Question 1

All of the following are considered fossil fuels except ________.

Accepted Answer

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

Question 2

Given the following reactions 2S (s)+ 3O2 (g)→ 2SO3 (g)ΔH = -790 kJ
S (s)+ O2 (g)→ SO2(g)ΔH = -297 kJ
The enthalpy of the reaction in which sulfur dioxide is oxidized to sulfur trioxide
2SO2 (g)+ O2 (g)→ 2SO3 (g)
Is ________ kJ.

Accepted Answer

A) 196 
B) -196 
C) 1087 
D) -1384 
E) -543 
A) 196 
B) -196 
C) 1087 
D) -1384 
E) -543

Question 3

Given the following reactions N2 (g)+ 2O2 (g)→ 2NO2 (g)ΔH = 66.4 kJ
2NO (g)+ O2 (g)→ 2NO2 (g)ΔH = -114.2 kJ
The enthalpy of the reaction of the nitrogen to produce nitric oxide
N2 (g)+ O2 (g)→ 2NO (g)
Is ________ kJ.

Accepted Answer

A) 180.6 
B) -47.8 
C) 47.8 
D) 90.3 
E) -180.6 
A) 180.6 
B) -47.8 
C) 47.8 
D) 90.3 
E) -180.6

Question 4

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 5

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)△H = -890.0 kJ
Calculate the value of q (kJ)in this exothermic reaction when 1.80 g of methane is combusted at constant pressure.

Accepted Answer

A) -100.1 kJ 
B) 0.0324 kJ 
C) -0.0100 kJ 
D) 30.9 kJ 
E) -1.00 × 105 kJ 
A) -100.1 kJ 
B) 0.0324 kJ 
C) -0.0100 kJ 
D) 30.9 kJ 
E) -1.00 × 105 kJ

Question 6

The term Btu which stands for ________ is commonly used in engineering applications.

Accepted Answer

A) Best thermal unit 
B) Bunsen thermal unit 
C) British thermal unit 
D) Bake thermal unit 
E) Brush thermal unit 
A) Best thermal unit 
B) Bunsen thermal unit 
C) British thermal unit 
D) Bake thermal unit 
E) Brush thermal unit

Question 7

How much heat is required to raise the temperature of a 1.15 kg piece of copper metal from 25.0 °C to 77.5 °C? The specific heat capacity of solid copper metal is 0.385 J/g-K.

Accepted Answer

A) 2.32 ×   J 
B) 1.57 ×   J 
C) 23.2 J 
D) 6.38 ×   J 
E) 0.00638 J 
A) 2.32 ×   J 
B) 1.57 ×   J 
C) 23.2 J 
D) 6.38 ×   J 
E) 0.00638 J

Question 8

A 100-watt electric incandescent light bulb consumes ________ J of energy in 24 hours.[1 Watt (W)= 1 J/sec]

Accepted Answer

A) 2.40 × 103 
B) 8.64 × 103 
C) 4.17 
D) 2.10 × 103 
E) 8.64 × 106 
A) 2.40 × 103 
B) 8.64 × 103 
C) 4.17 
D) 2.10 × 103 
E) 8.64 × 106

Question 9

The value of ΔH° for the reaction below is +128.1 kJ: CH3OH (l)→ CO (g)+ 2H2 (g)
How many kJ of heat are consumed when 5.10 g of CO (g)is formed as shown in the equation?

Accepted Answer

A) 0.182 kJ 
B) 162 kJ 
C) 8.31 kJ 
D) 23.3 kJ 
E) 62.0 kJ 
A) 0.182 kJ 
B) 162 kJ 
C) 8.31 kJ 
D) 23.3 kJ 
E) 62.0 kJ

Question 10

The temperature of a 15-g sample of lead metal increases from 22 °C to 37 °C upon the addition of 29.0 J of heat.The specific heat capacity of the lead is ________ J/g-K.

Accepted Answer

A) 7.8 
B) 1.9 
C) 29 
D) 0.13 
E) -29 
A) 7.8 
B) 1.9 
C) 29 
D) 0.13 
E) -29

Question 11

Given the following reactions N2 (g)+ O2 (g)→ 2NO (g)ΔH = +180.7 kJ
2NO (g)+ O2(g)→ 2N   (g)ΔH = -113.1 kJ
The enthalpy of reaction for
4NO (g)→ 2NO2 (g)+ N2 (g)
Is ________ kJ.

Accepted Answer

A) 67.6 
B) 45.5 
C) -293.8 
D) -45.5 
E) 293.8 
A) 67.6 
B) 45.5 
C) -293.8 
D) -45.5 
E) 293.8

Question 12

A typical fast food meal consists of a burger,fries,and a soft-drink and contains 58.0 grams of fat,39.0 grams of protein,and 177 grams of carbohydrate.If jogging burns 950.0 kJ/hour,how many minutes would it take to completely burn off the meal? The respective fuel values for protein,fat,and carbohydrate are 17,38,and 17 kJ/g,respectively.

Accepted Answer

A) 6.19 
B) 208 
C) 371 
D) 17.3 
E) 9.70 
A) 6.19 
B) 208 
C) 371 
D) 17.3 
E) 9.70

Question 13

Given the data in the table below,ΔH°rxn for the reaction IF5 (g)+ F2 (g)→ IF7 (g)
Is ________ kJ.

Accepted Answer

A) 1801 
B) -1801 
C) 121 
D) -121 
E) -101 
A) 1801 
B) -1801 
C) 121 
D) -121 
E) -101

Question 14

A 26.9 g rock rolls down the hill at a speed of 81.9 m/s .What is the kinetic energy of the rock?

Accepted Answer

A) 90.2 J 
B) 145 J 
C) 0.950 J 
D) 90200 J 
E) 1450 J 
A) 90.2 J 
B) 145 J 
C) 0.950 J 
D) 90200 J 
E) 1450 J

Question 15

How many joules of heat are absorbed when the temperature of a 13.9 g sample of CaCO3 (s)increases from   to   Specific heat of calcium carbonate is

Accepted Answer

A) 130 J 
B) 0.68 J 
C) s-130 J 
D) -0.68 J 
E) 9.5 J 
A) 130 J 
B) 0.68 J 
C) s-130 J 
D) -0.68 J 
E) 9.5 J

Question 16

Which of the following is a statement of Hess's law?

Accepted Answer

A) If a reaction is carried out in a series of steps, the ΔH for the reaction will equal the sum of the enthalpy changes for the individual steps. 
B) If a reaction is carried out in a series of steps, the ΔH for the reaction will equal the product of the enthalpy changes for the individual steps. 
C) The ΔH for a process in the forward direction is equal in magnitude and opposite in sign to the ΔH for the process in the reverse direction. 
D) The ΔH for a process in the forward direction is equal to the ΔH for the process in the reverse direction. 
E) The ΔH of a reaction depends on the physical states of the reactants and products. 
A) If a reaction is carried out in a series of steps, the ΔH for the reaction will equal the sum of the enthalpy changes for the individual steps. 
B) If a reaction is carried out in a series of steps, the ΔH for the reaction will equal the product of the enthalpy changes for the individual steps. 
C) The ΔH for a process in the forward direction is equal in magnitude and opposite in sign to the ΔH for the process in the reverse direction. 
D) The ΔH for a process in the forward direction is equal to the ΔH for the process in the reverse direction. 
E) The ΔH of a reaction depends on the physical states of the reactants and products.

Question 17

The change in the internal energy of a system that absorbs 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) -5,155 
D) -10,155 
E) 1.91 × 107 
A) 10,155 
B) 5,155 
C) -5,155 
D) -10,155 
E) 1.91 × 107

Question 18

The value of ΔH° for the following reaction is 177.8 kJ.The value of Δ   for CaO(s)is ________ kJ/mol. CaCO3 (s)→ CaO (s)+ CO2 (g)

Accepted Answer

A) -1600 
B) -813.4 
C) -635.5 
D) 813.4 
E) 177.8 
A) -1600 
B) -813.4 
C) -635.5 
D) 813.4 
E) 177.8

Question 19

Of the following,ΔH°f is not zero for ________.

Accepted Answer

A) Sc (g) 
B) Si (s) 
C) P4 (s, white) 
D) Br2 (l) 
E) Ca (s) 
A) Sc (g) 
B) Si (s) 
C) P4 (s, white) 
D) Br2 (l) 
E) Ca (s)

Question 20

The temperature of a 24.3 g sample of gold increases from   to   If the specific heat of gold is   how many joules of heat are absorbed?

Accepted Answer

A) 24.5 J 
B) 0.0414 J 
C) -24.5 J 
D) 0.293 J 
E) 1.01 J 
A) 24.5 J 
B) 0.0414 J 
C) -24.5 J 
D) 0.293 J 
E) 1.01 J

Exam 5: Thermochemistry

All of the following are considered fossil fuels except ________.

Given the following reactions 2S (s)+ 3O2 (g)→ 2SO3 (g)ΔH = -790 kJ S (s)+ O2 (g)→ SO2(g)ΔH = -297 kJ The enthalpy of the reaction in which sulfur dioxide is oxidized to sulfur trioxide 2SO2 (g)+ O2 (g)→ 2SO3 (g) Is ________ kJ.

Given the following reactions N2 (g)+ 2O2 (g)→ 2NO2 (g)ΔH = 66.4 kJ 2NO (g)+ O2 (g)→ 2NO2 (g)ΔH = -114.2 kJ The enthalpy of the reaction of the nitrogen to produce nitric oxide N2 (g)+ O2 (g)→ 2NO (g) Is ________ kJ.

Given the data in the table below,ΔH°rxn for the reaction 2SO2 (g)+ O2 (g)→ 2SO3 (g) Is ________ 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)△H = -890.0 kJ Calculate the value of q (kJ)in this exothermic reaction when 1.80 g of methane is combusted at constant pressure.

The term Btu which stands for ________ is commonly used in engineering applications.

How much heat is required to raise the temperature of a 1.15 kg piece of copper metal from 25.0 °C to 77.5 °C? The specific heat capacity of solid copper metal is 0.385 J/g-K.

A 100-watt electric incandescent light bulb consumes ________ J of energy in 24 hours.[1 Watt (W)= 1 J/sec]

The value of ΔH° for the reaction below is +128.1 kJ: CH3OH (l)→ CO (g)+ 2H2 (g) How many kJ of heat are consumed when 5.10 g of CO (g)is formed as shown in the equation?

The temperature of a 15-g sample of lead metal increases from 22 °C to 37 °C upon the addition of 29.0 J of heat.The specific heat capacity of the lead is ________ J/g-K.

Given the following reactions N2 (g)+ O2 (g)→ 2NO (g)ΔH = +180.7 kJ 2NO (g)+ O2(g)→ 2N (g)ΔH = -113.1 kJ The enthalpy of reaction for 4NO (g)→ 2NO2 (g)+ N2 (g) Is ________ kJ.

Given the data in the table below,ΔH°rxn for the reaction IF5 (g)+ F2 (g)→ IF7 (g) Is ________ kJ.

A 26.9 g rock rolls down the hill at a speed of 81.9 m/s .What is the kinetic energy of the rock?

How many joules of heat are absorbed when the temperature of a 13.9 g sample of CaCO3 (s)increases from to Specific heat of calcium carbonate is

Which of the following is a statement of Hess's law?

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

The value of ΔH° for the following reaction is 177.8 kJ.The value of Δ for CaO(s)is ________ kJ/mol. CaCO3 (s)→ CaO (s)+ CO2 (g)

Of the following,ΔH°f is not zero for ________.

The temperature of a 24.3 g sample of gold increases from to If the specific heat of gold is how many joules of heat are absorbed?

Introduction: Matter, energy, and Measurement

Atoms, molecules, and Ions

Chemical Reactions and Reaction Stoichiometry

Reactions in Aqueous Solution

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

Given the following reactions 2S (s)+ 3O₂ (g)→ 2SO₃ (g)ΔH = -790 kJ S (s)+ O₂ (g)→ SO₂(g)ΔH = -297 kJ The enthalpy of the reaction in which sulfur dioxide is oxidized to sulfur trioxide 2SO₂ (g)+ O₂ (g)→ 2SO₃ (g) Is ________ kJ.

Given the following reactions N₂ (g)+ 2O₂ (g)→ 2NO₂ (g)ΔH = 66.4 kJ 2NO (g)+ O₂(g)→ 2NO₂ (g)ΔH = -114.2 kJ The enthalpy of the reaction of the nitrogen to produce nitric oxide N₂ (g)+ O₂ (g)→ 2NO (g) Is ________ kJ.

Given the data in the table below,ΔH°_rxn for the reaction 2SO₂ (g)+ O₂ (g)→ 2SO₃ (g) Is ________ 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)△H = -890.0 kJ Calculate the value of q (kJ)in this exothermic reaction when 1.80 g of methane is combusted at constant pressure.

The value of ΔH° for the reaction below is +128.1 kJ: CH₃OH (l)→ CO (g)+ 2H₂ (g) How many kJ of heat are consumed when 5.10 g of CO (g)is formed as shown in the equation?

Given the following reactions N₂ (g)+ O₂ (g)→ 2NO (g)ΔH = +180.7 kJ 2NO (g)+ O₂(g)→ 2N (g)ΔH = -113.1 kJ The enthalpy of reaction for 4NO (g)→ 2NO₂ (g)+ N₂ (g) Is ________ kJ.

Given the data in the table below,ΔH°_rxn for the reaction IF₅ (g)+ F₂ (g)→ IF₇ (g) Is ________ kJ.

How many joules of heat are absorbed when the temperature of a 13.9 g sample of CaCO₃ (s)increases from to Specific heat of calcium carbonate is

The value of ΔH° for the following reaction is 177.8 kJ.The value of Δ for CaO(s)is ________ kJ/mol. CaCO₃ (s)→ CaO (s)+ CO₂ (g)

Of the following,ΔH°_f is not zero for ________.