H2S(g)+ 3/2 O2(g)→ H2O (l)+ SO2(g)ΔrH° = -562.3 kJ/mol 1/8 S8(s)+ O2(g)→ SO2(g)ΔrH° = -297.0 kJ/mol H2(g)+ 1/2O2 → H2O (l)ΔrH° = -266.9 kJ/mol Compute ΔrH° for H2(g)+ 1/8 S8 (s)→ H2S(g)in kJ/mol.

A) 562.3 kJ/mol B) 276.6 kJ/mol C) 265.3 kJ/mol D) 20.5 kJ/mol E) -1.6 kJ/mol A) 562.3 kJ/mol B) 276.6 kJ/mol C) 265.3 kJ/mol D) 20.5 kJ/mol E) -1.6 kJ/mol

What is the enthalpy of reaction for the neutralization reaction occurring between dilute Ba(OH)2(aq)and dilute HNO3(aq)? Values of ΔfH° from data tables are given below. Hint: Balance the equation so the coefficients are the lowest possible set of whole numbers.

A) +426.0 kJ/mol B) -111.6 kJ/mol C) -426.0 kJ/mol D) -571.6 kJ/mol E) -460.0 kJ/mol A) +426.0 kJ/mol B) -111.6 kJ/mol C) -426.0 kJ/mol D) -571.6 kJ/mol E) -460.0 kJ/mol

The heat of combustion,ΔrHcomb,of 1-butene(l),C4H8(l),is -2696.9 kJ/mol.From the following values of ΔfH° CO2(g)= -393.5 kJ/mol and ΔfH° H2O(l)= -285.8 kJ/mol,calculate the standard enthalpy of formation of butene(l).

A) +2017 kJ/mol B) -2017 kJ/mol C) -3376 kJ/mol D) -107.7 kJ/mol E) -20.30 kJ/mol A) +2017 kJ/mol B) -2017 kJ/mol C) -3376 kJ/mol D) -107.7 kJ/mol E) -20.30 kJ/mol

The standard enthalpy of formation for CuSO4 ∙ 5 H2O(s)is -2278.0 kJ/mol at 25 °C.The chemical equation to which this value applies is:

A) Cu(s)+ S(s)+ 5 H2O(g)+ 2 O2(g)→ CuSO4 ∙ 5 H2O(s) B) Cu(s)+ S(s)+ 9/2 O2(g)+ 5 H2(g)→ CuSO4 ∙ 5 H2O(s) C) Cu(s)+ SO4(g)+ 5 H2O(g)→ CuSO4 ∙ 5 H2O(s) D) Cu(s)+ S(s)+ 5/9 O2(g)+ 5 H2(g)→ CuSO4 ∙ 5 H2O(s) E) 2 Cu(s)+ 2 SO2(g)+ 5 H2O(g)→ 2 CuSO4 ∙ 5 H2O(s) A) Cu(s)+ S(s)+ 5 H2O(g)+ 2 O2(g)→ CuSO4 ∙ 5 H2O(s) B) Cu(s)+ S(s)+ 9/2 O2(g)+ 5 H2(g)→ CuSO4 ∙ 5 H2O(s) C) Cu(s)+ SO4(g)+ 5 H2O(g)→ CuSO4 ∙ 5 H2O(s) D) Cu(s)+ S(s)+ 5/9 O2(g)+ 5 H2(g)→ CuSO4 ∙ 5 H2O(s) E) 2 Cu(s)+ 2 SO2(g)+ 5 H2O(g)→ 2 CuSO4 ∙ 5 H2O(s)

Exam 7: Thermochemistry

Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: (l)→ O(l)+ (g) H = -196 kJ Calculate the value of q (kJ)in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pressure?

(Multiple Choice)

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Question 81

The enthalpy of a system is the internal energy minus the pressure-volume product.

(True/False)

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Question 82

H₂S(g)+ 3/2 O₂(g)→ H₂O (l)+ SO₂(g)Δ_rH° = -562.3 kJ/mol 1/8 S₈(s)+ O₂(g)→ SO₂(g)Δ_rH° = -297.0 kJ/mol H₂(g)+ 1/2O₂ → H₂O (l)Δ_rH° = -266.9 kJ/mol Compute Δ_rH° for H₂(g)+ 1/8 S₈ (s)→ H₂S(g)in kJ/mol.

(Multiple Choice)

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Question 83

The heat of combustion of several fuels are listed in the table below.On a per gram basis,which fuel releases the most energy?

(Multiple Choice)

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Question 84

What is the enthalpy of reaction for the neutralization reaction occurring between dilute Ba(OH)₂(aq)and dilute HNO₃(aq)? Values of Δ_fH° from data tables are given below. Hint: Balance the equation so the coefficients are the lowest possible set of whole numbers.

(Multiple Choice)

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Question 85

Enthalpy is an extensive property.

(True/False)

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Question 86

The heat of combustion,Δ_rH_comb,of 1-butene(l),C₄H₈(l),is -2696.9 kJ/mol.From the following values of Δ_fH° CO₂(g)= -393.5 kJ/mol and Δ_fH° H₂O(l)= -285.8 kJ/mol,calculate the standard enthalpy of formation of butene(l).

(Multiple Choice)

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Question 87

14.0 g of metal at 24.0 °C has 250 joules of heat added to it.The metal's specific heat is 0.105 J/g °C.What is its final temperature?

(Multiple Choice)

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Question 88

Calculate the kinetic energy of a 150 g baseball moving at a speed of 39.m (87 mph).

(Multiple Choice)

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Question 89

A sample gives off 2505 cal when burned in a bomb calorimeter.The temperature of the calorimeter assembly increases by 2.24 °C.What is the heat capacity of the calorimeter?

(Multiple Choice)

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Question 90

When 50.0 mL of 0.400 mol L^-1 Ca(NO₃)₂ is added to 50.0 mL of 0.800 mol L^-1 NaF,CaF₂ precipitates,as shown in the net ionic equation below.The initial temperature of both solutions is 23.0 °C.Assuming that the reaction goes to completion,and that the resulting solution has a mass of 100.00 g and a specific heat of 4.18 J g^-1°C^-1 ,calculate the final temperature of the solution. Ca²⁺(aq)+ 2 F^-(aq)→ CaF₂(s) H = -11.5 kJ

(Multiple Choice)

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Question 91

How much heat is required to raise the temperature of 175 g of aluminum from 21.0 °C to 145 °C? The specific heat of aluminum is 0.903 J g^-1 °C^-1.

(Multiple Choice)

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Question 92

Calculate the work needed to make room for products in the combustion of sulfur,S₈(s),to SO₂(g)at STP.

(Multiple Choice)

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Question 93

The specific heat of copper is 0.385 J g^-1k^-1.If 34.2 g of copper,initially at 21.0 °C,absorbs 4.689 kJ,what will be the final temperature of the copper?

(Multiple Choice)

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Question 94

Choose the INCORRECT statement.

(Multiple Choice)

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Question 95

The standard enthalpy of formation for CuSO₄∙ 5 H₂O(s)is -2278.0 kJ/mol at 25 °C.The chemical equation to which this value applies is:

(Multiple Choice)

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Question 96

A mixture of 125 g of iron and 250 g of water is heated from 25.0 °C to 70.0 °C.How much heat is absorbed by the mixture? (Specific heat of water = 4.18 J/g °C;iron = 0.473 J/g °C)

(Multiple Choice)

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Question 97

Using the heat of combustion of methanol as -726.6 kJ/mol and the following data: Determine Δ_rH° for the following reaction: CO(g)+ 2 H₂(g)→ CH₃OH(l)

(Multiple Choice)

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Question 98

250.0 g of hot coffee at 95.0 °C are placed in a 0.2000 kg mug at 20.0 °C.The specific heat of the coffee is 4.00 J/g °C,while that of the mug is 0.80 J/g °C.Assuming no heat is lost to the surroundings,what is the final temperature of the system: mug + coffee?

(Multiple Choice)

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Question 99

Consider the reaction: Compute Δ_rH° for this reaction.

(Multiple Choice)

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Question 100

Showing 81 - 100 of 125

Exam 7: Thermochemistry

Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: (l)→ O(l)+ (g) H = -196 kJ Calculate the value of q (kJ)in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pressure?

The enthalpy of a system is the internal energy minus the pressure-volume product.

H2S(g)+ 3/2 O2(g)→ H2O (l)+ SO2(g)ΔrH° = -562.3 kJ/mol 1/8 S8(s)+ O2(g)→ SO2(g)ΔrH° = -297.0 kJ/mol H2(g)+ 1/2O2 → H2O (l)ΔrH° = -266.9 kJ/mol Compute ΔrH° for H2(g)+ 1/8 S8 (s)→ H2S(g)in kJ/mol.

The heat of combustion of several fuels are listed in the table below.On a per gram basis,which fuel releases the most energy?

What is the enthalpy of reaction for the neutralization reaction occurring between dilute Ba(OH)2(aq)and dilute HNO3(aq)? Values of ΔfH° from data tables are given below. Hint: Balance the equation so the coefficients are the lowest possible set of whole numbers.

Enthalpy is an extensive property.

The heat of combustion,ΔrHcomb,of 1-butene(l),C4H8(l),is -2696.9 kJ/mol.From the following values of ΔfH° CO2(g)= -393.5 kJ/mol and ΔfH° H2O(l)= -285.8 kJ/mol,calculate the standard enthalpy of formation of butene(l).

14.0 g of metal at 24.0 °C has 250 joules of heat added to it.The metal's specific heat is 0.105 J/g °C.What is its final temperature?

Calculate the kinetic energy of a 150 g baseball moving at a speed of 39.m (87 mph).

A sample gives off 2505 cal when burned in a bomb calorimeter.The temperature of the calorimeter assembly increases by 2.24 °C.What is the heat capacity of the calorimeter?

How much heat is required to raise the temperature of 175 g of aluminum from 21.0 °C to 145 °C? The specific heat of aluminum is 0.903 J g-1 °C-1.

Calculate the work needed to make room for products in the combustion of sulfur,S8(s),to SO2(g)at STP.

The specific heat of copper is 0.385 J g-1k-1.If 34.2 g of copper,initially at 21.0 °C,absorbs 4.689 kJ,what will be the final temperature of the copper?

Choose the INCORRECT statement.

The standard enthalpy of formation for CuSO4 ∙ 5 H2O(s)is -2278.0 kJ/mol at 25 °C.The chemical equation to which this value applies is:

A mixture of 125 g of iron and 250 g of water is heated from 25.0 °C to 70.0 °C.How much heat is absorbed by the mixture? (Specific heat of water = 4.18 J/g °C;iron = 0.473 J/g °C)

Using the heat of combustion of methanol as -726.6 kJ/mol and the following data: Determine ΔrH° for the following reaction: CO(g)+ 2 H2(g)→ CH3OH(l)

250.0 g of hot coffee at 95.0 °C are placed in a 0.2000 kg mug at 20.0 °C.The specific heat of the coffee is 4.00 J/g °C,while that of the mug is 0.80 J/g °C.Assuming no heat is lost to the surroundings,what is the final temperature of the system: mug + coffee?

Consider the reaction: Compute ΔrH° for this reaction.

Matter: Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Valence Bond and Molecular Orbital Theories

Intermolecular Forces: Liquids and Solids

Spontaneous Change: Entropy and Gibbs Energy

Solutions and Their Physical Properties

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acidbase Equilibria

Solubility and Complex-Ion Equilibria

Electrochemistry

Chemical Kinetics

Chemistry of the Main-Group Elements I: Groups 1,2,13,and 14

Chemistry of the Main-Group Elements Ii: Groups 18,17,16,15,and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

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H₂S(g)+ 3/2 O₂(g)→ H₂O (l)+ SO₂(g)Δ_rH° = -562.3 kJ/mol 1/8 S₈(s)+ O₂(g)→ SO₂(g)Δ_rH° = -297.0 kJ/mol H₂(g)+ 1/2O₂ → H₂O (l)Δ_rH° = -266.9 kJ/mol Compute Δ_rH° for H₂(g)+ 1/8 S₈ (s)→ H₂S(g)in kJ/mol.

What is the enthalpy of reaction for the neutralization reaction occurring between dilute Ba(OH)₂(aq)and dilute HNO₃(aq)? Values of Δ_fH° from data tables are given below. Hint: Balance the equation so the coefficients are the lowest possible set of whole numbers.

The heat of combustion,Δ_rH_comb,of 1-butene(l),C₄H₈(l),is -2696.9 kJ/mol.From the following values of Δ_fH° CO₂(g)= -393.5 kJ/mol and Δ_fH° H₂O(l)= -285.8 kJ/mol,calculate the standard enthalpy of formation of butene(l).

How much heat is required to raise the temperature of 175 g of aluminum from 21.0 °C to 145 °C? The specific heat of aluminum is 0.903 J g^-1 °C^-1.

Calculate the work needed to make room for products in the combustion of sulfur,S₈(s),to SO₂(g)at STP.

The specific heat of copper is 0.385 J g^-1k^-1.If 34.2 g of copper,initially at 21.0 °C,absorbs 4.689 kJ,what will be the final temperature of the copper?

The standard enthalpy of formation for CuSO₄∙ 5 H₂O(s)is -2278.0 kJ/mol at 25 °C.The chemical equation to which this value applies is:

Using the heat of combustion of methanol as -726.6 kJ/mol and the following data: Determine Δ_rH° for the following reaction: CO(g)+ 2 H₂(g)→ CH₃OH(l)

Consider the reaction: Compute Δ_rH° for this reaction.