Question 1

How much energy is evolved during the formation of 98.7 g of Fe according to the reaction below? Fe2O3(s)+ 2Al(s)→ Al2O3(s)+ 2Fe(s)ΔrH° = -852 kJ

Accepted Answer

A) 753 kJ 
B) 1.51 × 103 kJ 
C) 4.20 × 103 kJ 
D) 482 kJ 
E) 241 kJ 
A) 753 kJ 
B) 1.51 × 103 kJ 
C) 4.20 × 103 kJ 
D) 482 kJ 
E) 241 kJ

Question 2

Give the temperature and pressure for the standard state for a liquid.

Accepted Answer

The answer of Give the temperature and pressure for the...

Question 3

Calculate the mass of NH4ClO4, molar mass = 117.49 g mol-1, required to create a temperature change of -1.0 °C in a coffee cup calorimeter containing 115 mL of water. The enthalpy of solution for NH4ClO4 is 33.47 kJ mol-1. The specific heat of water is 4.184 J g-1 °C-1, and assume the density of the solution is 1.00 g mL-1.

Accepted Answer

A) 1.7 g 
B) 3.2 g 
C) 2.8 g 
D) 4.0 g 
E) 0.83 g 
A) 1.7 g 
B) 3.2 g 
C) 2.8 g 
D) 4.0 g 
E) 0.83 g

Question 4

Calculate the heat transfer (J)when 3.15 g of platinum (specific heat capacity = 0.133 J g-1 °C-1)at 86.1 °C cools to room temperature, 24.3 °C.

Accepted Answer

A) -26 J 
B) 26 J 
C) -60 J 
D) 60 J 
E) -17 J 
A) -26 J 
B) 26 J 
C) -60 J 
D) 60 J 
E) -17 J

Question 5

A chemist wishes to calibrate a bomb calorimeter, so he combusts 7.529 g of D-galactose, ΔcombustionU = -15.48 kJ g-1, which causes a temperature change from 26.38 °C to 34.60 °C. What should the chemist report for the value of Ccal?

Accepted Answer

A) 24.34 kJ °C-1 
B) 8.009 kJ °C-1 
C) 14.18 kJ °C-1 
D) 16.67 kJ °C-1 
E) 9.170 kJ °C-1 
A) 24.34 kJ °C-1 
B) 8.009 kJ °C-1 
C) 14.18 kJ °C-1 
D) 16.67 kJ °C-1 
E) 9.170 kJ °C-1

Question 6

A 5.00 g sample of liquid water at 25.0 °C is heated by the addition of 145 J of energy. The final temperature of the water is ________ °C. The specific heat capacity of liquid water is 4.184 J g-1 K-1.

Accepted Answer

A) 146 
B) 25.1 
C) -18.1 
D) 31.9 
E) 6.94 
A) 146 
B) 25.1 
C) -18.1 
D) 31.9 
E) 6.94

Question 7

Define molar heat capacity.

Accepted Answer

A) the quantity of heat required to raise the temperature of 1 mol of a substance by 1 °C 
B) the quantity of heat required to change a system's temperature by 1 °C 
C) the quantity of heat required to raise the temperature of 1 g of a substance by 1 °C 
D) the quantity of heat required to raise the temperature of 1 g of a substance by 1 °F 
E) the quantity of heat required to raise the temperature of 1 L of a substance by 1 °C 
A) the quantity of heat required to raise the temperature of 1 mol of a substance by 1 °C 
B) the quantity of heat required to change a system's temperature by 1 °C 
C) the quantity of heat required to raise the temperature of 1 g of a substance by 1 °C 
D) the quantity of heat required to raise the temperature of 1 g of a substance by 1 °F 
E) the quantity of heat required to raise the temperature of 1 L of a substance by 1 °C

Question 8

How much heat is absorbed when 50.00 g of C(s)reacts in the presence of excess SO2(g)to produce CS2(l)and CO(g)according to the following chemical equation? 5C(s)+ 2SO2(g)→ CS2(l)+ 4CO(g)ΔrH° = 239.9 kJ

Accepted Answer

A) 199.7 kJ mol-1 
B) 239.9 kJ mol-1 
C) 998.3 kJ mol-1 
D) 2398 kJ mol-1 
A) 199.7 kJ mol-1 
B) 239.9 kJ mol-1 
C) 998.3 kJ mol-1 
D) 2398 kJ mol-1

Question 9

An unknown metal alloy, mass = 26.3 g, has a temperature increase of 8.31 °C after a heat transfer of 94.0 J. Calculate the specific heat capacity of the alloy.

Accepted Answer

A) 0.813 J g-1 °C-1 
B) 0.517 J g-1 °C-1 
C) 0.349 J g-1 °C-1 
D) 0.288 J g-1 °C-1 
E) 0.430 J g-1 °C-1 
A) 0.813 J g-1 °C-1 
B) 0.517 J g-1 °C-1 
C) 0.349 J g-1 °C-1 
D) 0.288 J g-1 °C-1 
E) 0.430 J g-1 °C-1

Question 10

Use the standard reaction enthalpies given below to determine ΔrH° for the following reaction: 2NO(g)+ O2(g)→ 2NO2(g)ΔrH° = ?
Given:
N2(g)+ O2(g)→ 2NO(g)ΔrH° = +183 kJ
1/2 N2(g)+ O2(g)→ NO2(g)ΔrH° = +33 kJ

Accepted Answer

A) -150. kJ mol-1 
B) -117 kJ mol-1 
C) -333 kJ mol-1 
D) +115 kJ mol-1 
E) +238 kJ mol-1 
A) -150. kJ mol-1 
B) -117 kJ mol-1 
C) -333 kJ mol-1 
D) +115 kJ mol-1 
E) +238 kJ mol-1

Question 11

When 1.50 mol of CH4(g)reacts with excess Cl2(g)at constant pressure according to the chemical equation shown below, 1062 kJ of heat are released. Calculate the value of ΔH for this reaction, as written. 2CH4(g)+ 3Cl2(g)→ 2CHCl3(l)+ 3H2(g)ΔrH° = ?

Accepted Answer

A) -1420 kJ mol-1 
B) -708 kJ mol-1 
C) +708 kJ mol-1 
D) +1420 kJ mol-1 
A) -1420 kJ mol-1 
B) -708 kJ mol-1 
C) +708 kJ mol-1 
D) +1420 kJ mol-1

Question 12

Determine the specific heat capacity of an alloy that requires 59.3 kJ to raise the temperature of 150.0 g alloy from 298 K to 398 K.

Accepted Answer

A) 4.38 J g-1 °C-1 
B) 2.29 J g-1 °C-1 
C) 3.95 J g-1 °C-1 
D) 2.53 J g-1 °C-1 
E) 1.87 J g-1 °C-1 
A) 4.38 J g-1 °C-1 
B) 2.29 J g-1 °C-1 
C) 3.95 J g-1 °C-1 
D) 2.53 J g-1 °C-1 
E) 1.87 J g-1 °C-1

Question 13

A 6.55 g sample of aniline (C6H5NH2, molar mass = 93.13 g mol-1)was combusted in a bomb calorimeter with a heat capacity of 14.25 kJ °C-1. If the initial temperature was 32.9 °C, use the information below to determine the value of the final temperature of the calorimeter. 4C6H5NH2(l)+ 35O2(g)→ 24CO2(g)+ 14H2O(g)+ 4NO2(g)
ΔrU° = -1.28 × 104 kJ mol-1

Accepted Answer

A) 257 °C 
B) 46.6 °C 
C) 96.1 °C 
D) 41.9 °C 
E) 931 °C 
A) 257 °C 
B) 46.6 °C 
C) 96.1 °C 
D) 41.9 °C 
E) 931 °C

Question 14

A 21.8 g sample of ethanol (C2H5OH)is burned in a bomb calorimeter according to the following reaction. If the temperature rises from 25.0 °C to 62.3 °C, determine the heat capacity of the calorimeter. The molar mass of ethanol is 46.07 g mol-1. C2H5OH(l)+ 3O2(g)→ 2CO2(g)+ 3H2O(g)ΔrU = -1235 kJ mol-1

Accepted Answer

A) 4.99 kJ °C-1 
B) 5.65 kJ °C-1 
C) 63.7 kJ °C-1 
D) 33.1 kJ °C-1 
E) 15.7 kJ °C-1 
A) 4.99 kJ °C-1 
B) 5.65 kJ °C-1 
C) 63.7 kJ °C-1 
D) 33.1 kJ °C-1 
E) 15.7 kJ °C-1

Question 15

A 6.55 g sample of aniline (C6H5NH2, molar mass = 93.13 g mol-1)was combusted in a bomb calorimeter. If the temperature rose by 32.9 °C, use the information below to determine the heat capacity of the calorimeter. 4C6H5NH2(l)+ 35O2(g)? 24CO2(g)+ 14H2O(g)+ 4NO2(g)
$\Delta$rU= -3.20 × 103 kJ mol-1

Accepted Answer

A) 97.3 kJ °C-1 
B) 38.9 kJ °C-1 
C) 5.94 kJ °C-1 
D) 6.84 kJ °C-1 
E) 12.8 kJ °C-1 
A) 97.3 kJ °C-1 
B) 38.9 kJ °C-1 
C) 5.94 kJ °C-1 
D) 6.84 kJ °C-1 
E) 12.8 kJ °C-1

Question 16

Calculate the amount of heat (in kJ)necessary to raise the temperature of 47.8 g benzene by 57.0 K. The specific heat capacity of benzene is 1.05 J g-1 °C-1.

Accepted Answer

A) 1.61 kJ 
B) 16.6 kJ 
C) 2.59 kJ 
D) 2.86 kJ 
E) 3.85 kJ 
A) 1.61 kJ 
B) 16.6 kJ 
C) 2.59 kJ 
D) 2.86 kJ 
E) 3.85 kJ

Question 17

Calculate the initial temperature of 448 g of grapes (specific heat capacity = 1.76 J g-1 °C-1)that absorb 17472 J of heat while warming up to room temperature, 23.1 °C.

Accepted Answer

A) 3.15 °C 
B) 0.941 °C 
C) -13.5 °C 
D) 8.49 °C 
E) 5.23 °C 
A) 3.15 °C 
B) 0.941 °C 
C) -13.5 °C 
D) 8.49 °C 
E) 5.23 °C

Question 18

When 2.50 g of Ba(s)is added to 100.00 g of water in a container open to the atmosphere, the reaction shown below occurs and the temperature of the resulting solution rises from 22.00 °C to 40.32 °C. If the specific heat of the solution is 4.18 J g-1°C-1, calculate ΔH for the reaction, as written. Ba(s)+ 2H2O(l)→ Ba(OH)2(aq)+ H2(g)ΔrH = ?

Accepted Answer

A) -431 kJ mol-1 
B) -3.14 kJ mol-1 
C) +3.14 kJ mol-1 
D) +431 kJ mol-1 
A) -431 kJ mol-1 
B) -3.14 kJ mol-1 
C) +3.14 kJ mol-1 
D) +431 kJ mol-1

Question 19

The combustion of titanium with oxygen produces titanium dioxide: Ti(s)+ O2(g)→ TiO2(s)
When 2.060 g of titanium is combusted in a bomb calorimeter, the temperature of the calorimeter increases from 25.00 °C to 91.60 °C. In a separate experiment, the heat capacity of the calorimeter is measured to be 9.84 kJ K-1. The heat of reaction for the combustion of a mole of Ti in this calorimeter is ________ kJ mol-1.

Accepted Answer

A) 14.3 
B) 19.6 
C) -311 
D) -0.154 
E) -1.52 × 104 
A) 14.3 
B) 19.6 
C) -311 
D) -0.154 
E) -1.52 × 104

Question 20

An unknown metal alloy, mass = 36.1 g, has a temperature change of 31.6 to 24.8 °C after a heat transfer of -103.0 J. Calculate the specific heat capacity of the alloy.

Accepted Answer

A) 0.500 J g-1 °C-1 
B) 0.384 J g-1 °C-1 
C) 0.579 J g-1 °C-1 
D) 0.420 J g-1 °C-1 
E) 1.85 J g-1 °C-1 
A) 0.500 J g-1 °C-1 
B) 0.384 J g-1 °C-1 
C) 0.579 J g-1 °C-1 
D) 0.420 J g-1 °C-1 
E) 1.85 J g-1 °C-1

How much energy is evolved during the formation of 98.7 g of Fe according to the reaction below? Fe₂O₃(s)+ 2Al(s)→ Al₂O₃(s)+ 2Fe(s)Δ_rH°= -852 kJ

Give the temperature and pressure for the standard state for a liquid.

Calculate the heat transfer (J)when 3.15 g of platinum (specific heat capacity = 0.133 J g^-1 °C^-1)at 86.1 °C cools to room temperature, 24.3 °C.

A chemist wishes to calibrate a bomb calorimeter, so he combusts 7.529 g of D-galactose, Δ_combustionU = -15.48 kJ g^-1, which causes a temperature change from 26.38 °C to 34.60 °C. What should the chemist report for the value of C_cal?

A 5.00 g sample of liquid water at 25.0 °C is heated by the addition of 145 J of energy. The final temperature of the water is ________ °C. The specific heat capacity of liquid water is 4.184 J g^-1 K^-1.

Define molar heat capacity.

How much heat is absorbed when 50.00 g of C(s)reacts in the presence of excess SO₂(g)to produce CS₂(l)and CO(g)according to the following chemical equation? 5C(s)+ 2SO₂(g)→ CS₂(l)+ 4CO(g)Δ_rH° = 239.9 kJ

An unknown metal alloy, mass = 26.3 g, has a temperature increase of 8.31 °C after a heat transfer of 94.0 J. Calculate the specific heat capacity of the alloy.

Use the standard reaction enthalpies given below to determine Δ_rH° for the following reaction: 2NO(g)+ O₂(g)→ 2NO₂(g)Δ_rH°= ? Given: N₂(g)+ O₂(g)→ 2NO(g)Δ_rH°= +183 kJ 1/2 N₂(g)+ O₂(g)→ NO₂(g)Δ_rH°= +33 kJ

When 1.50 mol of CH₄(g)reacts with excess Cl₂(g)at constant pressure according to the chemical equation shown below, 1062 kJ of heat are released. Calculate the value of ΔH for this reaction, as written. 2CH₄(g)+ 3Cl₂(g)→ 2CHCl₃(l)+ 3H₂(g)Δ_rH° = ?

Determine the specific heat capacity of an alloy that requires 59.3 kJ to raise the temperature of 150.0 g alloy from 298 K to 398 K.

Calculate the amount of heat (in kJ)necessary to raise the temperature of 47.8 g benzene by 57.0 K. The specific heat capacity of benzene is 1.05 J g^-1 °C^-1.

Calculate the initial temperature of 448 g of grapes (specific heat capacity = 1.76 J g^-1 °C^-1)that absorb 17472 J of heat while warming up to room temperature, 23.1 °C.

An unknown metal alloy, mass = 36.1 g, has a temperature change of 31.6 to 24.8 °C after a heat transfer of -103.0 J. Calculate the specific heat capacity of the alloy.

Units of Measurement for Physical and Chemical Change

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Chemical Reactions and Stoichiometry

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Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

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Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry II: Reactions

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Exam 6: Thermochemistry

How much energy is evolved during the formation of 98.7 g of Fe according to the reaction below? Fe2O3(s)+ 2Al(s)→ Al2O3(s)+ 2Fe(s)ΔrH° = -852 kJ

Give the temperature and pressure for the standard state for a liquid.

Calculate the heat transfer (J)when 3.15 g of platinum (specific heat capacity = 0.133 J g-1 °C-1)at 86.1 °C cools to room temperature, 24.3 °C.

A chemist wishes to calibrate a bomb calorimeter, so he combusts 7.529 g of D-galactose, ΔcombustionU = -15.48 kJ g-1, which causes a temperature change from 26.38 °C to 34.60 °C. What should the chemist report for the value of Ccal?

A 5.00 g sample of liquid water at 25.0 °C is heated by the addition of 145 J of energy. The final temperature of the water is ________ °C. The specific heat capacity of liquid water is 4.184 J g-1 K-1.

Define molar heat capacity.

How much heat is absorbed when 50.00 g of C(s)reacts in the presence of excess SO2(g)to produce CS2(l)and CO(g)according to the following chemical equation? 5C(s)+ 2SO2(g)→ CS2(l)+ 4CO(g)ΔrH° = 239.9 kJ

An unknown metal alloy, mass = 26.3 g, has a temperature increase of 8.31 °C after a heat transfer of 94.0 J. Calculate the specific heat capacity of the alloy.

Use the standard reaction enthalpies given below to determine ΔrH° for the following reaction: 2NO(g)+ O2(g)→ 2NO2(g)ΔrH° = ? Given: N2(g)+ O2(g)→ 2NO(g)ΔrH° = +183 kJ 1/2 N2(g)+ O2(g)→ NO2(g)ΔrH° = +33 kJ

When 1.50 mol of CH4(g)reacts with excess Cl2(g)at constant pressure according to the chemical equation shown below, 1062 kJ of heat are released. Calculate the value of ΔH for this reaction, as written. 2CH4(g)+ 3Cl2(g)→ 2CHCl3(l)+ 3H2(g)ΔrH° = ?

Determine the specific heat capacity of an alloy that requires 59.3 kJ to raise the temperature of 150.0 g alloy from 298 K to 398 K.

Calculate the amount of heat (in kJ)necessary to raise the temperature of 47.8 g benzene by 57.0 K. The specific heat capacity of benzene is 1.05 J g-1 °C-1.

Calculate the initial temperature of 448 g of grapes (specific heat capacity = 1.76 J g-1 °C-1)that absorb 17472 J of heat while warming up to room temperature, 23.1 °C.

An unknown metal alloy, mass = 36.1 g, has a temperature change of 31.6 to 24.8 °C after a heat transfer of -103.0 J. Calculate the specific heat capacity of the alloy.

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

Gases

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry II: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallury

Transition Metals and Coordination Compounds

Filters

How much energy is evolved during the formation of 98.7 g of Fe according to the reaction below? Fe₂O₃(s)+ 2Al(s)→ Al₂O₃(s)+ 2Fe(s)Δ_rH°= -852 kJ

Calculate the heat transfer (J)when 3.15 g of platinum (specific heat capacity = 0.133 J g^-1 °C^-1)at 86.1 °C cools to room temperature, 24.3 °C.

A chemist wishes to calibrate a bomb calorimeter, so he combusts 7.529 g of D-galactose, Δ_combustionU = -15.48 kJ g^-1, which causes a temperature change from 26.38 °C to 34.60 °C. What should the chemist report for the value of C_cal?

A 5.00 g sample of liquid water at 25.0 °C is heated by the addition of 145 J of energy. The final temperature of the water is ________ °C. The specific heat capacity of liquid water is 4.184 J g^-1 K^-1.

How much heat is absorbed when 50.00 g of C(s)reacts in the presence of excess SO₂(g)to produce CS₂(l)and CO(g)according to the following chemical equation? 5C(s)+ 2SO₂(g)→ CS₂(l)+ 4CO(g)Δ_rH° = 239.9 kJ

Use the standard reaction enthalpies given below to determine Δ_rH° for the following reaction: 2NO(g)+ O₂(g)→ 2NO₂(g)Δ_rH°= ? Given: N₂(g)+ O₂(g)→ 2NO(g)Δ_rH°= +183 kJ 1/2 N₂(g)+ O₂(g)→ NO₂(g)Δ_rH°= +33 kJ

When 1.50 mol of CH₄(g)reacts with excess Cl₂(g)at constant pressure according to the chemical equation shown below, 1062 kJ of heat are released. Calculate the value of ΔH for this reaction, as written. 2CH₄(g)+ 3Cl₂(g)→ 2CHCl₃(l)+ 3H₂(g)Δ_rH° = ?

Calculate the amount of heat (in kJ)necessary to raise the temperature of 47.8 g benzene by 57.0 K. The specific heat capacity of benzene is 1.05 J g^-1 °C^-1.

Calculate the initial temperature of 448 g of grapes (specific heat capacity = 1.76 J g^-1 °C^-1)that absorb 17472 J of heat while warming up to room temperature, 23.1 °C.