 x 10-8 M

The molar mass of NH3 is 17.0 g/mol. How many grams of NH3 are present in 3.50 moles? Select one: a. 51.4 g b. 67.4 g c. 59.5 g d. 65.7 g

c. 59.5 g

What is the correct molar mass of Ca(OH)2 ? Select one: a. 68.7 g b. 58.5 g c. 74.0 g d. 84.9 g

c. 74.0 g

What pressure will be needed to reduce the volume of 77.4 L of helium at 98.0 kPa to a volume of 60.0L? Select one: a. 226 kPa b. 146 kPa c. 176 kPa d. 126 kPa

d. 126 kPa

Determine the temperature of 2.49 moles of gas contained in a 2.00L vessel at a pressure of 1.41 atm. Select one: a. 43.8K b. 23.8K c. 15.8K d. 13.8K

d. 13.8K

What are the coefficients to correctly balance the formula equation? AlCl3(aq) + Pb(NO3)2(aq) → PbCl2(s) + Al(NO3)3(aq) Select one: a. 2,4,3,6 b. 1,2,2,3 c. 1,2,3,6 d. 2,3,3,2

d. 2,3,3,2

You have 422.0 cm3 of nitrogen(IV) oxide at a temperature of 295.15 K and a pressure of 101.325 kPa. What volume will the NO2 occupy at 155.00 kPa and 317.15 K? Select one: a. 496.4 cm3 b. 396.4 cm3 c. 196.4 cm3 d. 296.4 cm3

d. 296.4 cm3

What is the pressure in atmospheres of a 0.108 mole sample of helium gas at a temperature of 20.0°C if its volume is 0.505 L? Select one: a. 7.14 atm b. 4.14 atm c. 6.14 atm d. 5.14 atm

d. 5.14 atm

Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm. Select one: a. 5.81L b. 8.81L c. 9.81L d. 7.81L

d. 7.81L

What is the term for a solution in which water is the solvent? Select one: a. Liquid b. Hydrated c. Spectator Ions d. Aqueous

d. Aqueous

What type of energy change is shown in the following reaction Sn +Cl2 → SnCl2 enthalpy = -325KJ Select one: a. Sigma b. Endothermic c. Amphoteric d. Exothermic

d. Exothermic

What are the substances produced when KOH (aq) neutralizes HCl (aq) ? Select one: a. H2O and NaCl b. H3O and KCl2 c. KOH and Nacl d. H2O and KCl

d. H2O and KCl

The elemental analysis of a sample of ionic compound gave the following results: 2.82 g Na, 4.35 g Cl, and 7.83 g O. The empirical formula of this compound is: Select one: a. NaClO2 b. NaClO3 c. NaClO d. NaClO4

d. NaClO4

A reaction in which the atoms of one element replace the atoms of another element in a compound can be classified as what type of reaction? Select one: a. Combustion b. Double Replacement c. Synthesis d. Single Replacement

d. Single Replacement

What is the substance that is dissolved in a solution? Select one: a. Solvent b. Water c. Liquid d. Solute

d. Solute

If a crystal is added to an aqueous solution and it causes many crystals to come out of the solution, what type of solution was it originally? Select one: a. Unsaturated b. Ionic c. Covalent d. Supersaturated

d. Supersaturated

What term refers to the ease with which an acid or base forms ions in solution? Select one: a. Concentrated b. Aqueous c. strength d. Weak

d. Weak

Dyes with pH-sensitive colors are used as Select one: a. None of the above b. primary standards. c. titrants. d. indicators.

d. indicators.

Bases feel Select one: a. moist. b. rough. c. dry. d. slippery.

d. slippery.

The conjugate of a strong acid is a Select one: a. weak acid. b. strong base. c. strong acid. d. weak base.

d. weak base.