Consider the following reaction at equilibrium: 2SO2 (g) + O2 (g) 2SO3 (g) OH° = - 99 kJ Le Cha^telier's principle predicts that an increase in temperature will result in .

A) the partial pressure of O2 will decrease B) a decrease in the partial pressure of SO3 C) a decrease in the partial pressure of SO2 D) an increase in Keq E) no changes in equilibrium partial pressures A) the partial pressure of O2 will decrease B) a decrease in the partial pressure of SO3 C) a decrease in the partial pressure of SO2 D) an increase in Keq E) no changes in equilibrium partial pressures

Kp = 0.0198 at 721 K for the reaction 2HI (g) H2 (g) + I2 (g) In a particular experiment, the partial pressures of H2 and I2 at equilibrium are 0.710 and 0.888 atm, respectively. The partial pressure of HI is atm.

A) 7.87 B) 1.98 C) 0.125 D) 0.389 E) 5.64 A) 7.87 B) 1.98 C) 0.125 D) 0.389 E) 5.64

At 400 K, the equilibrium constant for the reaction Br2 (g) + Cl2 (g) 2BrCl (g) Is Kp = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br2 (g), 1.00 atm of Cl2 (g), and 2.00 Atm of BrCl (g). Use Q to determine which of the statements below is true.

A) At equilibrium, the total pressure in the vessel will be less than the initial total pressure. B) The equilibrium partial pressures of Br2, Cl2, and BrCl will be the same as the initial values. C) The equilibrium partial pressure of BrCl (g) will be greater than 2.00 atm. D) The reaction will go to completion since there are equal amounts of Br2 and Cl2. E) The equilibrium partial pressure of Br2 will be greater than 1.00 atm. A) At equilibrium, the total pressure in the vessel will be less than the initial total pressure. B) The equilibrium partial pressures of Br2, Cl2, and BrCl will be the same as the initial values. C) The equilibrium partial pressure of BrCl (g) will be greater than 2.00 atm. D) The reaction will go to completion since there are equal amounts of Br2 and Cl2. E) The equilibrium partial pressure of Br2 will be greater than 1.00 atm.

The equilibrium constant (Kp) for the interconversion of PCl5 and PCl3 is 0.0121: PCl5 (g) PCl3 (g) + Cl2 (g) A vessel is charged with PCl5, giving an initial pressure of 0.123 atm. At equilibrium, the partial Pressure of PCl3 is _ atm.

A) 0.123 B) 0.078 C) 0.033 D) 0.045 E) 0.090 A) 0.123 B) 0.078 C) 0.033 D) 0.045 E) 0.090

Dinitrogentetraoxide partially decomposes according to the following equilibrium: N2O4 (g) -2NO2 (g) A 1)000- L flask is charged with 3.00 × 10- 2 mol of N2O4. At equilibrium, 2.36 × 10- 2 mol of N2O4 remains. Keq for this reaction is .

A) 0.391 B) 0.723 C) 6.93 × 10- 3 D) 1.92 × 10- 4 E) 0.212 A) 0.391 B) 0.723 C) 6.93 × 10- 3 D) 1.92 × 10- 4 E) 0.212

Dinitrogentetraoxide partially decomposes according to the following equilibrium: N2O4 (g) 2NO2 (g) A 1)00- L flask is charged with 0.400 mol of N2O4. At equilibrium at 373 K, 0.0055 mol of N2O4 remains. Keq for this reaction is .

A) 2.2 × 10- 4 B) 0.22 C) 0.87 D) 13 E) 0.022 A) 2.2 × 10- 4 B) 0.22 C) 0.87 D) 13 E) 0.022

Consider the following reaction at equilibrium: 2CO2 (g) 2CO (g) + O2 (g) OH° = - 514 kJ Le Cha^telier's principle predicts that an increase in temperature will .

A) increase the value of the equilibrium constant B) decrease the partial pressure of CO2 (g) C) decrease the value of the equilibrium constant D) increase the partial pressure of O2 (g) E) increase the partial pressure of CO A) increase the value of the equilibrium constant B) decrease the partial pressure of CO2 (g) C) decrease the value of the equilibrium constant D) increase the partial pressure of O2 (g) E) increase the partial pressure of CO

A) all chemical reactions have ceased B) the rate constants of the forward and reverse reactions are equal C) the rates of the forward and reverse reactions are equal D) the value of the equilibrium constant is 1 E) the limiting reagent has been consumed A) all chemical reactions have ceased B) the rate constants of the forward and reverse reactions are equal C) the rates of the forward and reverse reactions are equal D) the value of the equilibrium constant is 1 E) the limiting reagent has been consumed

The value of Keq for the equilibrium H2 (g) + I2 (g) 2 HI (g) Is 794 at 25 °C. What is the value of Keq for the equilibrium below? 1/2 H2 (g) + 1/2 I2 (g) HI (g)

A) 397 B) 0.035 C) 1588 D) 28 E) 0.0013 A) 397 B) 0.035 C) 1588 D) 28 E) 0.0013

Exam 15: Chemical Equilibrium

Consider the following reaction at equilibrium: 2SO₂(g) + O₂(g) 2SO₃(g) OH° = - 99 kJ Le Cha^{^}telier's principle predicts that an increase in temperature will result in .

(Multiple Choice)

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Question 21

The relationship between the concentrations of reactants and products of a system at equilibrium is given by the law of mass action.

(True/False)

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Question 22

Consider the following reaction at equilibrium: Le Cha^{^}telier's principle predicts that adding O₂(g) to the reaction container will _ .

(Multiple Choice)

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Question 23

Acetic acid is a weak acid that dissociates into the acetate ion and a proton in aqueous solution: HC₂H₃O₂(aq) C₂H₃O₂^-(aq) + H⁺(aq) At equilibrium at 25 °C a 0.100 M solution of acetic acid has the following concentrations: [HC₂H₃O₂] = 0.0990 M, [C₂H₃O₂^-] = 1.33 × 10^-³M, and [H⁺] = 1.33 × 10^-³M. The equilibrium Constant, K_eq, for the ionization of acetic acid at 25 °C is _ .

(Multiple Choice)

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Question 24

The reaction below is exothermiC: 2SO₂(g) + O₂(g) 2SO₃(g) Le Cha^{^}telier's Principle predicts that will result in an increase in the number of moles of SO₃(g) in the reaction container.

(Multiple Choice)

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Question 25

K_p= 0.0198 at 721 K for the reaction 2HI (g) H₂(g) + I₂(g) In a particular experiment, the partial pressures of H₂and I₂at equilibrium are 0.710 and 0.888 atm, respectively. The partial pressure of HI is atm.

(Multiple Choice)

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Question 26

In what year was Fritz Haber awarded the Nobel Prize in chemistry for his development of a process for synthesizing ammonia directly from nitrogen and hydrogen?

(Multiple Choice)

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Question 27

At 400 K, the equilibrium constant for the reaction Br₂(g) + Cl₂(g) 2BrCl (g) Is K_p= 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br₂(g), 1.00 atm of Cl₂(g), and 2.00 Atm of BrCl (g). Use Q to determine which of the statements below is true.

(Multiple Choice)

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Question 28

The equilibrium constant (K_p) for the reaction below is 7.00 × 10^-²at 22 °C: A sample of NH₄HS is placed in an evacuated container and allowed to come to equilibrium. The partial pressure of NH₃is then increased by the addition of 0.590 atm of NH₃. The partial pressure of H₂S at equilibrium is now atm.

(Multiple Choice)

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Question 29

The effect of a catalyst on a chemical reaction is to react with product, effectively removing it and shifting the equilibrium to the right.

(True/False)

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Question 30

The equilibrium constant (K_p) for the interconversion of PCl₅and PCl₃is 0.0121: PCl₅(g) PCl₃(g) + Cl₂(g) A vessel is charged with PCl₅, giving an initial pressure of 0.123 atm. At equilibrium, the partial Pressure of PCl₃is _ atm.

(Multiple Choice)

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Question 31

Dinitrogentetraoxide partially decomposes according to the following equilibrium: N₂O₄(g) -2NO₂(g) A 1)000- L flask is charged with 3.00 × 10^-²mol of N₂O₄. At equilibrium, 2.36 × 10^-²mol of N₂O₄remains. K_eqfor this reaction is .

(Multiple Choice)

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Question 32

If the value for the equilibrium constant is much greater than 1, then the equilibrium mixture contains mostly .

(Short Answer)

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Question 33

The equilibrium constant for the gas phase reaction Is K_eq= 230 at 300 °C. At equilibrium, _ _.

(Multiple Choice)

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Question 34

Dinitrogentetraoxide partially decomposes according to the following equilibrium: N₂O₄(g) 2NO₂(g) A 1)00- L flask is charged with 0.400 mol of N₂O₄. At equilibrium at 373 K, 0.0055 mol of N₂O₄remains. K_eqfor this reaction is .

(Multiple Choice)

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Question 35

Consider the following reaction at equilibrium: 2CO₂(g) 2CO (g) + O₂(g) OH° = - 514 kJ Le Cha^{^}telier's principle predicts that an increase in temperature will .

(Multiple Choice)

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Question 36

At equilibrium, .

(Multiple Choice)

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Question 37

The value of K_eqfor the equilibrium H₂(g) + I₂(g) 2 HI (g) Is 794 at 25 °C. What is the value of K_eqfor the equilibrium below? 1/2 H₂(g) + 1/2 I₂(g) HI (g)

(Multiple Choice)

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Question 38

How does the reaction quotient of a reaction (Q) differ from the equilibrium constant (K_eq) of the same reaction?

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Question 39

Consider the following reaction at equilibrium. 2CO₂(g) 2CO (g) + O₂(g) OH° = - 514 kJ Le Cha^{^}telier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction .

(Multiple Choice)

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Question 40

Showing 21 - 40 of 58

Exam 15: Chemical Equilibrium

Consider the following reaction at equilibrium: 2SO2 (g) + O2 (g) 2SO3 (g) OH° = - 99 kJ Le Cha^telier's principle predicts that an increase in temperature will result in .

The relationship between the concentrations of reactants and products of a system at equilibrium is given by the law of mass action.

Consider the following reaction at equilibrium: Le Cha^telier's principle predicts that adding O2 (g) to the reaction container will _ .

The reaction below is exothermiC: 2SO2 (g) + O2 (g) 2SO3 (g) Le Cha^telier's Principle predicts that will result in an increase in the number of moles of SO3 (g) in the reaction container.

Kp = 0.0198 at 721 K for the reaction 2HI (g) H2 (g) + I2 (g) In a particular experiment, the partial pressures of H2 and I2 at equilibrium are 0.710 and 0.888 atm, respectively. The partial pressure of HI is atm.

In what year was Fritz Haber awarded the Nobel Prize in chemistry for his development of a process for synthesizing ammonia directly from nitrogen and hydrogen?

At 400 K, the equilibrium constant for the reaction Br2 (g) + Cl2 (g) 2BrCl (g) Is Kp = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br2 (g), 1.00 atm of Cl2 (g), and 2.00 Atm of BrCl (g). Use Q to determine which of the statements below is true.

The effect of a catalyst on a chemical reaction is to react with product, effectively removing it and shifting the equilibrium to the right.

The equilibrium constant (Kp) for the interconversion of PCl5 and PCl3 is 0.0121: PCl5 (g) PCl3 (g) + Cl2 (g) A vessel is charged with PCl5, giving an initial pressure of 0.123 atm. At equilibrium, the partial Pressure of PCl3 is _ atm.

Dinitrogentetraoxide partially decomposes according to the following equilibrium: N2O4 (g) -2NO2 (g) A 1)000- L flask is charged with 3.00 × 10- 2 mol of N2O4. At equilibrium, 2.36 × 10- 2 mol of N2O4 remains. Keq for this reaction is .

If the value for the equilibrium constant is much greater than 1, then the equilibrium mixture contains mostly .

The equilibrium constant for the gas phase reaction Is Keq = 230 at 300 °C. At equilibrium, _ _.

Dinitrogentetraoxide partially decomposes according to the following equilibrium: N2O4 (g) 2NO2 (g) A 1)00- L flask is charged with 0.400 mol of N2O4. At equilibrium at 373 K, 0.0055 mol of N2O4 remains. Keq for this reaction is .

Consider the following reaction at equilibrium: 2CO2 (g) 2CO (g) + O2 (g) OH° = - 514 kJ Le Cha^telier's principle predicts that an increase in temperature will .

At equilibrium, .

The value of Keq for the equilibrium H2 (g) + I2 (g) 2 HI (g) Is 794 at 25 °C. What is the value of Keq for the equilibrium below? 1/2 H2 (g) + 1/2 I2 (g) HI (g)

How does the reaction quotient of a reaction (Q) differ from the equilibrium constant (Keq) of the same reaction?

Consider the following reaction at equilibrium. 2CO2 (g) 2CO (g) + O2 (g) OH° = - 514 kJ Le Cha^telier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction .

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Consider the following reaction at equilibrium: 2SO₂(g) + O₂(g) 2SO₃(g) OH° = - 99 kJ Le Cha^{^}telier's principle predicts that an increase in temperature will result in .

Consider the following reaction at equilibrium: Le Cha^{^}telier's principle predicts that adding O₂(g) to the reaction container will _ .

The reaction below is exothermiC: 2SO₂(g) + O₂(g) 2SO₃(g) Le Cha^{^}telier's Principle predicts that will result in an increase in the number of moles of SO₃(g) in the reaction container.

K_p= 0.0198 at 721 K for the reaction 2HI (g) H₂(g) + I₂(g) In a particular experiment, the partial pressures of H₂and I₂at equilibrium are 0.710 and 0.888 atm, respectively. The partial pressure of HI is atm.

At 400 K, the equilibrium constant for the reaction Br₂(g) + Cl₂(g) 2BrCl (g) Is K_p= 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br₂(g), 1.00 atm of Cl₂(g), and 2.00 Atm of BrCl (g). Use Q to determine which of the statements below is true.

The equilibrium constant (K_p) for the interconversion of PCl₅and PCl₃is 0.0121: PCl₅(g) PCl₃(g) + Cl₂(g) A vessel is charged with PCl₅, giving an initial pressure of 0.123 atm. At equilibrium, the partial Pressure of PCl₃is _ atm.

Dinitrogentetraoxide partially decomposes according to the following equilibrium: N₂O₄(g) -2NO₂(g) A 1)000- L flask is charged with 3.00 × 10^-²mol of N₂O₄. At equilibrium, 2.36 × 10^-²mol of N₂O₄remains. K_eqfor this reaction is .

The equilibrium constant for the gas phase reaction Is K_eq= 230 at 300 °C. At equilibrium, _ _.

Dinitrogentetraoxide partially decomposes according to the following equilibrium: N₂O₄(g) 2NO₂(g) A 1)00- L flask is charged with 0.400 mol of N₂O₄. At equilibrium at 373 K, 0.0055 mol of N₂O₄remains. K_eqfor this reaction is .

Consider the following reaction at equilibrium: 2CO₂(g) 2CO (g) + O₂(g) OH° = - 514 kJ Le Cha^{^}telier's principle predicts that an increase in temperature will .

The value of K_eqfor the equilibrium H₂(g) + I₂(g) 2 HI (g) Is 794 at 25 °C. What is the value of K_eqfor the equilibrium below? 1/2 H₂(g) + 1/2 I₂(g) HI (g)

How does the reaction quotient of a reaction (Q) differ from the equilibrium constant (K_eq) of the same reaction?

Consider the following reaction at equilibrium. 2CO₂(g) 2CO (g) + O₂(g) OH° = - 514 kJ Le Cha^{^}telier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction .