You are given pure samples of pentane, CH3CH2CH2CH2CH3(l), and 1,3-pentadiene, CH2=CHCH=CHCH3(l). What prediction would you make concerning their standard molar entropies at 298 K?

A) S°pentane > S°1, 3-pentadiene B) S°pentane 1, 3-pentadiene C) S°pentane F1F1F1S1F1F1F10 S°1, 3-pentadiene D) S°pentane = S°1, 3-pentadiene + 2 E) More information is needed to make reasonable predictions. A) S°pentane > S°1, 3-pentadiene B) S°pentane 1, 3-pentadiene C) S°pentane F1F1F1S1F1F1F10 S°1, 3-pentadiene D) S°pentane = S°1, 3-pentadiene + 2 E) More information is needed to make reasonable predictions.

Calculate F1F1F1S1F1F1F10G° for the reaction

A) 566.60 kJ B) 50.38 kJ C) 25.19 kJ D) -25.19 kJ E) -566.60 kJ A) 566.60 kJ B) 50.38 kJ C) 25.19 kJ D) -25.19 kJ E) -566.60 kJ

Which relationship or statement best describes F1F1F1S1F1F1F10S° for the following reaction? HgS(s) + O2(g) F1F1F1S1F1F1F10 Hg(l) + SO2(g)

A) .F1F1F1S1F1F1F10S° F1F1F1S1F1F1F10 0 B) .F1F1F1S1F1F1F10S° 0 D) .F1F1F1S1F1F1F10S° = F1F1F1S1F1F1F10H°/T E) More information is needed to make a reasonable prediction. A) .F1F1F1S1F1F1F10S° F1F1F1S1F1F1F10 0 B) .F1F1F1S1F1F1F10S° 0 D) .F1F1F1S1F1F1F10S° = F1F1F1S1F1F1F10H°/T E) More information is needed to make a reasonable prediction.

Which relationship or statement best describes F1F1F1S1F1F1F10S° for the following reaction? C2H5OH(l) + 3O2(g) F1F1F1S1F1F1F10 2CO2(g) + 3H2O(l)

A) .F1F1F1S1F1F1F10S° F1F1F1S1F1F1F10 0 B) .F1F1F1S1F1F1F10S° 0 D) .F1F1F1S1F1F1F10S° = F1F1F1S1F1F1F10H°/T E) More information is needed to make a reasonable prediction. A) .F1F1F1S1F1F1F10S° F1F1F1S1F1F1F10 0 B) .F1F1F1S1F1F1F10S° 0 D) .F1F1F1S1F1F1F10S° = F1F1F1S1F1F1F10H°/T E) More information is needed to make a reasonable prediction.

Calculate F1F1F1S1F1F1F10S° for the reaction

A) -548.1 J/K B) -147.7 J/K C) 147.7 J/K D) 310.1 J/K E ) 548.1 J/K A) -548.1 J/K B) -147.7 J/K C) 147.7 J/K D) 310.1 J/K E ) 548.1 J/K

A chemical reaction has F1F1F1S1F1F1F10G° = 10.0 kJ and F1F1F1S1F1F1F10S° = 50.0 J/K a. Calculate F1F1F1S1F1F1F10H° for this reaction at 25°C. b. Could this reaction ever be spontaneous? Explain your answer.

a. F1F1F1S1F1F1F10H° = 24.9 kJ b. Yes.

Which relationship or statement best describes F1F1F1S1F1F1F10S° for the following reaction? CaO(s) + CO2(g) F1F1F1S1F1F1F10 CaCO3(s)

A) .F1F1F1S1F1F1F10S° F1F1F1S1F1F1F10 0 B) .F1F1F1S1F1F1F10S° 0 D) .F1F1F1S1F1F1F10S° = F1F1F1S1F1F1F10H°/T E) More information is needed to make a reasonable prediction. A) .F1F1F1S1F1F1F10S° F1F1F1S1F1F1F10 0 B) .F1F1F1S1F1F1F10S° 0 D) .F1F1F1S1F1F1F10S° = F1F1F1S1F1F1F10H°/T E) More information is needed to make a reasonable prediction.

A reaction has F1F1F1S1F1F1F10G = 10.0 kJ and F1F1F1S1F1F1F10G° = 15.0 kJ at a temperature of 50 °C. Calculate the value of the reaction quotient Q under these conditions.

A) 0.16 B) 9.1 × 10-5 C) 1.1 × 104 D) 6.4 E) 6.0 × 10-6 A) 0.16 B) 9.1 × 10-5 C) 1.1 × 104 D) 6.4 E) 6.0 × 10-6

What is the free energy change, F1F1F1S1F1F1F10G°, for the equilibrium between hydrogen iodide, hydrogen, and iodine at 453°C?

A) 6.4 kJ B) 8.8 kJ C) 15 kJ D) 19 kJ E) 24 kJ A) 6.4 kJ B) 8.8 kJ C) 15 kJ D) 19 kJ E) 24 kJ

Which relationship or statement best describes F1F1F1S1F1F1F10S° for the following reaction? Pb(s) + Cl2(g) F1F1F1S1F1F1F10 PbCl2(s)

A) .F1F1F1S1F1F1F10S° F1F1F1S1F1F1F10 0 B) .F1F1F1S1F1F1F10S° 0 D) .F1F1F1S1F1F1F10S° = F1F1F1S1F1F1F10H°/T E) More information is needed to make a reasonable prediction. A) .F1F1F1S1F1F1F10S° F1F1F1S1F1F1F10 0 B) .F1F1F1S1F1F1F10S° 0 D) .F1F1F1S1F1F1F10S° = F1F1F1S1F1F1F10H°/T E) More information is needed to make a reasonable prediction.

Calculate F1F1F1S1F1F1F10G° for the combustion of propane.

A) -2073.1 kJ B) -1387.3 kJ C) -598.5 kJ D) 598.5 kJ E) 2073.1 kJ A) -2073.1 kJ B) -1387.3 kJ C) -598.5 kJ D) 598.5 kJ E) 2073.1 kJ

Hydrogen sulfide decomposes according to the following reaction 2H2S(g) F1F1F1S1F1F1F10 2H2(g) + S2(g) For this reaction at 298K F1F1F1S1F1F1F10S° = 78.1 J/K, F1F1F1S1F1F1F10H° = 169.4 kJ, and F1F1F1S1F1F1F10G° = 146.1 kJ. What is the value of F1F1F1S1F1F1F10G° at 900 K?

A) -69881 kJ B) 48.4 kJ C) 99.1 kJ D) 240 kJ E) 441 kJ A) -69881 kJ B) 48.4 kJ C) 99.1 kJ D) 240 kJ E) 441 kJ

Exam 20: Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

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You are given pure samples of pentane, CH₃CH₂CH₂CH₂CH₃(l), and 1,3-pentadiene, CH₂=CHCH=CHCH₃(l). What prediction would you make concerning their standard molar entropies at 298 K?

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Question 21

Under a given set of conditions, all microstates of a system are equally probable.

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Question 22

The temperature at which the following process reaches equilibrium at 1.0 atm is the normal boiling point of hydrogen peroxide. Use the following thermodynamic information at 298 K to determine this temperature.

(Multiple Choice)

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Question 23

The temperature at which the following process reaches equilibrium at 1.0 atm is the normal melting point for phosphoric acid. Use the following thermodynamic data at 298 K to determine this temperature.

(Multiple Choice)

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Question 24

Which of the following conditions will ensure that a chemical reaction will definitely proceed in the forward direction, toward products?

(Multiple Choice)

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Question 25

Calculate G°for the reaction

(Multiple Choice)

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Question 26

Which relationship or statement best describes S° for the following reaction? HgS(s) + O₂(g)  Hg(l) + SO₂(g)

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Question 27

Which relationship or statement best describes S° for the following reaction? C₂H₅OH(l) + 3O₂(g)  2CO₂(g) + 3H₂O(l)

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Question 28

A sample of water is heated at a constant pressure of one atmosphere. Initially, the sample is ice at 260 K, and at the end the sample consists of steam at 400 K. In which of the following 5K temperature intervals would there be the greatest increase in the entropy of the sample?

(Multiple Choice)

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Question 29

Calculate S° for the reaction

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Question 30

A chemical reaction has G° = 10.0 kJ and S° = 50.0 J/K a. Calculate H°for this reaction at 25°C. b. Could this reaction ever be spontaneous? Explain your answer.

(Essay)

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Question 31

Which relationship or statement best describes S° for the following reaction? CaO(s) + CO₂(g)  CaCO₃(s)

(Multiple Choice)

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Question 32

A reaction has G = 10.0 kJ and G° = 15.0 kJ at a temperature of 50 °C. Calculate the value of the reaction quotient Q under these conditions.

(Multiple Choice)

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Question 33

What is the free energy change, G°, for the equilibrium between hydrogen iodide, hydrogen, and iodine at 453°C?

(Multiple Choice)

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Question 34

The second law of thermodynamics tells us that

(Multiple Choice)

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Question 35

Which relationship or statement best describes S° for the following reaction? Pb(s) + Cl₂(g)  PbCl₂(s)

(Multiple Choice)

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Question 36

In tables of thermodynamic data provided in chemistry books, one finds H°_f, G°_f, and S° listed. Briefly, explain why the entropy data are supplied as S°, while the enthalpy and free energy data are in the form of H°_f and G°_f, respectively.

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Question 37

Calculate G°for the combustion of propane.

(Multiple Choice)

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Question 38

For a chemical reaction to be non-spontaneous at any temperature, which of the following conditions must be met?

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Question 39

Hydrogen sulfide decomposes according to the following reaction 2H₂S(g)  2H₂(g) + S₂(g) For this reaction at 298K S°= 78.1 J/K, H°= 169.4 kJ, and G° = 146.1 kJ. What is the value of G° at 900 K?

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Question 40

Showing 21 - 40 of 94

Exam 20: Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

You are given pure samples of pentane, CH3CH2CH2CH2CH3(l), and 1,3-pentadiene, CH2=CHCH=CHCH3(l). What prediction would you make concerning their standard molar entropies at 298 K?

Under a given set of conditions, all microstates of a system are equally probable.

The temperature at which the following process reaches equilibrium at 1.0 atm is the normal boiling point of hydrogen peroxide. Use the following thermodynamic information at 298 K to determine this temperature.

The temperature at which the following process reaches equilibrium at 1.0 atm is the normal melting point for phosphoric acid. Use the following thermodynamic data at 298 K to determine this temperature.

Which of the following conditions will ensure that a chemical reaction will definitely proceed in the forward direction, toward products?

Calculate G° for the reaction

Which relationship or statement best describes S° for the following reaction? HgS(s) + O2(g)  Hg(l) + SO2(g)

Which relationship or statement best describes S° for the following reaction? C2H5OH(l) + 3O2(g)  2CO2(g) + 3H2O(l)

A sample of water is heated at a constant pressure of one atmosphere. Initially, the sample is ice at 260 K, and at the end the sample consists of steam at 400 K. In which of the following 5K temperature intervals would there be the greatest increase in the entropy of the sample?

Calculate S° for the reaction

A chemical reaction has G° = 10.0 kJ and S° = 50.0 J/K a. Calculate H° for this reaction at 25°C. b. Could this reaction ever be spontaneous? Explain your answer.

Which relationship or statement best describes S° for the following reaction? CaO(s) + CO2(g)  CaCO3(s)

A reaction has G = 10.0 kJ and G° = 15.0 kJ at a temperature of 50 °C. Calculate the value of the reaction quotient Q under these conditions.

What is the free energy change, G°, for the equilibrium between hydrogen iodide, hydrogen, and iodine at 453°C?

The second law of thermodynamics tells us that

Which relationship or statement best describes S° for the following reaction? Pb(s) + Cl2(g)  PbCl2(s)

In tables of thermodynamic data provided in chemistry books, one finds H°f, G°f, and S° listed. Briefly, explain why the entropy data are supplied as S°, while the enthalpy and free energy data are in the form of H°f and G°f, respectively.

Calculate G° for the combustion of propane.

For a chemical reaction to be non-spontaneous at any temperature, which of the following conditions must be met?

Hydrogen sulfide decomposes according to the following reaction 2H2S(g)  2H2(g) + S2(g) For this reaction at 298K S° = 78.1 J/K, H° = 169.4 kJ, and G° = 146.1 kJ. What is the value of G° at 900 K?

Keys to the Study of Chemistry

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Stoichiometry of Formulas and Equations

The Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

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Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main Group Elements: Bonding, Structure, and Reactivity

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

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Ionic Equilibria in Aqueous Systems

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The Elements in Nature and Industry

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You are given pure samples of pentane, CH₃CH₂CH₂CH₂CH₃(l), and 1,3-pentadiene, CH₂=CHCH=CHCH₃(l). What prediction would you make concerning their standard molar entropies at 298 K?

Calculate G°for the reaction

Which relationship or statement best describes S° for the following reaction? HgS(s) + O₂(g)  Hg(l) + SO₂(g)

Which relationship or statement best describes S° for the following reaction? C₂H₅OH(l) + 3O₂(g)  2CO₂(g) + 3H₂O(l)

A chemical reaction has G° = 10.0 kJ and S° = 50.0 J/K a. Calculate H°for this reaction at 25°C. b. Could this reaction ever be spontaneous? Explain your answer.

Which relationship or statement best describes S° for the following reaction? CaO(s) + CO₂(g)  CaCO₃(s)

Which relationship or statement best describes S° for the following reaction? Pb(s) + Cl₂(g)  PbCl₂(s)

In tables of thermodynamic data provided in chemistry books, one finds H°_f, G°_f, and S° listed. Briefly, explain why the entropy data are supplied as S°, while the enthalpy and free energy data are in the form of H°_f and G°_f, respectively.

Calculate G°for the combustion of propane.

Hydrogen sulfide decomposes according to the following reaction 2H₂S(g)  2H₂(g) + S₂(g) For this reaction at 298K S°= 78.1 J/K, H°= 169.4 kJ, and G° = 146.1 kJ. What is the value of G° at 900 K?