For the equilibrium N2O4(g) 2NO2(g),at 298 K,Kp = 0.15.For this reaction system,it is found that the partial pressure of N2O4 is 3.5 × 10-2 atm at equilibrium.What is the partial pressure of NO2 at equilibrium? (R = 0.0821 L ∙ atm/(K ∙ mol))

A) 4.8 atm B) 23 atm C) 0.0018 atm D) 0.0052 atm E) 0.072 atm A) 4.8 atm B) 23 atm C) 0.0018 atm D) 0.0052 atm E) 0.072 atm E

Consider the following equilibrium: 2NO(g)+ 3F2(g) 2NOF3(g) Suppose 0.20 mol of NO and 0.30 mol of F2 are added to a 5.0-L container.If x mol of NOF3 is present at equilibrium,how many moles of fluorine are present at equilibrium?

A) 0.30 - x B) 0.30 - 2x C) 0.06 - 0.20x D) 0.30 - x E) 0.20 - x A) 0.30 - x B) 0.30 - 2x C) 0.06 - 0.20x D) 0.30 - x E) 0.20 - x

One method for the decomposition of carbon dioxide proceeds as follows: 2CO2(g) 2CO(g)+ O2(g); ΔH = 559 kJ Which of the following changes will cause an increase in the equilibrium concentration of CO?

A) adding more O2 to the system B) adding a catalyst C) removing CO2 from the system D) increasing the pressure of the system at constant temperature E) increasing the temperature of the system A) adding more O2 to the system B) adding a catalyst C) removing CO2 from the system D) increasing the pressure of the system at constant temperature E) increasing the temperature of the system

Exactly 1.0 mol N2O4 is placed in an empty 1.0-L container and allowed to reach equilibrium described by the equation N2O4(g) 2NO2(g). If at equilibrium the N2O4 is 28.0% dissociated,what is the value of the equilibrium constant,Kc,for the reaction under these conditions?

A) 0.44 B) 2.3 C) 0.31 D) 0.78 E) 0.11 A) 0.44 B) 2.3 C) 0.31 D) 0.78 E) 0.11

Solid HgO,liquid Hg,and gaseous O2 are placed in a glass bulb and allowed to reach equilibrium. 2HgO(s) 2Hg(l)+ O2(g); ΔH = 181.6 kJ The amount of Hg(l)in the bulb could be increased

A) by removing some HgO(s). B) by adding an inert gas. C) by adding some HgO(s). D) by increasing the pressure. E) by increasing the temperature. A) by removing some HgO(s). B) by adding an inert gas. C) by adding some HgO(s). D) by increasing the pressure. E) by increasing the temperature.

Consider the following equilibrium: 1/2N2O4(g) NO2(g); Kc = 3.3 at 100°C For which of the following equilibria is Kc less than 3.3 at 100°C?

A) 1/4N2O4(g) 1/2NO2(g) B) N2O4(g) 2NO2(g) C) 4N2O4(g) 8NO2(g) D) 3N2O4(g) 6NO2(g) E) 2N2O4(g) 4NO2(g) A) 1/4N2O4(g) 1/2NO2(g) B) N2O4(g) 2NO2(g) C) 4N2O4(g) 8NO2(g) D) 3N2O4(g) 6NO2(g) E) 2N2O4(g) 4NO2(g)

At 298 K,the value of Kc for the reaction H2(g)+ Br2(g) 2HBr(g)is 2.0 × 1019.What is Kc for HBr(g) 1/2H2(g)+ 1/2Br2(g)?

A) 4.0 × 10-38 B) 5.0 × 10-20 C) 1.0 × 1019 D) -2.0 × 1019 E) 2.2 × 10-10 A) 4.0 × 10-38 B) 5.0 × 10-20 C) 1.0 × 1019 D) -2.0 × 1019 E) 2.2 × 10-10

Exam 14: Chemical Equilibrium

For the equilibrium N₂O₄(g) 2NO₂(g),at 298 K,K_p = 0.15.For this reaction system,it is found that the partial pressure of N₂O₄ is 3.5 × 10^-2 atm at equilibrium.What is the partial pressure of NO₂ at equilibrium? (R = 0.0821 L ∙ atm/(K ∙ mol))

Free

(Multiple Choice)

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Question 1

Correct Answer:

Verified

What balanced equation is the following equilibrium expression derived from?

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(Multiple Choice)

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Question 2

Correct Answer:

Verified

For which of the following systems at equilibrium and at constant temperature will decreasing the volume cause the equilibrium to shift to the right?

Free

(Multiple Choice)

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Question 3

Correct Answer:

Verified

Consider the following equilibrium: 2NO(g)+ 3F₂(g) 2NOF₃(g) Suppose 0.20 mol of NO and 0.30 mol of F₂ are added to a 5.0-L container.If x mol of NOF₃ is present at equilibrium,how many moles of fluorine are present at equilibrium?

(Multiple Choice)

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Question 4

Which of the following equilibria would not be affected by pressure changes at constant temperature?

(Multiple Choice)

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Question 5

What is the expression for K_c for the following equilibrium? CaSO₃(s) CaO(s)+ SO₂(g)

(Multiple Choice)

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Question 6

One method for the decomposition of carbon dioxide proceeds as follows: 2CO₂(g) 2CO(g)+ O₂(g); ΔH = 559 kJ Which of the following changes will cause an increase in the equilibrium concentration of CO?

(Multiple Choice)

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Question 7

Exactly 1.0 mol N₂O₄ is placed in an empty 1.0-L container and allowed to reach equilibrium described by the equation N₂O₄(g) 2NO₂(g). If at equilibrium the N₂O₄ is 28.0% dissociated,what is the value of the equilibrium constant,K_c,for the reaction under these conditions?

(Multiple Choice)

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Question 8

Which of the following equilibria would be affected by volume changes at constant temperature?

(Multiple Choice)

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Question 9

Solid HgO,liquid Hg,and gaseous O₂ are placed in a glass bulb and allowed to reach equilibrium. 2HgO(s) 2Hg(l)+ O₂(g); ΔH = 181.6 kJ The amount of Hg(l)in the bulb could be increased

(Multiple Choice)

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Question 10

Which of the following statements is true in a reaction system at equilibrium?

(Multiple Choice)

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Question 11

What is the balanced equation for the following equilibrium expression?

(Multiple Choice)

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Question 12

For which of the following values of the equilibrium constant does the reaction mixture contain mostly products?

(Multiple Choice)

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Question 13

Consider the following system at equilibrium: N₂(g)+ 3H₂(g) 2NH₃(g); ΔH° = -92.94 kJ Which of the following changes will shift the equilibrium to the right? I.increasing the temperature II.decreasing the temperature III.increasing the volume IV.decreasing the volume V.removing some NH₃ VI.adding some NH₃ VII.removing some N₂ VIII.adding some N₂

(Multiple Choice)

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Question 14

The reaction quotient for a system is .If the equilibrium constant for the system is ,what will happen as the reaction mixture approaches equilibrium?

(Multiple Choice)

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Question 15

Consider the reaction S₂Cl₂(l)+ CCl₄(l) CS₂(g)+ 3Cl₂(g); ΔH° = 84.3 kJ If the above reactants and products are contained in a closed vessel and the reaction system is at equilibrium,the number of moles of CS₂ can be increased by

(Multiple Choice)

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Question 16

Which expression correctly describes the equilibrium constant K_c for the following reaction? 2C₂H₂(g)+ 5O₂(g) 4CO₂(g)+ 2H₂O(g)

(Multiple Choice)

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Question 17

Consider the following equilibrium: 1/2N₂O₄(g) NO₂(g); K_c = 3.3 at 100°C For which of the following equilibria is K_c less than 3.3 at 100°C?

(Multiple Choice)

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Question 18

At 298 K,the value of K_c for the reaction H₂(g)+ Br₂(g) 2HBr(g)is 2.0 × 10¹⁹.What is K_c for HBr(g) 1/2H₂(g)+ 1/2Br₂(g)?

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Question 19

A(n)_____ is a substance that increases the rate of a reaction but is not consumed by it.

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Question 20

Showing 1 - 20 of 97

Exam 14: Chemical Equilibrium

For the equilibrium N2O4(g) 2NO2(g),at 298 K,Kp = 0.15.For this reaction system,it is found that the partial pressure of N2O4 is 3.5 × 10-2 atm at equilibrium.What is the partial pressure of NO2 at equilibrium? (R = 0.0821 L ∙ atm/(K ∙ mol))

What balanced equation is the following equilibrium expression derived from?

For which of the following systems at equilibrium and at constant temperature will decreasing the volume cause the equilibrium to shift to the right?

Consider the following equilibrium: 2NO(g)+ 3F2(g) 2NOF3(g) Suppose 0.20 mol of NO and 0.30 mol of F2 are added to a 5.0-L container.If x mol of NOF3 is present at equilibrium,how many moles of fluorine are present at equilibrium?

Which of the following equilibria would not be affected by pressure changes at constant temperature?

What is the expression for Kc for the following equilibrium? CaSO3(s) CaO(s)+ SO2(g)

One method for the decomposition of carbon dioxide proceeds as follows: 2CO2(g) 2CO(g)+ O2(g); ΔH = 559 kJ Which of the following changes will cause an increase in the equilibrium concentration of CO?

Exactly 1.0 mol N2O4 is placed in an empty 1.0-L container and allowed to reach equilibrium described by the equation N2O4(g) 2NO2(g). If at equilibrium the N2O4 is 28.0% dissociated,what is the value of the equilibrium constant,Kc,for the reaction under these conditions?

Which of the following equilibria would be affected by volume changes at constant temperature?

Solid HgO,liquid Hg,and gaseous O2 are placed in a glass bulb and allowed to reach equilibrium. 2HgO(s) 2Hg(l)+ O2(g); ΔH = 181.6 kJ The amount of Hg(l)in the bulb could be increased

Which of the following statements is true in a reaction system at equilibrium?

What is the balanced equation for the following equilibrium expression?

For which of the following values of the equilibrium constant does the reaction mixture contain mostly products?

The reaction quotient for a system is .If the equilibrium constant for the system is ,what will happen as the reaction mixture approaches equilibrium?

Consider the reaction S2Cl2(l)+ CCl4(l) CS2(g)+ 3Cl2(g); ΔH° = 84.3 kJ If the above reactants and products are contained in a closed vessel and the reaction system is at equilibrium,the number of moles of CS2 can be increased by

Which expression correctly describes the equilibrium constant Kc for the following reaction? 2C2H2(g)+ 5O2(g) 4CO2(g)+ 2H2O(g)

Consider the following equilibrium: 1/2N2O4(g) NO2(g); Kc = 3.3 at 100°C For which of the following equilibria is Kc less than 3.3 at 100°C?

At 298 K,the value of Kc for the reaction H2(g)+ Br2(g) 2HBr(g)is 2.0 × 1019.What is Kc for HBr(g) 1/2H2(g)+ 1/2Br2(g)?

A(n)_____ is a substance that increases the rate of a reaction but is not consumed by it.

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For the equilibrium N₂O₄(g) 2NO₂(g),at 298 K,K_p = 0.15.For this reaction system,it is found that the partial pressure of N₂O₄ is 3.5 × 10^-2 atm at equilibrium.What is the partial pressure of NO₂ at equilibrium? (R = 0.0821 L ∙ atm/(K ∙ mol))

Consider the following equilibrium: 2NO(g)+ 3F₂(g) 2NOF₃(g) Suppose 0.20 mol of NO and 0.30 mol of F₂ are added to a 5.0-L container.If x mol of NOF₃ is present at equilibrium,how many moles of fluorine are present at equilibrium?

What is the expression for K_c for the following equilibrium? CaSO₃(s) CaO(s)+ SO₂(g)

One method for the decomposition of carbon dioxide proceeds as follows: 2CO₂(g) 2CO(g)+ O₂(g); ΔH = 559 kJ Which of the following changes will cause an increase in the equilibrium concentration of CO?

Exactly 1.0 mol N₂O₄ is placed in an empty 1.0-L container and allowed to reach equilibrium described by the equation N₂O₄(g) 2NO₂(g). If at equilibrium the N₂O₄ is 28.0% dissociated,what is the value of the equilibrium constant,K_c,for the reaction under these conditions?

Solid HgO,liquid Hg,and gaseous O₂ are placed in a glass bulb and allowed to reach equilibrium. 2HgO(s) 2Hg(l)+ O₂(g); ΔH = 181.6 kJ The amount of Hg(l)in the bulb could be increased

Consider the reaction S₂Cl₂(l)+ CCl₄(l) CS₂(g)+ 3Cl₂(g); ΔH° = 84.3 kJ If the above reactants and products are contained in a closed vessel and the reaction system is at equilibrium,the number of moles of CS₂ can be increased by

Which expression correctly describes the equilibrium constant K_c for the following reaction? 2C₂H₂(g)+ 5O₂(g) 4CO₂(g)+ 2H₂O(g)

Consider the following equilibrium: 1/2N₂O₄(g) NO₂(g); K_c = 3.3 at 100°C For which of the following equilibria is K_c less than 3.3 at 100°C?

At 298 K,the value of K_c for the reaction H₂(g)+ Br₂(g) 2HBr(g)is 2.0 × 10¹⁹.What is K_c for HBr(g) 1/2H₂(g)+ 1/2Br₂(g)?