Suppose 75.0 g of PCl5(g)is introduced into a 3.00 L vessel containing 10.0 g of Cl2(g),and the system is allowed to reach equilibrium at 250ºC. PCl5(g) PCl3(g)+ Cl2(g) If KP = 1.80 for this reaction,what is the total pressure inside the vessel at equilibrium? (R = 0.08206 L • atm/K • mol)

A) 6.83 atm B) 8.86 atm C) 5.38 atm D) 3.47 atm E) 1.68 atm A) 6.83 atm B) 8.86 atm C) 5.38 atm D) 3.47 atm E) 1.68 atm

Nitrogen dioxide decomposes according to the reaction 2NO2(g) 2NO(g)+ O2(g) Where KP = 4.48 × 10-13 at 25°C.What is the value for Kc?(R = 0.08206 L • atm/K • mol)

A) 1.83 × 10-14 B) 4.48 × 10-14 C) 9.19 × 10-13 D) 2.18 × 10-13 E) 1.10 × 10-11 A) 1.83 × 10-14 B) 4.48 × 10-14 C) 9.19 × 10-13 D) 2.18 × 10-13 E) 1.10 × 10-11

Find the temperature at which KP = 42.0 for the reaction H2(g)+ I2(g) 2HI(g). [Given: at 25°C,for H2(g),ΔH°f = 0,S° = 131.0 J/mol • K; for I2(g),ΔH°f = 62.26 kJ/mol,S° =260.6 J/mol • K; for HI(g),ΔH°f = 25.9 kJ/mol,S° = 206.3 J/mol • K; assume that ΔH° and ΔS° Are independent of temperature.]

A) 1040 K B) 168 K C) 539 K D) 1400 K E) 34,200 K A) 1040 K B) 168 K C) 539 K D) 1400 K E) 34,200 K

When the reaction 2H2S(g) 2H2(g)+ S2(g)is carried out at 1065°C,KP = 0.012.Starting with pure H2S at 1065°C,what must the initial pressure of H2S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H2(g)?

A) 1.06 atm B) 1.86 atm C) 0.94 atm D) 0.90 atm E) 1.52 atm A) 1.06 atm B) 1.86 atm C) 0.94 atm D) 0.90 atm E) 1.52 atm

Exam 15: Chemical Equilibrium

The solubility product constant,K_sp,at 25°C for AgI(s)in water has the value 8.3 × 10^-17. Calculate ΔG at 25°C for the process AgI(s) Ag⁺(aq)+ I^-(aq)where [Ag⁺] = 9.1 × 10^-9 M and [I^-] = 9.1 × 10^-9 M.(R = 8.314 J/K • mol)

(Multiple Choice)

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Question 101

Suppose 75.0 g of PCl₅(g)is introduced into a 3.00 L vessel containing 10.0 g of Cl2(g),and the system is allowed to reach equilibrium at 250ºC. PCl₅(g) PCl₃(g)+ Cl₂(g) If K_P = 1.80 for this reaction,what is the total pressure inside the vessel at equilibrium? (R = 0.08206 L • atm/K • mol)

(Multiple Choice)

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Question 102

Suppose 50.0 g of N₂O₄ is introduced into an evacuated 2.00-L vessel and allowed to come to equilibrium with its decomposition product,N₂O₄(g) 2NO₂(g).For this reaction K_c = 0.133.Once the system has reached equilibrium,5.00 g of NO₂ is injected into the vessel,and the system is allowed to equilibrate once again.What is the mass of N2O4 in the final equilibrium mixture?

(Multiple Choice)

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Question 103

What is defined as a fraction with equilibrium product concentrations in the numerator and equilibrium reactant concentrations in the denominator and each concentration raised to a power equal to the corresponding stoichiometric coefficient in the balanced chemical equation?

(Multiple Choice)

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Question 104

For the following reaction at equilibrium,which choice gives a change that will shift the position of equilibrium to favor formation of more products? 2NOBr(g) 2NO(g)+ Br₂(g),ΔHº_rxn = 30 kJ/mol

(Multiple Choice)

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Question 105

Nitrogen dioxide decomposes according to the reaction 2NO₂(g) 2NO(g)+ O₂(g) Where K_P = 4.48 × 10^-13 at 25°C.What is the value for K_c?(R = 0.08206 L • atm/K • mol)

(Multiple Choice)

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Question 106

Suppose 25.0 g of HI(g)is injected into a 4.00-L reaction vessel that contains 20.0 g of I₂(g). When the system comes to equilibrium at 400.ºC,what will be the total pressure inside the reaction vessel? (R = 0.08206 L • atm/K • mol) 2HI(g) H₂(g)+ I₂(g),K_c = 0.0156 at 400.ºC

(Multiple Choice)

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Question 107

A temperature increase favors an endothermic reaction.

(True/False)

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Question 108

For the reaction of A + B C + D + heat,the reverse reaction is exothermic.

(True/False)

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Question 109

The equilibrium constant for the reaction AgBr(s) Ag⁺(aq)+ Br^- (aq)is the solubility product constant,K_sp = 7.7 × 10^-13 at 25°C.Calculate ΔG 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? (R = 8.314 J/K • mol)

(Multiple Choice)

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Question 110

Consider the reaction N₂(g)+ O₂(g) 2NO(g),for which K_c = 0.10 at 2000ºC.Starting with initial concentrations of 0.040 M for N₂ and 0.040 M for O₂ ,what is the equilibrium concentration of NO?

(Multiple Choice)

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Question 111

Which is the correct equilibrium constant expression for the following reaction? FeO(s)+ H₂(g) Fe(s)+ H₂O(g)

(Multiple Choice)

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Question 112

At 450°C,tert-butyl alcohol decomposes into water and isobutene. (CH₃)3COH(g) (CH₃)₂CCH₂(g)+ H₂O(g) A reaction vessel contains these compounds at equilibrium.What will happen if the volume of the container is reduced by 50% at constant temperature?

(Multiple Choice)

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Question 113

For the endothermic reaction A₂(g) 2A(g),a snapshot of an equilibrium mixture of A(g) and A₂(g)may look as follows.(Each circle represents 1.0 mol of A atoms,and the volume of the box is 1.0 L.) What is the equilibrium constant K_c for this reaction at 298 K? (R = 0.08206 L • atm/K • mol)

(Multiple Choice)

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Question 114

The standard free energy of formation of gaseous hydrogen iodide is 1.30 kJ/mol at 25°C.What is K_P for the reaction H₂(g)+ I₂(g) 2HI(g)at this temperature?

(Multiple Choice)

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Question 115

At equilibrium,the rate of the forward reaction is equal to the rate of the reverse reaction.

(True/False)

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Question 116

Find the temperature at which K_P = 42.0 for the reaction H₂(g)+ I₂(g) 2HI(g). [Given: at 25°C,for H₂(g),ΔH°_f = 0,S° = 131.0 J/mol • K; for I₂(g),ΔH°_f = 62.26 kJ/mol,S° =260.6 J/mol • K; for HI(g),ΔH°_f = 25.9 kJ/mol,S° = 206.3 J/mol • K; assume that ΔH° and ΔS° Are independent of temperature.]

(Multiple Choice)

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Question 117

Consider the reaction N₂(g)+ 3H₂(g) 2NH₃(g).If nitrogen is added to the system at equilibrium,what will happen to the ammonia concentration?

(Short Answer)

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Question 118

When the reaction 2H₂S(g) 2H₂(g)+ S₂(g)is carried out at 1065°C,K_P = 0.012.Starting with pure H₂S at 1065°C,what must the initial pressure of H₂S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H₂(g)?

(Multiple Choice)

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Question 119

For the equilibrium A₂(g) 2A(g),if a sample of A₂(g)is placed in a sealed container and allowed to come to equilibrium,which graph best represents the relationship between Q_c and time as equilibrium is established?

(Multiple Choice)

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Question 120

Showing 101 - 120 of 135

Exam 15: Chemical Equilibrium

The solubility product constant,Ksp,at 25°C for AgI(s)in water has the value 8.3 × 10-17. Calculate ΔG at 25°C for the process AgI(s) Ag+(aq)+ I-(aq)where [Ag+] = 9.1 × 10-9 M and [I-] = 9.1 × 10-9 M.(R = 8.314 J/K • mol)

Suppose 75.0 g of PCl5(g)is introduced into a 3.00 L vessel containing 10.0 g of Cl2(g),and the system is allowed to reach equilibrium at 250ºC. PCl5(g) PCl3(g)+ Cl2(g) If KP = 1.80 for this reaction,what is the total pressure inside the vessel at equilibrium? (R = 0.08206 L • atm/K • mol)

What is defined as a fraction with equilibrium product concentrations in the numerator and equilibrium reactant concentrations in the denominator and each concentration raised to a power equal to the corresponding stoichiometric coefficient in the balanced chemical equation?

For the following reaction at equilibrium,which choice gives a change that will shift the position of equilibrium to favor formation of more products? 2NOBr(g) 2NO(g)+ Br2(g),ΔHºrxn = 30 kJ/mol

Nitrogen dioxide decomposes according to the reaction 2NO2(g) 2NO(g)+ O2(g) Where KP = 4.48 × 10-13 at 25°C.What is the value for Kc?(R = 0.08206 L • atm/K • mol)

Suppose 25.0 g of HI(g)is injected into a 4.00-L reaction vessel that contains 20.0 g of I2(g). When the system comes to equilibrium at 400.ºC,what will be the total pressure inside the reaction vessel? (R = 0.08206 L • atm/K • mol) 2HI(g) H2(g)+ I2(g),Kc = 0.0156 at 400.ºC

A temperature increase favors an endothermic reaction.

For the reaction of A + B C + D + heat,the reverse reaction is exothermic.

Consider the reaction N2(g)+ O2(g) 2NO(g),for which Kc = 0.10 at 2000ºC.Starting with initial concentrations of 0.040 M for N2 and 0.040 M for O2 ,what is the equilibrium concentration of NO?

Which is the correct equilibrium constant expression for the following reaction? FeO(s)+ H2(g) Fe(s)+ H2O(g)

At 450°C,tert-butyl alcohol decomposes into water and isobutene. (CH3)3COH(g) (CH3)2CCH2(g)+ H2O(g) A reaction vessel contains these compounds at equilibrium.What will happen if the volume of the container is reduced by 50% at constant temperature?

For the endothermic reaction A2(g) 2A(g),a snapshot of an equilibrium mixture of A(g) and A2(g)may look as follows.(Each circle represents 1.0 mol of A atoms,and the volume of the box is 1.0 L.) What is the equilibrium constant Kc for this reaction at 298 K? (R = 0.08206 L • atm/K • mol)

The standard free energy of formation of gaseous hydrogen iodide is 1.30 kJ/mol at 25°C.What is KP for the reaction H2(g)+ I2(g) 2HI(g)at this temperature?

At equilibrium,the rate of the forward reaction is equal to the rate of the reverse reaction.

Consider the reaction N2(g)+ 3H2(g) 2NH3(g).If nitrogen is added to the system at equilibrium,what will happen to the ammonia concentration?

When the reaction 2H2S(g) 2H2(g)+ S2(g)is carried out at 1065°C,KP = 0.012.Starting with pure H2S at 1065°C,what must the initial pressure of H2S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H2(g)?

For the equilibrium A2(g) 2A(g),if a sample of A2(g)is placed in a sealed container and allowed to come to equilibrium,which graph best represents the relationship between Qc and time as equilibrium is established?

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The solubility product constant,K_sp,at 25°C for AgI(s)in water has the value 8.3 × 10^-17. Calculate ΔG at 25°C for the process AgI(s) Ag⁺(aq)+ I^-(aq)where [Ag⁺] = 9.1 × 10^-9 M and [I^-] = 9.1 × 10^-9 M.(R = 8.314 J/K • mol)

For the following reaction at equilibrium,which choice gives a change that will shift the position of equilibrium to favor formation of more products? 2NOBr(g) 2NO(g)+ Br₂(g),ΔHº_rxn = 30 kJ/mol

Nitrogen dioxide decomposes according to the reaction 2NO₂(g) 2NO(g)+ O₂(g) Where K_P = 4.48 × 10^-13 at 25°C.What is the value for K_c?(R = 0.08206 L • atm/K • mol)

Suppose 25.0 g of HI(g)is injected into a 4.00-L reaction vessel that contains 20.0 g of I₂(g). When the system comes to equilibrium at 400.ºC,what will be the total pressure inside the reaction vessel? (R = 0.08206 L • atm/K • mol) 2HI(g) H₂(g)+ I₂(g),K_c = 0.0156 at 400.ºC

Consider the reaction N₂(g)+ O₂(g) 2NO(g),for which K_c = 0.10 at 2000ºC.Starting with initial concentrations of 0.040 M for N₂ and 0.040 M for O₂ ,what is the equilibrium concentration of NO?

Which is the correct equilibrium constant expression for the following reaction? FeO(s)+ H₂(g) Fe(s)+ H₂O(g)

At 450°C,tert-butyl alcohol decomposes into water and isobutene. (CH₃)3COH(g) (CH₃)₂CCH₂(g)+ H₂O(g) A reaction vessel contains these compounds at equilibrium.What will happen if the volume of the container is reduced by 50% at constant temperature?

For the endothermic reaction A₂(g) 2A(g),a snapshot of an equilibrium mixture of A(g) and A₂(g)may look as follows.(Each circle represents 1.0 mol of A atoms,and the volume of the box is 1.0 L.) What is the equilibrium constant K_c for this reaction at 298 K? (R = 0.08206 L • atm/K • mol)

The standard free energy of formation of gaseous hydrogen iodide is 1.30 kJ/mol at 25°C.What is K_P for the reaction H₂(g)+ I₂(g) 2HI(g)at this temperature?

Consider the reaction N₂(g)+ 3H₂(g) 2NH₃(g).If nitrogen is added to the system at equilibrium,what will happen to the ammonia concentration?

When the reaction 2H₂S(g) 2H₂(g)+ S₂(g)is carried out at 1065°C,K_P = 0.012.Starting with pure H₂S at 1065°C,what must the initial pressure of H₂S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H₂(g)?

For the equilibrium A₂(g) 2A(g),if a sample of A₂(g)is placed in a sealed container and allowed to come to equilibrium,which graph best represents the relationship between Q_c and time as equilibrium is established?