Question 1

Rubidium has a heat of vaporization of 69.0 kJ/mol at its boiling point (686°C). Calculate $\Delta$S for this process, Rb(l) $\rarr$ Rb(g), at 1 atm and 686°C.

Accepted Answer

The answer of Rubidium has a heat of vaporization of...

Question 2

HI has a normal boiling point of -35.4°C, and its $\Delta$Hvap is 21.16 kJ/mol. Calculate the molar entropy of vaporization ($\Delta$Svap).

Accepted Answer

A) 598 J/K·mol 
B) 68.6 J/K·mol 
C) 75.2 J/K·mol 
D) 0.068 J/K·mol 
E) 89.0 J/K·mol 
A) 598 J/K·mol 
B) 68.6 J/K·mol 
C) 75.2 J/K·mol 
D) 0.068 J/K·mol 
E) 89.0 J/K·mol

Question 3

Arrange these compounds in order of increasing standard molar entropy at 25°C: C3H8(g), C2H4(g), ZnS(s), and H2O(l).

Accepted Answer

A) ZnS(s)2O(l)3H8(g)2H4(g) 
B) C2H4(g)2O(l)3H8(g)3H8(g)2H4(g)2O(l) 
D) C3H8(g)2H4(g)2O(l)2O(l)2H4(g)3H8(g) 
A) ZnS(s)2O(l)3H8(g)2H4(g) 
B) C2H4(g)2O(l)3H8(g)3H8(g)2H4(g)2O(l) 
D) C3H8(g)2H4(g)2O(l)2O(l)2H4(g)3H8(g)

Question 4

The solubility product constant at 25°C for AgI(s)in water has the value 8.3 * 10-17. Calculate $\Delta$Grxn at 25°C for the process AgI(s) $\rarr$ Ag+(aq)+ I- (aq)where [Ag+] = 9.1 * 10-9 and [I-] = 9.1 * 10-9.

Accepted Answer

A) +4.4 kJ/mol 
B) +91.7 kJ/mol 
C) 0.0 kJ/mol 
D) -91.7 kJ/mol 
E) -4.4 kJ/mol 
A) +4.4 kJ/mol 
B) +91.7 kJ/mol 
C) 0.0 kJ/mol 
D) -91.7 kJ/mol 
E) -4.4 kJ/mol

Question 5

Consider the reaction CO(g)+ 2H2(g) $\rarr$ CH3OH(l)at 25°C.
$\Delta$G°f (CO)= -137.3 kJ/mol
$\Delta$G°f (CH3OH)= -166.3 kJ/mol
$\Delta$H°f (CO)= -110.5 kJ/mol
$\Delta$H°f (CH3OH)= -238.7 kJ/mol
S°(CO)= 197.9 J/K·mol
S°(CH3OH)= 126.8 J/K·mol
Calculate value of the equilibrium constant (Kp)for this reaction at 25°C.

Accepted Answer

1.21 * 10<

Question 6

How does the entropy change when a gas is converted to a liquid?

Accepted Answer

The answer of How does the entropy change when a...

Question 7

The equilibrium constant for the reaction AgBr(s) $\rarr$ Ag+(aq)+ Br- (aq)is the solubility product constant, Ksp = 7.7* 10-13 at 25°C. Calculate $\Delta$G for the reaction when [Ag+] = 1.0 * 10-2 M and [Br-] = 1.0 * 10-3 M. Is the reaction spontaneous or nonspontaneous at these concentrations?

Accepted Answer

A) ($\Delta$G) = 69.1 kJ/mol, nonspontaneous 
B) ($\Delta$G) = -69.1 kJ/mol, spontaneous 
C) ($\Delta$G) = 97.5 kJ/mol, spontaneous 
D) ($\Delta$G) = 40.6 kJ/mol, nonspontaneous 
E) ($\Delta$G) = -97.5 kJ/mol, nonspontaneous 
A) ($\Delta$G) = 69.1 kJ/mol, nonspontaneous 
B) ($\Delta$G) = -69.1 kJ/mol, spontaneous 
C) ($\Delta$G) = 97.5 kJ/mol, spontaneous 
D) ($\Delta$G) = 40.6 kJ/mol, nonspontaneous 
E) ($\Delta$G) = -97.5 kJ/mol, nonspontaneous

Question 8

Which of these species would you expect to have the lowest standard entropy (S°)?

Accepted Answer

A) CH4(g) 
B) HF(g) 
C) NH3(g) 
D) H2O(g) 
A) CH4(g) 
B) HF(g) 
C) NH3(g) 
D) H2O(g)

Question 9

Arrange the following substances in the order of increasing entropy at 25°C. HF(g), NaF(s), SiF4(g), SiH4(g), Al(s)
Lowest $\rarr$ highest

Accepted Answer

A) SiF4(g)4(g)4(g)4(g) 
C) Al(s)4(g)4(g) 
D) Al(s)4(g)4(g) 
E) NaF(s)4(g)4(g) 
A) SiF4(g)4(g)4(g)4(g) 
C) Al(s)4(g)4(g) 
D) Al(s)4(g)4(g) 
E) NaF(s)4(g)4(g)

Question 10

Calculate the equilibrium constant for the decomposition of water 2H2O(l) $\rarr$ 2H2(g)+ O2(g)
At 25°C, given that $\Delta$G°f (H2O(l))= -237.2 kJ/mol.

Accepted Answer

A) 0.83 
B) 6.3 * 10-84 
C) 2.5 * 10-42 
D) 1.6 * 1083 
E) 4.7 * 105 
A) 0.83 
B) 6.3 * 10-84 
C) 2.5 * 10-42 
D) 1.6 * 1083 
E) 4.7 * 105

Question 11

For the reaction HCONH2(g) $\rarr$ NH3(g)+ CO(g), Kc = 4.84 at 400 K. If $\Delta$H° for this reaction is 29 kJ/mol, find Kc at 500 K.

Accepted Answer

A) 5.8 
B) 0.17 
C) 27 
D) 0.88 
E) 10.3 
A) 5.8 
B) 0.17 
C) 27 
D) 0.88 
E) 10.3

Question 12

Predict the sign of $\Delta$S for the reaction 6CO2(g)+ 6H2O(g) $\rarr$ C6H12O6(g)+ 6O2(g).

Accepted Answer

The answer of Predict the sign of $\Delta$S for the...

Question 13

Assuming $\Delta$S° and $\Delta$H° do not vary with temperature, at what temperature will the reaction shown below become spontaneous?
C(s)+ H2O(g) $\rarr$H2(g)+ CO(s)($\Delta$S° = 133.6 J/K·mol; $\Delta$H° = 131.3 kJ/mol)

Accepted Answer

The answer of Assuming $\Delta$S° and $\Delta$H° do not vary...

Question 14

For the reaction SbCl5(g) $\rarr$ SbCl3(g)+ Cl2(g),
$\Delta$G°f (SbCl5)= -334.34 kJ/mol
$\Delta$G°f (SbCl3)= -301.25 kJ/mol
$\Delta$H°f (SbCl5)= -394.34 kJ/mol
$\Delta$H°f (SbCl3)= -313.80 kJ/mol
Will this reaction proceed spontaneously at 298 K and 1 atm pressure?

Accepted Answer

The answer of For the reaction SbCl5(g) $\rarr$ SbCl3(g)+ Cl2(g),
$\Delta$G°f...

Question 15

Using the thermodynamic data provided below, calculate Ksp for Mg(OH)2(s)at 25°.

Accepted Answer

8.90 * 10^-12 (agree

Question 16

What is the free energy change for the reaction SiO2(s)+ Pb(s) $\rarr$PbO2(s)+ Si(s)?
$\Delta$G°f (PbO2)= -217 kJ/mol
$\Delta$G°f (SiO2)= -856 kJ/mol

Accepted Answer

The answer of What is the free energy change for...

Question 17

Choose the substance with the higher entropy per mole at a given temperature: Br2(l)or Br2(g).

Accepted Answer

Question 18

For the reaction CuS(s)+ H2(g) $\rarr$ H2S(g)+ Cu(s),
$\Delta$G°f (CuS)= -53.6 kJ/mol
$\Delta$G°f (H2S)= -33.6 kJ/mol
$\Delta$H°f (CuS)= -53.1 kJ/mol
$\Delta$H°f (H2S)= -20.6 kJ/mol
Calculate the value of the equilibrium constant (Kp)at 798 K and 1 atm pressure.

Accepted Answer

The answer of For the reaction CuS(s)+ H2(g) $\rarr$ H2S(g)+...

Question 19

For the reaction CuS(s)+ H2(g) $\rarr$ H2S(g)+ Cu(s),
$\Delta$G°f (CuS)= -53.6 kJ/mol
$\Delta$G°f (H2S)= -33.6 kJ/mol
$\Delta$H°f (CuS)= -53.1 kJ/mol
$\Delta$H°f (H2S)= -20.6 kJ/mol
Will this reaction proceed spontaneously at 298 K and 1 atm pressure?

Accepted Answer

The answer of For the reaction CuS(s)+ H2(g) $\rarr$ H2S(g)+...

Question 20

For the reaction 3H2(g)+ N2(g) $\rarr$ 2NH3(g), Kc = 9.0 at 350°C. What is the value of $\Delta$G at this temperature when 1.0 mol NH3, 5.0 mol N2, and 5.0 mol H2 are mixed in a 2.5 L reactor?

Accepted Answer

The answer of For the reaction 3H2(g)+ N2(g) $\rarr$ 2NH3(g),...

Rubidium has a heat of vaporization of 69.0 kJ/mol at its boiling point (686°C). Calculate $\Delta$ S for this process, Rb(l) $\rarr$ Rb(g), at 1 atm and 686°C.

HI has a normal boiling point of -35.4°C, and its $\Delta$ H_vap is 21.16 kJ/mol. Calculate the molar entropy of vaporization ( $\Delta$ S_vap).

Arrange these compounds in order of increasing standard molar entropy at 25°C: C₃H₈(g), C₂H₄(g), ZnS(s), and H₂O(l).

The solubility product constant at 25°C for AgI(s)in water has the value 8.3 * 10^-17. Calculate $\Delta$ G_rxn at 25°C for the process AgI(s) $\rarr$ Ag⁺(aq)+ I^-(aq)where [Ag⁺] = 9.1 * 10^-9 and [I^-] = 9.1 * 10^-9.

How does the entropy change when a gas is converted to a liquid?

Which of these species would you expect to have the lowest standard entropy (S°)?

Arrange the following substances in the order of increasing entropy at 25°C. HF(g), NaF(s), SiF₄(g), SiH₄(g), Al(s) Lowest $\rarr$ highest

Calculate the equilibrium constant for the decomposition of water 2H₂O(l) $\rarr$ 2H₂(g)+ O₂(g) At 25°C, given that $\Delta$ G°_f(H₂O(l))= -237.2 kJ/mol.

For the reaction HCONH₂(g) $\rarr$ NH₃(g)+ CO(g), K_c = 4.84 at 400 K. If $\Delta$ H° for this reaction is 29 kJ/mol, find K_c at 500 K.

Predict the sign of $\Delta$ S for the reaction 6CO₂(g)+ 6H₂O(g) $\rarr$ C₆H₁₂O₆(g)+ 6O₂(g).

Assuming $\Delta$ S° and $\Delta$ H° do not vary with temperature, at what temperature will the reaction shown below become spontaneous? C(s)+ H₂O(g) $\rarr$ H₂(g)+ CO(s)( $\Delta$ S° = 133.6 J/K·mol; $\Delta$ H° = 131.3 kJ/mol)

For the reaction SbCl₅(g) $\rarr$ SbCl₃(g)+ Cl₂(g), $\Delta$ G°_f (SbCl₅)= -334.34 kJ/mol $\Delta$ G°_f (SbCl₃)= -301.25 kJ/mol $\Delta$ H°_f (SbCl₅)= -394.34 kJ/mol $\Delta$ H°_f (SbCl₃)= -313.80 kJ/mol Will this reaction proceed spontaneously at 298 K and 1 atm pressure?

Using the thermodynamic data provided below, calculate K_sp for Mg(OH)₂(s)at 25°.

What is the free energy change for the reaction SiO₂(s)+ Pb(s) $\rarr$ PbO₂(s)+ Si(s)? $\Delta$ G°_f (PbO₂)= -217 kJ/mol $\Delta$ G°_f (SiO₂)= -856 kJ/mol

Choose the substance with the higher entropy per mole at a given temperature: Br₂(l)or Br₂(g).

For the reaction CuS(s)+ H₂(g) $\rarr$ H₂S(g)+ Cu(s), $\Delta$ G°_f (CuS)= -53.6 kJ/mol $\Delta$ G°_f (H₂S)= -33.6 kJ/mol $\Delta$ H°_f (CuS)= -53.1 kJ/mol $\Delta$ H°_f (H₂S)= -20.6 kJ/mol Calculate the value of the equilibrium constant (K_p)at 798 K and 1 atm pressure.

For the reaction CuS(s)+ H₂(g) $\rarr$ H₂S(g)+ Cu(s), $\Delta$ G°_f (CuS)= -53.6 kJ/mol $\Delta$ G°_f (H₂S)= -33.6 kJ/mol $\Delta$ H°_f (CuS)= -53.1 kJ/mol $\Delta$ H°_f (H₂S)= -20.6 kJ/mol Will this reaction proceed spontaneously at 298 K and 1 atm pressure?

For the reaction 3H₂(g)+ N₂(g) $\rarr$ 2NH₃(g), K_c = 9.0 at 350°C. What is the value of $\Delta$ G at this temperature when 1.0 mol NH₃, 5.0 mol N₂, and 5.0 mol H₂ are mixed in a 2.5 L reactor?

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

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Exam 18: Thermodynamics

Rubidium has a heat of vaporization of 69.0 kJ/mol at its boiling point (686°C). Calculate Δ\DeltaΔ S for this process, Rb(l) →\rarr→ Rb(g), at 1 atm and 686°C.

HI has a normal boiling point of -35.4°C, and its Δ\DeltaΔ Hvap is 21.16 kJ/mol. Calculate the molar entropy of vaporization ( Δ\DeltaΔ Svap).

Arrange these compounds in order of increasing standard molar entropy at 25°C: C3H8(g), C2H4(g), ZnS(s), and H2O(l).

The solubility product constant at 25°C for AgI(s)in water has the value 8.3 * 10-17. Calculate Δ\DeltaΔ Grxn at 25°C for the process AgI(s) →\rarr→ Ag+(aq)+ I- (aq)where [Ag+] = 9.1 * 10-9 and [I-] = 9.1 * 10-9.

How does the entropy change when a gas is converted to a liquid?

Which of these species would you expect to have the lowest standard entropy (S°)?

Arrange the following substances in the order of increasing entropy at 25°C. HF(g), NaF(s), SiF4(g), SiH4(g), Al(s) Lowest →\rarr→ highest

Calculate the equilibrium constant for the decomposition of water 2H2O(l) →\rarr→ 2H2(g)+ O2(g) At 25°C, given that Δ\DeltaΔ G°f (H2O(l))= -237.2 kJ/mol.

For the reaction HCONH2(g) →\rarr→ NH3(g)+ CO(g), Kc = 4.84 at 400 K. If Δ\DeltaΔ H° for this reaction is 29 kJ/mol, find Kc at 500 K.

Predict the sign of Δ\DeltaΔ S for the reaction 6CO2(g)+ 6H2O(g) →\rarr→ C6H12O6(g)+ 6O2(g).

Assuming Δ\DeltaΔ S° and Δ\DeltaΔ H° do not vary with temperature, at what temperature will the reaction shown below become spontaneous? C(s)+ H2O(g) →\rarr→ H2(g)+ CO(s)( Δ\DeltaΔ S° = 133.6 J/K·mol; Δ\DeltaΔ H° = 131.3 kJ/mol)

For the reaction SbCl5(g) →\rarr→ SbCl3(g)+ Cl2(g), Δ\DeltaΔ G°f (SbCl5)= -334.34 kJ/mol Δ\DeltaΔ G°f (SbCl3)= -301.25 kJ/mol Δ\DeltaΔ H°f (SbCl5)= -394.34 kJ/mol Δ\DeltaΔ H°f (SbCl3)= -313.80 kJ/mol Will this reaction proceed spontaneously at 298 K and 1 atm pressure?

Using the thermodynamic data provided below, calculate Ksp for Mg(OH)2(s)at 25°.

What is the free energy change for the reaction SiO2(s)+ Pb(s) →\rarr→ PbO2(s)+ Si(s)? Δ\DeltaΔ G°f (PbO2)= -217 kJ/mol Δ\DeltaΔ G°f (SiO2)= -856 kJ/mol

Choose the substance with the higher entropy per mole at a given temperature: Br2(l)or Br2(g).

For the reaction CuS(s)+ H2(g) →\rarr→ H2S(g)+ Cu(s), Δ\DeltaΔ G°f (CuS)= -53.6 kJ/mol Δ\DeltaΔ G°f (H2S)= -33.6 kJ/mol Δ\DeltaΔ H°f (CuS)= -53.1 kJ/mol Δ\DeltaΔ H°f (H2S)= -20.6 kJ/mol Calculate the value of the equilibrium constant (Kp)at 798 K and 1 atm pressure.

For the reaction CuS(s)+ H2(g) →\rarr→ H2S(g)+ Cu(s), Δ\DeltaΔ G°f (CuS)= -53.6 kJ/mol Δ\DeltaΔ G°f (H2S)= -33.6 kJ/mol Δ\DeltaΔ H°f (CuS)= -53.1 kJ/mol Δ\DeltaΔ H°f (H2S)= -20.6 kJ/mol Will this reaction proceed spontaneously at 298 K and 1 atm pressure?

For the reaction 3H2(g)+ N2(g) →\rarr→ 2NH3(g), Kc = 9.0 at 350°C. What is the value of Δ\DeltaΔ G at this temperature when 1.0 mol NH3, 5.0 mol N2, and 5.0 mol H2 are mixed in a 2.5 L reactor?

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

Rubidium has a heat of vaporization of 69.0 kJ/mol at its boiling point (686°C). Calculate $\Delta$ S for this process, Rb(l) $\rarr$ Rb(g), at 1 atm and 686°C.

HI has a normal boiling point of -35.4°C, and its $\Delta$ H_vap is 21.16 kJ/mol. Calculate the molar entropy of vaporization ( $\Delta$ S_vap).

Arrange these compounds in order of increasing standard molar entropy at 25°C: C₃H₈(g), C₂H₄(g), ZnS(s), and H₂O(l).

The solubility product constant at 25°C for AgI(s)in water has the value 8.3 * 10^-17. Calculate $\Delta$ G_rxn at 25°C for the process AgI(s) $\rarr$ Ag⁺(aq)+ I^-(aq)where [Ag⁺] = 9.1 * 10^-9 and [I^-] = 9.1 * 10^-9.

Arrange the following substances in the order of increasing entropy at 25°C. HF(g), NaF(s), SiF₄(g), SiH₄(g), Al(s) Lowest $\rarr$ highest

Calculate the equilibrium constant for the decomposition of water 2H₂O(l) $\rarr$ 2H₂(g)+ O₂(g) At 25°C, given that $\Delta$ G°_f(H₂O(l))= -237.2 kJ/mol.

For the reaction HCONH₂(g) $\rarr$ NH₃(g)+ CO(g), K_c = 4.84 at 400 K. If $\Delta$ H° for this reaction is 29 kJ/mol, find K_c at 500 K.

Predict the sign of $\Delta$ S for the reaction 6CO₂(g)+ 6H₂O(g) $\rarr$ C₆H₁₂O₆(g)+ 6O₂(g).

Assuming $\Delta$ S° and $\Delta$ H° do not vary with temperature, at what temperature will the reaction shown below become spontaneous? C(s)+ H₂O(g) $\rarr$ H₂(g)+ CO(s)( $\Delta$ S° = 133.6 J/K·mol; $\Delta$ H° = 131.3 kJ/mol)

For the reaction SbCl₅(g) $\rarr$ SbCl₃(g)+ Cl₂(g), $\Delta$ G°_f (SbCl₅)= -334.34 kJ/mol $\Delta$ G°_f (SbCl₃)= -301.25 kJ/mol $\Delta$ H°_f (SbCl₅)= -394.34 kJ/mol $\Delta$ H°_f (SbCl₃)= -313.80 kJ/mol Will this reaction proceed spontaneously at 298 K and 1 atm pressure?

Using the thermodynamic data provided below, calculate K_sp for Mg(OH)₂(s)at 25°.

What is the free energy change for the reaction SiO₂(s)+ Pb(s) $\rarr$ PbO₂(s)+ Si(s)? $\Delta$ G°_f (PbO₂)= -217 kJ/mol $\Delta$ G°_f (SiO₂)= -856 kJ/mol

Choose the substance with the higher entropy per mole at a given temperature: Br₂(l)or Br₂(g).

For the reaction CuS(s)+ H₂(g) $\rarr$ H₂S(g)+ Cu(s), $\Delta$ G°_f (CuS)= -53.6 kJ/mol $\Delta$ G°_f (H₂S)= -33.6 kJ/mol $\Delta$ H°_f (CuS)= -53.1 kJ/mol $\Delta$ H°_f (H₂S)= -20.6 kJ/mol Calculate the value of the equilibrium constant (K_p)at 798 K and 1 atm pressure.

For the reaction CuS(s)+ H₂(g) $\rarr$ H₂S(g)+ Cu(s), $\Delta$ G°_f (CuS)= -53.6 kJ/mol $\Delta$ G°_f (H₂S)= -33.6 kJ/mol $\Delta$ H°_f (CuS)= -53.1 kJ/mol $\Delta$ H°_f (H₂S)= -20.6 kJ/mol Will this reaction proceed spontaneously at 298 K and 1 atm pressure?

For the reaction 3H₂(g)+ N₂(g) $\rarr$ 2NH₃(g), K_c = 9.0 at 350°C. What is the value of $\Delta$ G at this temperature when 1.0 mol NH₃, 5.0 mol N₂, and 5.0 mol H₂ are mixed in a 2.5 L reactor?