In the gas phase, methyl isocyanate (CH3NC)isomerizes to acetonitrile (CH3CN), H3C-N$\equiv$C (g) H3C-C$\equiv$N (g) With $\Delta$H° = -89.5 kJ/mol and $\Delta$G° = - 73.8 kJ/mol at 25°C. Find the equilibrium constant for this reaction at 100°C.

A) 1.68 $\times$ 10-10 B) 5.96 $\times$ 109 C) 2.16 $\times$ 1010 D) 4.63 $\times$ 10-11 E) 8.64 $\times$ 1012 A) 1.68 $\times$ 10-10 B) 5.96 $\times$ 109 C) 2.16 $\times$ 1010 D) 4.63 $\times$ 10-11 E) 8.64 $\times$ 1012

For the reaction CuS(s)+ H2(g) 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.

The answer of For the reaction CuS(s)+ H2(g) ...

Given the following data, estimate the boiling point of bromine, Br2, assuming that $\Delta$S° and $\Delta$H° are temperature-independent.

The answer of Given the following data, estimate the boiling...

Nitrosyl chloride (NOCl)decomposes at elevated temperatures according to the equation 2NOCl(g) 2NO(g)+ Cl2(g). Calculate Kp for this reaction at 227°C.($\Delta$H° = 81.2 kJ/mol, $\Delta$S° = 128 J/K·mol)

A) 1.59 $\times$ 10-2 B) 2.10 $\times$ 10-7 C) 62.8 D) 4.90 $\times$ 106 E) 3.20 $\times$ 109 A) 1.59 $\times$ 10-2 B) 2.10 $\times$ 10-7 C) 62.8 D) 4.90 $\times$ 106 E) 3.20 $\times$ 109

Calculate $\Delta$G° for the combustion of ethanol vapor, C2H5OH(g), at 750°C in oxygen to form carbon dioxide and water vapor. The following data is valid at 25°C:

A) -1407 kJ/mol B) -2151 kJ/mol C) -1307 kJ/mol D) -4486 kJ/mol E) -1377 kJ/mol A) -1407 kJ/mol B) -2151 kJ/mol C) -1307 kJ/mol D) -4486 kJ/mol E) -1377 kJ/mol

Find the temperature at which the reaction N2O4(g) 2NO2(g)will be in equilibrium when both gases are present at partial pressures of 1.00 atm.

A) 300°C B) 28°C C) 55°C D) 32°C E) 562°C A) 300°C B) 28°C C) 55°C D) 32°C E) 562°C

At 700 K, the equilibrium constant for the reaction CO(g)+ H2O(g) CO2(g)+ H2(g)is 5.10.What is $\Delta$G° for this reaction at this temperature?

The answer of At 700 K, the equilibrium constant for...

Without reference to a table, arrange these reactions according to increasing $\Delta$S. 1)CH4(g)+ H2O(g)$\to$ CO(g)+ 3H2(g) 2)C(s)+ O2(g)$\to$ CO2(g) 3)H2O2(l)$\to$ H2O(l)+ 1/2O2(g)

A) 1 < 3 < 2 B) 2 < 3 < 1 C) 2 < 1 < 3 D) 3 < 2 < 1 E) 3 < 1 < 2 A) 1 < 3 < 2 B) 2 < 3 < 1 C) 2 < 1 < 3 D) 3 < 2 < 1 E) 3 < 1 < 2

The following reaction is nonspontaneous at 25°C: Cu2O(s)$\to$ 2Cu(s)+ 1/2O2(g), $\Delta$G° = 141 kJ/mol If $\Delta$S° = 75.8 J/K·mol, what is the lowest temperature at which the reaction will be spontaneous?

The answer of The following reaction is nonspontaneous at 25°C: Cu2O(s)$\to$...

Exam 18: Entropy, Free Energy, and Equilibrium

In the gas phase, methyl isocyanate (CH₃NC)isomerizes to acetonitrile (CH₃CN), H₃C-N $\equiv$ C (g) $In the gas phase, methyl isocyanate (CH3NC)isomerizes to acetonitrile (CH3CN), H3C-N \equiv C (g) H3C-C \equiv N (g) With \Delta H° = -89.5 kJ/mol and \Delta G° = - 73.8 kJ/mol at 25°C. Find the equilibrium constant for this reaction at 100°C.$ H₃C-C $\equiv$ N (g) With $\Delta$ H° = -89.5 kJ/mol and $\Delta$ G° = - 73.8 kJ/mol at 25°C. Find the equilibrium constant for this reaction at 100°C.

(Multiple Choice)

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Question 21

For the reaction H₂O₂(g) $\to$ H₂O(g)+ ¹/₂O₂(g), $\Delta$ H° = -106 kJ/mol and $\Delta$ S° = 58 J/K·mol at 25°C. Calculate $\Delta$ G° for this reaction at this temperature.

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Question 22

For the reaction SbCl₅(g) $For the reaction SbCl5(g) SbCl3(g)+ Cl2(g), \Delta G°f (SbCl5)= -334.34 kJ/mol \Delta G°f (SbCl3)= -301.25 kJ/mol \Delta H°f (SbCl5)= -394.34 kJ/mol \Delta H°f (SbCl3)= -313.80 kJ/mol Calculate the value of the equilibrium constant (Kp)for this reaction at 298 K.$ 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 Calculate the value of the equilibrium constant (K_p)for this reaction at 298 K.

(Short Answer)

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Question 23

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

(Short Answer)

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Question 24

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

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Question 25

The reaction rates of many spontaneous reactions are actually very slow. Which of these statements is the best explanation for this observation?

(Multiple Choice)

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Question 26

The free energy of formation of nitric oxide, NO, at 1000 K (roughly the temperature in an automobile engine during ignition)is about 78 kJ/mol.Calculate the equilibrium constant K_p for the reaction N₂(g)+ O₂(g) 2NO(g)at this temperature.

(Short Answer)

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Question 27

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

(Multiple Choice)

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Question 28

Given the following data, estimate the boiling point of bromine, Br₂, assuming that $\Delta$ S° and $\Delta$ H° are temperature-independent. $Given the following data, estimate the boiling point of bromine, Br2, assuming that \Delta S° and \Delta H° are temperature-independent.$

(Short Answer)

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Question 29

Calculate the free energy of formation of NaBr(s)given the following information: NaBr(s) $\to$ Na(s)+ ¹/₂Br₂(l), $\Delta$ G° = 349 kJ/mol

(Short Answer)

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Question 30

The normal freezing point of ammonia is -78°C. Predict the signs of $\Delta$ H, $\Delta$ S, and $\Delta$ G for ammonia when it freezes at -80°C and 1 atm: NH₃(l) $\to$ NH₃(s) $The normal freezing point of ammonia is -78°C. Predict the signs of \Delta H, \Delta S, and \Delta G for ammonia when it freezes at -80°C and 1 atm: NH3(l) \to NH3(s)$

(Short Answer)

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Question 31

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

(Short Answer)

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Question 32

Dissolving an ionic solid in water always results in an increase in entropy.

(True/False)

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Question 33

Nitrosyl chloride (NOCl)decomposes at elevated temperatures according to the equation 2NOCl(g) $Nitrosyl chloride (NOCl)decomposes at elevated temperatures according to the equation 2NOCl(g) 2NO(g)+ Cl2(g). Calculate Kp for this reaction at 227°C.( \Delta H° = 81.2 kJ/mol, \Delta S° = 128 J/K·mol)$ 2NO(g)+ Cl₂(g). Calculate K_p for this reaction at 227°C.( $\Delta$ H° = 81.2 kJ/mol, $\Delta$ S° = 128 J/K·mol)

(Multiple Choice)

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Question 34

Calculate $\Delta$ G° for the combustion of ethanol vapor, C₂H₅OH(g), at 750°C in oxygen to form carbon dioxide and water vapor. The following data is valid at 25°C: $Calculate \Delta G° for the combustion of ethanol vapor, C2H5OH(g), at 750°C in oxygen to form carbon dioxide and water vapor. The following data is valid at 25°C:$

(Multiple Choice)

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Question 35

Find the temperature at which the reaction N₂O₄(g) 2NO₂(g)will be in equilibrium when both gases are present at partial pressures of 1.00 atm.

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Question 36

At 700 K, the equilibrium constant for the reaction CO(g)+ H₂O(g) $At 700 K, the equilibrium constant for the reaction CO(g)+ H2O(g) CO2(g)+ H2(g)is 5.10.What is \Delta G° for this reaction at this temperature?$ CO₂(g)+ H₂(g)is 5.10.What is $\Delta$ G° for this reaction at this temperature?

(Short Answer)

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Question 37

Without reference to a table, arrange these reactions according to increasing $\Delta$ S. 1)CH₄(g)+ H₂O(g) $\to$ CO(g)+ 3H₂(g) 2)C(s)+ O₂(g) $\to$ CO₂(g) 3)H₂O₂(l) $\to$ H₂O(l)+ ¹/₂O₂(g)

(Multiple Choice)

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Question 38

A negative sign for $\Delta$ G indicates that, at constant T and P,

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Question 39

The following reaction is nonspontaneous at 25°C: Cu₂O(s) $\to$ 2Cu(s)+ ¹/₂O₂(g), $\Delta$ G° = 141 kJ/mol If $\Delta$ S° = 75.8 J/K·mol, what is the lowest temperature at which the reaction will be spontaneous?

(Short Answer)

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Question 40

Showing 21 - 40 of 112

For the reaction H₂O₂(g) $\to$ H₂O(g)+ ¹/₂O₂(g), $\Delta$ H° = -106 kJ/mol and $\Delta$ S° = 58 J/K·mol at 25°C. Calculate $\Delta$ G° for this reaction at this temperature.

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

The reaction rates of many spontaneous reactions are actually very slow. Which of these statements is the best explanation for this observation?

The free energy of formation of nitric oxide, NO, at 1000 K (roughly the temperature in an automobile engine during ignition)is about 78 kJ/mol.Calculate the equilibrium constant K_p for the reaction N₂(g)+ O₂(g) 2NO(g)at this temperature.

Given the following data, estimate the boiling point of bromine, Br₂, assuming that $\Delta$ S° and $\Delta$ H° are temperature-independent. $Given the following data, estimate the boiling point of bromine, Br<sub>2</sub>, assuming that \Delta S° and \Delta H° are temperature-independent.$

Calculate the free energy of formation of NaBr(s)given the following information: NaBr(s) $\to$ Na(s)+ ¹/₂Br₂(l), $\Delta$ G° = 349 kJ/mol

Dissolving an ionic solid in water always results in an increase in entropy.

Find the temperature at which the reaction N₂O₄(g) 2NO₂(g)will be in equilibrium when both gases are present at partial pressures of 1.00 atm.

Without reference to a table, arrange these reactions according to increasing $\Delta$ S. 1)CH₄(g)+ H₂O(g) $\to$ CO(g)+ 3H₂(g) 2)C(s)+ O₂(g) $\to$ CO₂(g) 3)H₂O₂(l) $\to$ H₂O(l)+ ¹/₂O₂(g)

A negative sign for $\Delta$ G indicates that, at constant T and P,

The following reaction is nonspontaneous at 25°C: Cu₂O(s) $\to$ 2Cu(s)+ ¹/₂O₂(g), $\Delta$ G° = 141 kJ/mol If $\Delta$ S° = 75.8 J/K·mol, what is the lowest temperature at which the reaction will be spontaneous?

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Exam 18: Entropy, Free Energy, and Equilibrium

In the gas phase, methyl isocyanate (CH3NC)isomerizes to acetonitrile (CH3CN), H3C-N ≡\equiv≡ C (g) H3C-C ≡\equiv≡ N (g) With Δ\DeltaΔ H° = -89.5 kJ/mol and Δ\DeltaΔ G° = - 73.8 kJ/mol at 25°C. Find the equilibrium constant for this reaction at 100°C.

For the reaction H2O2(g) →\to→ H2O(g)+ 1/2O2(g), Δ\DeltaΔ H° = -106 kJ/mol and Δ\DeltaΔ S° = 58 J/K·mol at 25°C. Calculate Δ\DeltaΔ G° for this reaction at this temperature.

For the reaction SbCl5(g) 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 Calculate the value of the equilibrium constant (Kp)for this reaction at 298 K.

For the reaction CuS(s)+ H2(g) 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.

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

The reaction rates of many spontaneous reactions are actually very slow. Which of these statements is the best explanation for this observation?

The free energy of formation of nitric oxide, NO, at 1000 K (roughly the temperature in an automobile engine during ignition)is about 78 kJ/mol.Calculate the equilibrium constant Kp for the reaction N2(g)+ O2(g) 2NO(g)at this temperature.

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

Given the following data, estimate the boiling point of bromine, Br2, assuming that Δ\DeltaΔ S° and Δ\DeltaΔ H° are temperature-independent.

Calculate the free energy of formation of NaBr(s)given the following information: NaBr(s) →\to→ Na(s)+ 1/2Br2(l), Δ\DeltaΔ G° = 349 kJ/mol

The normal freezing point of ammonia is -78°C. Predict the signs of Δ\DeltaΔ H, Δ\DeltaΔ S, and Δ\DeltaΔ G for ammonia when it freezes at -80°C and 1 atm: NH3(l) →\to→ NH3(s)

For the reaction 3H2(g)+ N2(g) 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?

Dissolving an ionic solid in water always results in an increase in entropy.

Nitrosyl chloride (NOCl)decomposes at elevated temperatures according to the equation 2NOCl(g) 2NO(g)+ Cl2(g). Calculate Kp for this reaction at 227°C.( Δ\DeltaΔ H° = 81.2 kJ/mol, Δ\DeltaΔ S° = 128 J/K·mol)

Calculate Δ\DeltaΔ G° for the combustion of ethanol vapor, C2H5OH(g), at 750°C in oxygen to form carbon dioxide and water vapor. The following data is valid at 25°C:

Find the temperature at which the reaction N2O4(g) 2NO2(g)will be in equilibrium when both gases are present at partial pressures of 1.00 atm.

At 700 K, the equilibrium constant for the reaction CO(g)+ H2O(g) CO2(g)+ H2(g)is 5.10.What is Δ\DeltaΔ G° for this reaction at this temperature?

Without reference to a table, arrange these reactions according to increasing Δ\DeltaΔ S. 1)CH4(g)+ H2O(g) →\to→ CO(g)+ 3H2(g) 2)C(s)+ O2(g) →\to→ CO2(g) 3)H2O2(l) →\to→ H2O(l)+ 1/2O2(g)

A negative sign for Δ\DeltaΔ G indicates that, at constant T and P,

The following reaction is nonspontaneous at 25°C: Cu2O(s) →\to→ 2Cu(s)+ 1/2O2(g), Δ\DeltaΔ G° = 141 kJ/mol If Δ\DeltaΔ S° = 75.8 J/K·mol, what is the lowest temperature at which the reaction will be spontaneous?

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For the reaction H₂O₂(g) $\to$ H₂O(g)+ ¹/₂O₂(g), $\Delta$ H° = -106 kJ/mol and $\Delta$ S° = 58 J/K·mol at 25°C. Calculate $\Delta$ G° for this reaction at this temperature.

The free energy of formation of nitric oxide, NO, at 1000 K (roughly the temperature in an automobile engine during ignition)is about 78 kJ/mol.Calculate the equilibrium constant K_p for the reaction N₂(g)+ O₂(g) 2NO(g)at this temperature.

Given the following data, estimate the boiling point of bromine, Br₂, assuming that $\Delta$ S° and $\Delta$ H° are temperature-independent. $Given the following data, estimate the boiling point of bromine, Br<sub>2</sub>, assuming that \Delta S° and \Delta H° are temperature-independent.$

Calculate the free energy of formation of NaBr(s)given the following information: NaBr(s) $\to$ Na(s)+ ¹/₂Br₂(l), $\Delta$ G° = 349 kJ/mol

Find the temperature at which the reaction N₂O₄(g) 2NO₂(g)will be in equilibrium when both gases are present at partial pressures of 1.00 atm.

Without reference to a table, arrange these reactions according to increasing $\Delta$ S. 1)CH₄(g)+ H₂O(g) $\to$ CO(g)+ 3H₂(g) 2)C(s)+ O₂(g) $\to$ CO₂(g) 3)H₂O₂(l) $\to$ H₂O(l)+ ¹/₂O₂(g)

A negative sign for $\Delta$ G indicates that, at constant T and P,

The following reaction is nonspontaneous at 25°C: Cu₂O(s) $\to$ 2Cu(s)+ ¹/₂O₂(g), $\Delta$ G° = 141 kJ/mol If $\Delta$ S° = 75.8 J/K·mol, what is the lowest temperature at which the reaction will be spontaneous?