Question 1

Calculate the kinetic energy in joules of an 80.0 g bullet traveling at 300.0 m/s.

Accepted Answer

A) 3.60 × 106 J 
B) 1.20 × 104 J 
C) 3.60 × 103 J 
D) 12.0 J 
E) 80.0 J 
A) 3.60 × 106 J 
B) 1.20 × 104 J 
C) 3.60 × 103 J 
D) 12.0 J 
E) 80.0 J

Question 2

The value of ΔH° for the following reaction is -3351 kJ: 2Al (s) + 3O2 (g) → 2Al2O3 (s)
The value of ΔH°f for Al2O3 (s)is ________ kJ.

Accepted Answer

A) -3351 
B) -1676 
C) -32.86 
D) -16.43 
E) +3351 
A) -3351 
B) -1676 
C) -32.86 
D) -16.43 
E) +3351

Question 3

Given the following reactions N2 (g) + O2 (g) → 2NO (g)ΔH = +180.7 kJ
2NO (g) + O2 (g) → 2NO2 (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 4

Given the equation:
CH4 (g)+ 2 O2 (g)→ CO2 (g)+ H2O (l)ΔH = -890.0 kJ
The heat liberated when 34.78 grams of methane (CH4)are burned in an excess amount of oxygen is ________ kJ.

Accepted Answer

Question 5

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 5.75 g of CO (g)is formed as shown in the equation?

Accepted Answer

A) 23.3 kJ 
B) 62.0 kJ 
C) 26.3 kJ 
D) 162 kJ 
E) 8.3 kJ 
A) 23.3 kJ 
B) 62.0 kJ 
C) 26.3 kJ 
D) 162 kJ 
E) 8.3 kJ

Question 6

________ is defined as the energy used to move an object against a force.

Accepted Answer

The answer of ________ is defined as the energy used...

Question 7

The value of ΔH° for the following reaction is 177.8 kJ. The value of ΔH°f 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 8

The internal energy of a system is always increased by ________.

Accepted Answer

A) adding heat to the system 
B) having the system do work on the surroundings 
C) withdrawing heat from the system 
D) adding heat to the system and having the system do work on the surroundings 
E) a volume compression 
A) adding heat to the system 
B) having the system do work on the surroundings 
C) withdrawing heat from the system 
D) adding heat to the system and having the system do work on the surroundings 
E) a volume compression

Question 9

Given the equation
H2O (l)→ H2O (g)ΔHrxn = 40.7 kJ at 100 °C
Calculate the heat required to convert 3.00 grams of liquid water at 100 °C to vapor.

Accepted Answer

Question 10

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 7.25 g of methane from 22.0 °C to 57.0 °C?

Accepted Answer

A) 115 J 
B) 558 J 
C) 1.26 × 103 J 
D) 8.67 × 10-3 J 
E) 41.3 J 
A) 115 J 
B) 558 J 
C) 1.26 × 103 J 
D) 8.67 × 10-3 J 
E) 41.3 J

Question 11

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 12

Given the data in the table below, ΔH°rxn for the reaction 3 Cl2 (g) + PH3 (g) → PCl3 (g) + 3 HCl (g)
Is ________ kJ.

Accepted Answer

A) -385.77 
B) -570.37 
C) 570.37 
D) 385.77 
E) The ΔH°f of Cl2 (g)is needed for the calculation. 
A) -385.77 
B) -570.37 
C) 570.37 
D) 385.77 
E) The ΔH°f of Cl2 (g)is needed for the calculation.

Question 13

A 4.50-g sample of liquid water at 25.0 °C is heated by the addition of 133 J of energy. The final temperature of the water is ________ °C. The specific heat capacity of liquid water is 4.18 J/g-K.

Accepted Answer

A) 149 
B) 25.1 
C) -17.9 
D) 32.1 
E) 7.07 
A) 149 
B) 25.1 
C) -17.9 
D) 32.1 
E) 7.07

Question 14

Given the data in the table below, ΔH°rxn for the reaction PCl3 (g) + 3 HCl (g) → 3Cl2 (g) + PH3 (g)
Is ________ kJ.

Accepted Answer

A) -570.37 
B) -385.77 
C) 570.37 
D) 385.77 
E) The ΔH°f of Cl2 (g)is needed for the calculation. 
A) -570.37 
B) -385.77 
C) 570.37 
D) 385.77 
E) The ΔH°f of Cl2 (g)is needed for the calculation.

Calculate the kinetic energy in joules of an 80.0 g bullet traveling at 300.0 m/s.

The value of ΔH° for the following reaction is -3351 kJ: 2Al (s) + 3O₂ (g) → 2Al₂O₃ (s) The value of ΔH°_f for Al₂O₃ (s)is ________ kJ.

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

Given the equation: CH₄ (g)+ 2 O₂ (g)→ CO₂ (g)+ H₂O (l)ΔH = -890.0 kJ The heat liberated when 34.78 grams of methane (CH₄)are burned in an excess amount of oxygen is ________ kJ.

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 5.75 g of CO (g)is formed as shown in the equation?

________ is defined as the energy used to move an object against a force.

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

The internal energy of a system is always increased by ________.

Given the equation H₂O (l)→ H₂O (g)ΔH_rxn= 40.7 kJ at 100 °C Calculate the heat required to convert 3.00 grams of liquid water at 100 °C to vapor.

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 7.25 g of methane from 22.0 °C to 57.0 °C?

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 data in the table below, ΔH°_rxn for the reaction 3 Cl₂ (g) + PH₃ (g) → PCl₃ (g) + 3 HCl (g) Is ________ kJ.

A 4.50-g sample of liquid water at 25.0 °C is heated by the addition of 133 J of energy. The final temperature of the water is ________ °C. The specific heat capacity of liquid water is 4.18 J/g-K.

Given the data in the table below, ΔH°_rxn for the reaction PCl₃ (g) + 3 HCl (g) → 3Cl₂ (g) + PH₃ (g) Is ________ kJ.

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

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Exam 5: Thermochemistry

Calculate the kinetic energy in joules of an 80.0 g bullet traveling at 300.0 m/s.

The value of ΔH° for the following reaction is -3351 kJ: 2Al (s) + 3O2 (g) → 2Al2O3 (s) The value of ΔH°f for Al2O3 (s)is ________ kJ.

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

Given the equation: CH4 (g)+ 2 O2 (g)→ CO2 (g)+ H2O (l)ΔH = -890.0 kJ The heat liberated when 34.78 grams of methane (CH4)are burned in an excess amount of oxygen is ________ kJ.

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 5.75 g of CO (g)is formed as shown in the equation?

________ is defined as the energy used to move an object against a force.

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

The internal energy of a system is always increased by ________.

Given the equation H2O (l)→ H2O (g)ΔHrxn = 40.7 kJ at 100 °C Calculate the heat required to convert 3.00 grams of liquid water at 100 °C to vapor.

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 7.25 g of methane from 22.0 °C to 57.0 °C?

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 data in the table below, ΔH°rxn for the reaction 3 Cl2 (g) + PH3 (g) → PCl3 (g) + 3 HCl (g) Is ________ kJ.

A 4.50-g sample of liquid water at 25.0 °C is heated by the addition of 133 J of energy. The final temperature of the water is ________ °C. The specific heat capacity of liquid water is 4.18 J/g-K.

Given the data in the table below, ΔH°rxn for the reaction PCl3 (g) + 3 HCl (g) → 3Cl2 (g) + PH3 (g) Is ________ kJ.

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

The value of ΔH° for the following reaction is -3351 kJ: 2Al (s) + 3O₂ (g) → 2Al₂O₃ (s) The value of ΔH°_f for Al₂O₃ (s)is ________ kJ.

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

Given the equation: CH₄ (g)+ 2 O₂ (g)→ CO₂ (g)+ H₂O (l)ΔH = -890.0 kJ The heat liberated when 34.78 grams of methane (CH₄)are burned in an excess amount of oxygen is ________ kJ.

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 5.75 g of CO (g)is formed as shown in the equation?

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

Given the equation H₂O (l)→ H₂O (g)ΔH_rxn= 40.7 kJ at 100 °C Calculate the heat required to convert 3.00 grams of liquid water at 100 °C to vapor.

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 data in the table below, ΔH°_rxn for the reaction 3 Cl₂ (g) + PH₃ (g) → PCl₃ (g) + 3 HCl (g) Is ________ kJ.

Given the data in the table below, ΔH°_rxn for the reaction PCl₃ (g) + 3 HCl (g) → 3Cl₂ (g) + PH₃ (g) Is ________ kJ.