Question 1

Renewable energy sources are essentially inexhaustible.

Accepted Answer

A) True 
 B)False

Question 2

A slice of apple pie contains 14.0 grams of fat, 2.00 grams of protein, and 52.0 grams of carbohydrate. The respective fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively. If cycling typically burns 1000.0 kJ/hour, ________ minutes of cycling are required to completely burn off the slice of pie.

Accepted Answer

A) 1.45 
B) 4.66 
C) 8.25 
D) 87.0 
E) < 1 
A) 1.45 
B) 4.66 
C) 8.25 
D) 87.0 
E) < 1

Question 3

Which one of the choices below is not considered a fossil fuel?

Accepted Answer

A) anthracite coal 
B) crude oil 
C) natural gas 
D) hydrogen 
E) petroleum 
A) anthracite coal 
B) crude oil 
C) natural gas 
D) hydrogen 
E) petroleum

Question 4

Objects can possess energy as ________. (a)endothermic energy
(b)potential energy
(c)kinetic energy

Accepted Answer

A) a only 
B) b only 
C) c only 
D) a and c 
E) b and c 
A) a only 
B) b only 
C) c only 
D) a and c 
E) b and c

Question 5

A 5-ounce cup of raspberry yogurt contains 6.0 g of protein, 2.0 g of fat, and 16.3 g of carbohydrate. The fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively. The fuel value of this cup of yogurt is ________ kJ.

Accepted Answer

A) 460 
B) 520 
C) 280 
D) 720 
E) 72 
A) 460 
B) 520 
C) 280 
D) 720 
E) 72

Question 6

A 50.0-g sample of liquid water at 25.0 °C is mixed with 23.0 g of water at 79.0 °C. The final temperature of the water is ________ °C.

Accepted Answer

A) 123 
B) 27.3 
C) 52.0 
D) 231 
E) 42.0 
A) 123 
B) 27.3 
C) 52.0 
D) 231 
E) 42.0

Question 7

The kinetic energy of a 10.3 g golf ball traveling at 48.0 m/s is ________ J.

Accepted Answer

A) 1.20 × 103 
B) 66 
C) 11.9 
D) 1.3 × 102 
E) 23.7 
A) 1.20 × 103 
B) 66 
C) 11.9 
D) 1.3 × 102 
E) 23.7

Question 8

ΔH for the reaction IF5 (g) → IF3 (g) + F2 (g)
Is ________ kJ, give the data below.
IF (g) + F2 (g) → IF3 (g)ΔH = -390 kJ
IF (g) + 2F2 (g) → IF5 (g)ΔH = -745 kJ

Accepted Answer

A) +355 
B) -1135 
C) +1135 
D) +35 
E) -35 
A) +355 
B) -1135 
C) +1135 
D) +35 
E) -35

Question 9

The specific heat capacity of liquid mercury is 0.14 J/g-K. How many joules of heat are needed to raise the temperature of 6.00 g of mercury from 25.1 °C to 65.3 °C?

Accepted Answer

A) 1.7 × 103 J 
B) 34 J 
C) 76 J 
D) 5.8 × 10-4 J 
E) 2.2 J 
A) 1.7 × 103 J 
B) 34 J 
C) 76 J 
D) 5.8 × 10-4 J 
E) 2.2 J

Question 10

The value of ΔE for a system that performs 151 kJ of work on its surroundings and loses 79 kJ of heat is ________ kJ.

Accepted Answer

A) +230. 
B) -230. 
C) +72 
D) -72 
E) -151 
A) +230. 
B) -230. 
C) +72 
D) -72 
E) -151

Question 11

The value of ΔH° for the reaction below is -482 kJ. Calculate the heat (kJ)released to the surroundings when 10.0 g of CO (g)reacts completely. 2CO (g) + O2 (g) → 2CO2 (g)

Accepted Answer

A) 2410 kJ 
B) 172 kJ 
C) 86.0 kJ 
D) 482 kJ 
E) -482 kJ 
A) 2410 kJ 
B) 172 kJ 
C) 86.0 kJ 
D) 482 kJ 
E) -482 kJ

Question 12

An 6.11 g sample of calcium carbonate [CaCO3 (s)] absorbs 84 J of heat, upon which the temperature of the sample increases from 19.2 °C to 35.9 °C. What is the specific heat of calcium carbonate?

Accepted Answer

A) 0.82 J/g-K 
B) -0.82 J/g-K 
C) 31 J/g-K 
D) 230 J/g-K 
E) 8600 J/g-K 
A) 0.82 J/g-K 
B) -0.82 J/g-K 
C) 31 J/g-K 
D) 230 J/g-K 
E) 8600 J/g-K

Question 13

The value of ΔH° for the reaction below is -790 kJ. The enthalpy change accompanying the reaction of 0.95 g of S is ________ kJ. 2S (s) + 3O2 (g) → 2SO3 (g)

Accepted Answer

A) 23 
B) -23 
C) -12 
D) 12 
E) -790 
A) 23 
B) -23 
C) -12 
D) 12 
E) -790

Question 14

The specific heat of bromine liquid is 0.226 J/g-K. The molar heat capacity (in J/mol-K)of bromine liquid is ________.

Accepted Answer

A) 707 J/mol-K 
B) 36.1 J/mol-K 
C) 18.1 J/mol-K 
D) 9.05 J/mol-K 
E) 0.226 J/mol-K 
A) 707 J/mol-K 
B) 36.1 J/mol-K 
C) 18.1 J/mol-K 
D) 9.05 J/mol-K 
E) 0.226 J/mol-K

Question 15

A 25.5-g piece of cheddar cheese contains 37% fat, 28% protein, and 4% carbohydrate. The respective fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively. The fuel value for this piece of cheese is ________ kJ.

Accepted Answer

A) 450 
B) 330 
C) 790 
D) 99 
E) 260 
A) 450 
B) 330 
C) 790 
D) 99 
E) 260

Question 16

The primary component of natural gas is propane.

Accepted Answer

A) True 
 B)False

Question 17

Given the data in the table below, ΔH°rxn for the reaction 2SO2 (g) + O2 (g) → 2SO3 (g)
Is ________ kJ.

Accepted Answer

A) -99 
B) 99 
C) -198 
D) 198 
E) The ΔH°f of O2 (g)is needed for the calculation. 
A) -99 
B) 99 
C) -198 
D) 198 
E) The ΔH°f of O2 (g)is needed for the calculation.

Question 18

Which one of the following is an exothermic process?

Accepted Answer

A) ice melting 
B) water evaporating 
C) boiling soup 
D) condensation of water vapor 
E) Ammonium thiocyanate and barium hydroxide are mixed at 25 °C: the temperature drops. 
A) ice melting 
B) water evaporating 
C) boiling soup 
D) condensation of water vapor 
E) Ammonium thiocyanate and barium hydroxide are mixed at 25 °C: the temperature drops.

Question 19

Work equals force times distance.

Accepted Answer

A) True 
 B)False

Question 20

The change in the internal energy of a system that releases 2,500 J of heat and that does 7,655 J of work on the surroundings is ________ J.

Accepted Answer

A) -10,155 
B) -5,155 
C) -1.91 × 107 
D) 10,155 
E) 5,155 
A) -10,155 
B) -5,155 
C) -1.91 × 107 
D) 10,155 
E) 5,155

Exam 5: Thermochemistry

Renewable energy sources are essentially inexhaustible.

Which one of the choices below is not considered a fossil fuel?

Objects can possess energy as ________. (a)endothermic energy (b)potential energy (c)kinetic energy

A 5-ounce cup of raspberry yogurt contains 6.0 g of protein, 2.0 g of fat, and 16.3 g of carbohydrate. The fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively. The fuel value of this cup of yogurt is ________ kJ.

A 50.0-g sample of liquid water at 25.0 °C is mixed with 23.0 g of water at 79.0 °C. The final temperature of the water is ________ °C.

The kinetic energy of a 10.3 g golf ball traveling at 48.0 m/s is ________ J.

ΔH for the reaction IF5 (g) → IF3 (g) + F2 (g) Is ________ kJ, give the data below. IF (g) + F2 (g) → IF3 (g)ΔH = -390 kJ IF (g) + 2F2 (g) → IF5 (g)ΔH = -745 kJ

The specific heat capacity of liquid mercury is 0.14 J/g-K. How many joules of heat are needed to raise the temperature of 6.00 g of mercury from 25.1 °C to 65.3 °C?

The value of ΔE for a system that performs 151 kJ of work on its surroundings and loses 79 kJ of heat is ________ kJ.

The value of ΔH° for the reaction below is -482 kJ. Calculate the heat (kJ)released to the surroundings when 10.0 g of CO (g)reacts completely. 2CO (g) + O2 (g) → 2CO2 (g)

An 6.11 g sample of calcium carbonate [CaCO3 (s)] absorbs 84 J of heat, upon which the temperature of the sample increases from 19.2 °C to 35.9 °C. What is the specific heat of calcium carbonate?

The value of ΔH° for the reaction below is -790 kJ. The enthalpy change accompanying the reaction of 0.95 g of S is ________ kJ. 2S (s) + 3O2 (g) → 2SO3 (g)

The specific heat of bromine liquid is 0.226 J/g-K. The molar heat capacity (in J/mol-K)of bromine liquid is ________.

A 25.5-g piece of cheddar cheese contains 37% fat, 28% protein, and 4% carbohydrate. The respective fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively. The fuel value for this piece of cheese is ________ kJ.

The primary component of natural gas is propane.

Given the data in the table below, ΔH°rxn for the reaction 2SO2 (g) + O2 (g) → 2SO3 (g) Is ________ kJ.

Which one of the following is an exothermic process?

Work equals force times distance.

The change in the internal energy of a system that releases 2,500 J of heat and that does 7,655 J of work on the surroundings is ________ J.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

ΔH for the reaction IF₅ (g) → IF₃ (g) + F₂ (g) Is ________ kJ, give the data below. IF (g) + F₂ (g) → IF₃ (g)ΔH = -390 kJ IF (g) + 2F₂ (g) → IF₅ (g)ΔH = -745 kJ

The value of ΔH° for the reaction below is -482 kJ. Calculate the heat (kJ)released to the surroundings when 10.0 g of CO (g)reacts completely. 2CO (g) + O₂ (g) → 2CO₂ (g)

An 6.11 g sample of calcium carbonate [CaCO₃ (s)] absorbs 84 J of heat, upon which the temperature of the sample increases from 19.2 °C to 35.9 °C. What is the specific heat of calcium carbonate?

The value of ΔH° for the reaction below is -790 kJ. The enthalpy change accompanying the reaction of 0.95 g of S is ________ kJ. 2S (s) + 3O₂ (g) → 2SO₃ (g)

Given the data in the table below, ΔH°_rxn for the reaction 2SO₂ (g) + O₂ (g) → 2SO₃ (g) Is ________ kJ.