Question 1

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

Accepted Answer

8.90

10^-1²

Question 2

How does the entropy change when a molecular solid is dissolved in water?

Accepted Answer

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

Question 3

Using the thermodynamic data provided below, calculate Ka for HCN(aq)at 25°.

Accepted Answer

2.8

10^-9...

Question 4

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)at 800 K and 1 atm pressure.

Accepted Answer

1.11 <img  loading="lazy" src="/assets/images/blured-textbook.svg" class="d-inline m-1" alt="blured image" width="139" height="30"> 10<s...

Question 5

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

Accepted Answer

A)  SiF4(g) 4(g) 
B)  HF(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)  F) B) and D)
G) A) and C)

Question 6

Ozone (O3) in the atmosphere can reaction with nitric oxide (NO) : O3(g) + NO(g)  →	o→  NO2(g) + O2(g) .
Calculate the  Δ\DeltaΔ G° for this reaction at 25°C. ( Δ\DeltaΔ H° = -199 kJ/mol,  Δ\DeltaΔ S° = -4.1 J/K·mol)

Accepted Answer

A)  1020 kJ/mol
B)  -1.22  ×	imes×  103 kJ/mol
C)  2.00  ×	imes×  103 kJ/mol
D)  -1.42  ×	imes×  103 kJ/mol
E)  -198 kJ/mol F) C) and D)
G) B) and D)

Question 7

Determine the equilibrium constant (Kp) at 25°C for the reaction p) at 25°C for the reaction   A) 2.9  	imes  10-60 B) 1.0  	imes  10-4 C) 1.2 D) 1.0  	imes  105 E) 3.4  	imes  1059 " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  2.9  ×	imes×  10-60
B)  1.0  ×	imes×  10-4
C)  1.2
D)  1.0  ×	imes×  105
E)  3.4  ×	imes×  1059 F) B) and C)
G) A) and D)

Question 8

Which species will have the lowest absolute entropy at 25°C?

Accepted Answer

A)  C2H5OH(l) 
B)  C2H2(g) 
C)  C3H8(g) 
D)  C3H7OH(l) 
E)  C2H6(g) F) None of the above
G) D) and E)

Question 9

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) .

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 F) A) and B)
G) A) and C)

Question 10

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. Is H2O2(g)stable with respect to dissociation into water vapor and oxygen gas at 25°C?

Accepted Answer

The answer of For the reaction H2O2(g)$\to$ H2O(g)+ 1/2O2(g), $\Delta$H°...

Question 11

Using the thermodynamic data provided below, determine the temperature in °C at which the decomposition of solid calcium carbonate to form solid calcium oxide and oxygen becomes spontaneous.

Accepted Answer

The answer of Using the thermodynamic data provided below, determine...

Question 12

Kw for the auto-ionization of water, H2O(l)  →	o→  H+(aq) + OH- (aq) , is 1.0  ×	imes×  10-14. What are the signs (+/-) of  Δ\DeltaΔ S° and  Δ\DeltaΔ H° for the reaction at 25°C?

Accepted Answer

A)  ( Δ\DeltaΔ S° = (+) and  Δ\DeltaΔ H° = (+) ) 
B)  ( Δ\DeltaΔ S° = (+) and  Δ\DeltaΔ H° = (-) ) 
C)  ( Δ\DeltaΔ S° = (-) and  Δ\DeltaΔ H° = (+) ) 
D)  ( Δ\DeltaΔ S° = (-) and  Δ\DeltaΔ H° = (-) )  E) A) and B)
F) A) and C)

Question 13

Determine the equilibrium constant Kp at 25°C for the reaction N2(g) + 3H2(g)  p at 25°C for the reaction N2(g) + 3H2(g)    2NH3(g)  [ \Delta G°f (NH3(g) ) = -16.6 kJ/mol]. A) 1.52  	imes  10-6 B) 6.60  	imes  105 C) 8.28  	imes  10-2 D) 2.60 E) 13.4 " class="answers-bank-image d-inline" rel="preload" > 2NH3(g)  [ Δ\DeltaΔ G°f (NH3(g) ) = -16.6 kJ/mol].

Accepted Answer

A)  1.52  ×	imes×  10-6
B)  6.60  ×	imes×  105
C)  8.28  ×	imes×  10-2
D)  2.60
E)  13.4 F) A) and B)
G) All of the above

Question 14

Predict the sign of $\Delta$S for the reaction O2(g)$\to$ 2O(g).

Accepted Answer

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

Question 15

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)for this reaction at 298 K.

Accepted Answer

3.11 <img  loading="lazy" src="/assets/images/blured-textbook.svg" class="d-inline m-1" alt="blured image" width="139" height="30"> 10<s...

Question 16

For a certain reaction, $\Delta$G° = 87 kJ/mol, $\Delta$H° = 100 kJ/mol at STP. At what temperature, in K, is the reaction in equilibrium, assuming that $\Delta$S° and $\Delta$H° are temperature-independent?

Accepted Answer

The answer of For a certain reaction, $\Delta$G° = 87...

Question 17

What is the free energy change for the reaction SiO2(s)+ Pb(s)$\to$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 18

Aluminum forms a layer of aluminum oxide when exposed to air which protects the bulk metal from further corrosion. 4Al(s) + 3O2(g)  →	o→ 2Al2O3(s) 
Using the thermodynamic data provided below, calculate  Δ\DeltaΔ S° for this reaction. 2(g)  	o 2Al2O3(s)  Using the thermodynamic data provided below, calculate  \Delta S° for this reaction.   A) 182.3 J/K·mol B) 131.5 J/K·mol C) -182.3 J/K·mol D) -626.2 J/K·mol E) -802.9 J/K·mol " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  182.3 J/K·mol
B)  131.5 J/K·mol
C)  -182.3 J/K·mol
D)  -626.2 J/K·mol
E)  -802.9 J/K·mol F) B) and D)
G) A) and B)

Question 19

Hydrogen peroxide (H2O2) decomposes according to the equation H2O2(l) 2O(l) + 1/2O2(g) .Calculate Kp for this reaction at 25°C. (\Delta">→\0H₂O(l) +¹/₂O₂(g) .CalculateK_pforthisreactionat25°C.(Δ o\0 H₂O(l) + ¹/₂O₂(g) .Calculate K_p for this reaction at 25°C. (\Delta→\0H₂O(l) +¹/₂O₂(g) .CalculateK_pforthisreactionat25°C.(Δ H° = -98.2 kJ/mol, Δ\DeltaΔ S° = 70.1 J/K·mol)

Accepted Answer

A)  1.3  ×	imes×  10-21
B)  20.9
C)  3.46  ×	imes×  1017.
D)  7.5  ×	imes×  1020
E)  8.6  ×	imes×  104 F) A) and E)
G) B) and C)

Question 20

For the reaction 3H2(g)+ N2(g)  2NH3(g), Kc = 9.0 at 350°C. Calculate $\Delta$G° at 350°C.

Accepted Answer

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

Exam 18: Entropy, Free Energy, and Equilibrium

Using the thermodynamic data provided below, determine the temperature in °C at which the decomposition of solid calcium carbonate to form solid calcium oxide and oxygen becomes spontaneous.

Correct Answer
verified

Correct Answer
verified
3.11 10
View Answer

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. Is H₂O₂(g)stable with respect to dissociation into water vapor and oxygen gas at 25°C?

Correct Answer
verified

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

Correct Answer
verified
8.90 10^-1^{2View Answer}

Correct Answer
verified
1.11 10
View Answer

For a certain reaction, $\Delta$ G° = 87 kJ/mol, $\Delta$ H° = 100 kJ/mol at STP. At what temperature, in K, is the reaction in equilibrium, assuming that $\Delta$ S° and $\Delta$ H° are temperature-independent?

Correct Answer
verified

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

Correct Answer
verified

Predict the sign of $\Delta$ S for the reaction O₂(g) $\to$ 2O(g).

Correct Answer
verified

Which species will have the lowest absolute entropy at 25°C?

Correct Answer
verified

How does the entropy change when a molecular solid is dissolved in water?

Correct Answer
verified

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) .

Correct Answer
verified

Ozone (O₃) in the atmosphere can reaction with nitric oxide (NO) : O₃(g) + NO(g) $\to$ NO₂(g) + O₂(g) . Calculate the $\Delta$ G° for this reaction at 25°C. ( $\Delta$ H° = -199 kJ/mol, $\Delta$ S° = -4.1 J/K·mol)

Correct Answer
verified

For the reaction 3H₂(g)+ N₂(g) $For the reaction 3H<sub>2</sub>(g)+ N<sub>2</sub>(g) 2NH<sub>3</sub>(g), K<sub>c</sub> = 9.0 at 350°C. Calculate \Delta G° at 350°C.$ 2NH₃(g), K_c = 9.0 at 350°C. Calculate $\Delta$ G° at 350°C.

Correct Answer
verified

Hydrogen peroxide (H₂O₂) decomposes according to the equation H₂O₂(l) $\to\0 H<sub>2</sub>O(l) + <sup>1</sup>/<sub>2</sub>O<sub>2</sub>(g) .Calculate K<sub>p</sub> for this reaction at 25°C. (\Delta$ H° = -98.2 kJ/mol, $\Delta$ S° = 70.1 J/K·mol)

Correct Answer
verified

Correct Answer
verified

K_w for the auto-ionization of water, H₂O(l) $\to$ H⁺(aq) + OH^- (aq) , is 1.0 $\times$ 10^-14. What are the signs (+/-) of $\Delta$ S° and $\Delta$ H° for the reaction at 25°C?

Correct Answer
verified

Determine the equilibrium constant (K_p) at 25°C for the reaction $Determine the equilibrium constant (K<sub>p</sub>) at 25°C for the reaction A) 2.9 \times 10<sup>-60</sup> B) 1.0 \times 10<sup>-4</sup> C) 1.2 D) 1.0 \times 10<sup>5</sup> E) 3.4 \times 10<sup>59</sup>$

Correct Answer
verified

Using the thermodynamic data provided below, calculate K_a for HCN(aq)at 25°.

Correct Answer
verified
2.8 10^-9...
View Answer

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

Correct Answer
verified

Correct Answer
verified

Exam 18: Entropy, Free Energy, and Equilibrium

Using the thermodynamic data provided below, determine the temperature in °C at which the decomposition of solid calcium carbonate to form solid calcium oxide and oxygen becomes spontaneous.

Correct AnswerverifiedShow Answer

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)for this reaction at 298 K.

Correct Answerverified3.11 10View AnswerShow Answer

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. Is H2O2(g)stable with respect to dissociation into water vapor and oxygen gas at 25°C?

Correct AnswerverifiedShow Answer

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

Correct Answerverified8.90 10-12View AnswerShow Answer

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)at 800 K and 1 atm pressure.

Correct Answerverified1.11 10View AnswerShow Answer

For a certain reaction, Δ\DeltaΔ G° = 87 kJ/mol, Δ\DeltaΔ H° = 100 kJ/mol at STP. At what temperature, in K, is the reaction in equilibrium, assuming that Δ\DeltaΔ S° and Δ\DeltaΔ H° are temperature-independent?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Predict the sign of Δ\DeltaΔ S for the reaction O2(g) →\to→ 2O(g).

Correct AnswerverifiedShow Answer

Which species will have the lowest absolute entropy at 25°C?

Correct AnswerverifiedShow Answer

How does the entropy change when a molecular solid is dissolved in water?

Correct AnswerverifiedShow Answer

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) .

Correct AnswerverifiedShow Answer

Ozone (O3) in the atmosphere can reaction with nitric oxide (NO) : O3(g) + NO(g) →\to→ NO2(g) + O2(g) . Calculate the Δ\DeltaΔ G° for this reaction at 25°C. ( Δ\DeltaΔ H° = -199 kJ/mol, Δ\DeltaΔ S° = -4.1 J/K·mol)

Correct AnswerverifiedShow Answer

For the reaction 3H2(g)+ N2(g) 2NH3(g), Kc = 9.0 at 350°C. Calculate Δ\DeltaΔ G° at 350°C.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Aluminum forms a layer of aluminum oxide when exposed to air which protects the bulk metal from further corrosion. 4Al(s) + 3O2(g) →\to→ 2Al2O3(s) Using the thermodynamic data provided below, calculate Δ\DeltaΔ S° for this reaction.

Correct AnswerverifiedShow Answer

Kw for the auto-ionization of water, H2O(l) →\to→ H+(aq) + OH- (aq) , is 1.0 ×\times× 10-14. What are the signs (+/-) of Δ\DeltaΔ S° and Δ\DeltaΔ H° for the reaction at 25°C?

Correct AnswerverifiedShow Answer

Determine the equilibrium constant (Kp) at 25°C for the reaction

Correct AnswerverifiedShow Answer

Using the thermodynamic data provided below, calculate Ka for HCN(aq)at 25°.

Correct Answerverified2.8 10-9...View AnswerShow Answer

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

Correct AnswerverifiedShow Answer

Determine the equilibrium constant Kp at 25°C for the reaction N2(g) + 3H2(g) 2NH3(g) [ Δ\DeltaΔ G°f (NH3(g) ) = -16.6 kJ/mol].

Correct AnswerverifiedShow Answer

Correct Answer
verified

Correct Answer
verified
3.11 10
View Answer

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. Is H₂O₂(g)stable with respect to dissociation into water vapor and oxygen gas at 25°C?

Correct Answer
verified

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

Correct Answer
verified
8.90 10^-1^{2View Answer}

Correct Answer
verified
1.11 10
View Answer

For a certain reaction, $\Delta$ G° = 87 kJ/mol, $\Delta$ H° = 100 kJ/mol at STP. At what temperature, in K, is the reaction in equilibrium, assuming that $\Delta$ S° and $\Delta$ H° are temperature-independent?

Correct Answer
verified

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

Correct Answer
verified

Predict the sign of $\Delta$ S for the reaction O₂(g) $\to$ 2O(g).

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

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) .

Correct Answer
verified

Ozone (O₃) in the atmosphere can reaction with nitric oxide (NO) : O₃(g) + NO(g) $\to$ NO₂(g) + O₂(g) . Calculate the $\Delta$ G° for this reaction at 25°C. ( $\Delta$ H° = -199 kJ/mol, $\Delta$ S° = -4.1 J/K·mol)

Correct Answer
verified

For the reaction 3H₂(g)+ N₂(g) $For the reaction 3H<sub>2</sub>(g)+ N<sub>2</sub>(g) 2NH<sub>3</sub>(g), K<sub>c</sub> = 9.0 at 350°C. Calculate \Delta G° at 350°C.$ 2NH₃(g), K_c = 9.0 at 350°C. Calculate $\Delta$ G° at 350°C.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

K_w for the auto-ionization of water, H₂O(l) $\to$ H⁺(aq) + OH^- (aq) , is 1.0 $\times$ 10^-14. What are the signs (+/-) of $\Delta$ S° and $\Delta$ H° for the reaction at 25°C?

Correct Answer
verified

Determine the equilibrium constant (K_p) at 25°C for the reaction $Determine the equilibrium constant (K<sub>p</sub>) at 25°C for the reaction A) 2.9 \times 10<sup>-60</sup> B) 1.0 \times 10<sup>-4</sup> C) 1.2 D) 1.0 \times 10<sup>5</sup> E) 3.4 \times 10<sup>59</sup>$

Correct Answer
verified

Using the thermodynamic data provided below, calculate K_a for HCN(aq)at 25°.

Correct Answer
verified
2.8 10^-9...
View Answer

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

Correct Answer
verified

Correct Answer
verified