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The reaction system POCl3(g) The reaction system POCl<sub>3</sub>(g) POCl(g) + Cl<sub>2</sub>(g) Is at equilibrium. Which of the following statements describes the behavior of the system if POCl is added to the container? A) The forward reaction will proceed to establish equilibrium. B) The reverse reaction will proceed to establish equilibrium. C) The partial pressures of POCl<sub>3 </sub>and POCl will remain steady while the partial pressure of chlorine increases. D) The partial pressure of chlorine remains steady while the partial pressures of POCl<sub>3 </sub>and POCl increase. E) The partial pressure of chlorine will increase while the partial pressure of POCl decreases. POCl(g) + Cl2(g) Is at equilibrium. Which of the following statements describes the behavior of the system if POCl is added to the container?


A) The forward reaction will proceed to establish equilibrium.
B) The reverse reaction will proceed to establish equilibrium.
C) The partial pressures of POCl3 and POCl will remain steady while the partial pressure of chlorine increases.
D) The partial pressure of chlorine remains steady while the partial pressures of POCl3 and POCl increase.
E) The partial pressure of chlorine will increase while the partial pressure of POCl decreases.

F) C) and D)
G) All of the above

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Write the mass-action expression, Qc , for the following chemical reaction. MgO(s) + SO2(g) + Write the mass-action expression, Q<sub>c </sub>, for the following chemical reaction. MgO(s) + SO<sub>2</sub>(g) + O<sub>2</sub>(g) MgSO<sub>4</sub>(s) A) B) C) D) E) None of the above expressions is correct. O2(g) Write the mass-action expression, Q<sub>c </sub>, for the following chemical reaction. MgO(s) + SO<sub>2</sub>(g) + O<sub>2</sub>(g) MgSO<sub>4</sub>(s) A) B) C) D) E) None of the above expressions is correct. MgSO4(s)


A) Write the mass-action expression, Q<sub>c </sub>, for the following chemical reaction. MgO(s) + SO<sub>2</sub>(g) + O<sub>2</sub>(g) MgSO<sub>4</sub>(s) A) B) C) D) E) None of the above expressions is correct.
B) Write the mass-action expression, Q<sub>c </sub>, for the following chemical reaction. MgO(s) + SO<sub>2</sub>(g) + O<sub>2</sub>(g) MgSO<sub>4</sub>(s) A) B) C) D) E) None of the above expressions is correct.
C) Write the mass-action expression, Q<sub>c </sub>, for the following chemical reaction. MgO(s) + SO<sub>2</sub>(g) + O<sub>2</sub>(g) MgSO<sub>4</sub>(s) A) B) C) D) E) None of the above expressions is correct.
D) Write the mass-action expression, Q<sub>c </sub>, for the following chemical reaction. MgO(s) + SO<sub>2</sub>(g) + O<sub>2</sub>(g) MgSO<sub>4</sub>(s) A) B) C) D) E) None of the above expressions is correct.
E) None of the above expressions is correct.

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

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The reaction system POCl3(g) The reaction system POCl<sub>3</sub>(g) POCl(g) + Cl<sub>2</sub>(g) Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of chlorine is reduced by 50%? A) POCl<sub>3 </sub>will be consumed as equilibrium is established. B) POCl will be consumed as equilibrium is established. C) Chlorine will be consumed as equilibrium is established. D) The partial pressure of POCl will decrease while the partial pressure of Cl<sub>2</sub> increases as equilibrium is established. E) The volume will have to decrease before equilibrium can be reestablished. POCl(g) + Cl2(g) Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of chlorine is reduced by 50%?


A) POCl3 will be consumed as equilibrium is established.
B) POCl will be consumed as equilibrium is established.
C) Chlorine will be consumed as equilibrium is established.
D) The partial pressure of POCl will decrease while the partial pressure of Cl2 increases as equilibrium is established.
E) The volume will have to decrease before equilibrium can be reestablished.

F) A) and D)
G) B) and E)

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Consider the equilibrium: A(s) Consider the equilibrium: A(s) B(s) + C(g) <font face= symbol ></font>H°<sub>rxn</sub> > 0 Predict and explain how or whether the following actions would affect this equilibrium. a. adding more solid A b. lowering the temperature c. increasing the pressure on the system by reducing its volume d. adding helium gas to increase the total pressure B(s) + C(g) H°rxn > 0 Predict and explain how or whether the following actions would affect this equilibrium. a. adding more solid A b. lowering the temperature c. increasing the pressure on the system by reducing its volume d. adding helium gas to increase the total pressure

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a. No effect. Pure solids and liquids ha...

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The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N2(g) + O2(g) The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N<sub>2</sub>(g) + O<sub>2</sub>(g) 2NO(g) At 2000°C, the equilibrium constant, K<sub>c </sub>, has a value of 4.10 × 10<sup>-4</sup>. What is the value of K<sub>p</sub>? A) 2.17 × 10<sup>-8</sup> B) 4.10 × 10<sup>-4</sup> C) 7.65 × 10<sup>-2</sup> D) 7.75 E) none of the above 2NO(g) At 2000°C, the equilibrium constant, Kc , has a value of 4.10 × 10-4. What is the value of Kp?


A) 2.17 × 10-8
B) 4.10 × 10-4
C) 7.65 × 10-2
D) 7.75
E) none of the above

F) C) and E)
G) C) and D)

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At 25°C, the equilibrium constant Kc for the reaction 2A(aq) At 25°C, the equilibrium constant K<sub>c</sub> for the reaction 2A(aq) B(aq) + C(aq) Is 65. If 2.50 mol of A is added to enough water to prepare 1.00 L of solution, what will the equilibrium concentration of A be? A) 0.038 M B) 0.14 M C) 0.28 M D) 1.18 M E) 2.4 M B(aq) + C(aq) Is 65. If 2.50 mol of A is added to enough water to prepare 1.00 L of solution, what will the equilibrium concentration of A be?


A) 0.038 M
B) 0.14 M
C) 0.28 M
D) 1.18 M
E) 2.4 M

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

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A container was charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature? 3H2(g) + N2(g) A container was charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature? 3H<sub>2</sub>(g) + N<sub>2</sub>(g) 2NH<sub>3</sub>(g) A) There will be no effect. B) More ammonia will be produced at the expense of hydrogen and nitrogen. C) Hydrogen and nitrogen will be produced at the expense of ammonia. D) The equilibrium constant will increase. E) The equilibrium constant will decrease. 2NH3(g)


A) There will be no effect.
B) More ammonia will be produced at the expense of hydrogen and nitrogen.
C) Hydrogen and nitrogen will be produced at the expense of ammonia.
D) The equilibrium constant will increase.
E) The equilibrium constant will decrease.

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

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In order to write the correct mass-action expression for a reaction one must


A) know the kinetic rate law for the reaction.
B) know the mechanism for the reaction.
C) have a properly balanced chemical equation.
D) have values for the concentrations of the reactants.
E) know the limiting reactant.

F) A) and B)
G) B) and E)

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The following reaction is at equilibrium in a sealed container. N2(g) + 3H2(g) The following reaction is at equilibrium in a sealed container. N<sub>2</sub>(g) + 3H<sub>2</sub>(g) 2NH<sub>3</sub>(g) <font face= symbol ></font>H°<sub>rxn</sub> < 0 Which, if any, of the following actions will increase the value of the equilibrium constant, K<sub>c</sub>? A) adding a catalyst B) adding more N<sub>2</sub> C) increasing the pressure D) lowering the temperature E) none of the above 2NH3(g) H°rxn < 0 Which, if any, of the following actions will increase the value of the equilibrium constant, Kc?


A) adding a catalyst
B) adding more N2
C) increasing the pressure
D) lowering the temperature
E) none of the above

F) All of the above
G) A) and B)

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N2(g) + O2(g) N<sub>2</sub>(g) + O<sub>2</sub>(g) <sub> </sub> 2NO(g) K<sub>c</sub> = 4.8 × 10<sup>-31</sup> 2NOBr(g) <sub> </sub> 2NO(g) + Br<sub>2</sub>(g) K<sub>c</sub> = 0.50 Given the above equilibrium constant data at 25 °C, what is the value of K<sub>c</sub> at this temperature for the reaction 2NOBr(g) <sub> </sub> N<sub>2</sub>(g) + O<sub>2</sub>(g) + Br<sub>2</sub>(g) ? A) 2.4 × 10<sup>-31</sup> B) 9.6 × 10<sup>-31</sup> C) 1.0 × 10<sup>30</sup> D) 4.2 × 10<sup>30</sup> E) none of the above 2NO(g) Kc = 4.8 × 10-31 2NOBr(g) N<sub>2</sub>(g) + O<sub>2</sub>(g) <sub> </sub> 2NO(g) K<sub>c</sub> = 4.8 × 10<sup>-31</sup> 2NOBr(g) <sub> </sub> 2NO(g) + Br<sub>2</sub>(g) K<sub>c</sub> = 0.50 Given the above equilibrium constant data at 25 °C, what is the value of K<sub>c</sub> at this temperature for the reaction 2NOBr(g) <sub> </sub> N<sub>2</sub>(g) + O<sub>2</sub>(g) + Br<sub>2</sub>(g) ? A) 2.4 × 10<sup>-31</sup> B) 9.6 × 10<sup>-31</sup> C) 1.0 × 10<sup>30</sup> D) 4.2 × 10<sup>30</sup> E) none of the above 2NO(g) + Br2(g) Kc = 0.50 Given the above equilibrium constant data at 25 °C, what is the value of Kc at this temperature for the reaction 2NOBr(g) N<sub>2</sub>(g) + O<sub>2</sub>(g) <sub> </sub> 2NO(g) K<sub>c</sub> = 4.8 × 10<sup>-31</sup> 2NOBr(g) <sub> </sub> 2NO(g) + Br<sub>2</sub>(g) K<sub>c</sub> = 0.50 Given the above equilibrium constant data at 25 °C, what is the value of K<sub>c</sub> at this temperature for the reaction 2NOBr(g) <sub> </sub> N<sub>2</sub>(g) + O<sub>2</sub>(g) + Br<sub>2</sub>(g) ? A) 2.4 × 10<sup>-31</sup> B) 9.6 × 10<sup>-31</sup> C) 1.0 × 10<sup>30</sup> D) 4.2 × 10<sup>30</sup> E) none of the above N2(g) + O2(g) + Br2(g) ?


A) 2.4 × 10-31
B) 9.6 × 10-31
C) 1.0 × 1030
D) 4.2 × 1030
E) none of the above

F) All of the above
G) A) and E)

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The equilibrium constant, Kp, has a value of 6.5 × 10-4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl2(g) The equilibrium constant, K<sub>p</sub>, has a value of 6.5 × 10<sup>-4</sup> at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl<sub>2</sub>(g) 2NOCl(g) What is the value of K<sub>c</sub>? A) 2.5 × 10<sup>-7</sup> B) 6.5 × 10<sup>-4</sup> C) 1.6 × 10<sup>-2</sup> D) 1.7 E) none of the above 2NOCl(g) What is the value of Kc?


A) 2.5 × 10-7
B) 6.5 × 10-4
C) 1.6 × 10-2
D) 1.7
E) none of the above

F) A) and E)
G) All of the above

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The reaction quotient for a gas phase reaction has a value of 2000. If the number of moles of reactants in the reaction equation is equal to that of the products, which of the following statements is definitely true?


A) The reaction must proceed to the left to establish equilibrium.
B) The reaction must proceed to the right to establish equilibrium.
C) When the system is at equilibrium, the concentrations of the products will be much larger than the concentrations of the reactants.
D) The concentrations of the products are generally larger than the concentrations of the reactants.
E) None of the above statements is true.

F) A) and B)
G) A) and E)

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For a gas-phase equilibrium, a change in the pressure of any single reactant or product will affect the amounts of other substances involved in the equilibrium.

A) True
B) False

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Which of the following has an effect on the magnitude of the equilibrium constant?


A) removing products as they are formed
B) adding more of a reactant
C) adding a catalyst
D) increasing the pressure, in a gas-phase reaction
E) change in temperature

F) B) and E)
G) A) and E)

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A mixture of 0.600 mol of bromine and 1.600 mol of iodine is placed into a rigid 1.000-L container at 350°C. Br2(g) + I2(g) A mixture of 0.600 mol of bromine and 1.600 mol of iodine is placed into a rigid 1.000-L container at 350°C. Br<sub>2</sub>(g) + I<sub>2</sub>(g) 2IBr(g) When the mixture has come to equilibrium, the concentration of iodine monobromide is 1.190 M. What is the equilibrium constant for this reaction at 350°C? A) 3.55 × 10<sup>-3</sup> B) 1.24 C) 1.47 D) 282 E) 325 2IBr(g) When the mixture has come to equilibrium, the concentration of iodine monobromide is 1.190 M. What is the equilibrium constant for this reaction at 350°C?


A) 3.55 × 10-3
B) 1.24
C) 1.47
D) 282
E) 325

F) A) and B)
G) All of the above

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Once a reaction system reaches equilibrium, the concentrations of reactions and products no longer change.

A) True
B) False

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Methanol can be synthesized by combining carbon monoxide and hydrogen. CO(g) + 2H2(g) Methanol can be synthesized by combining carbon monoxide and hydrogen. CO(g) + 2H<sub>2</sub>(g) CH<sub>3</sub>OH(g) <font face= symbol ></font>H°<sub>rxn</sub> = -90.7 kJ A reaction vessel contains these compounds at equilibrium. What effect will be seen when equilibrium is re-established after decreasing the temperature by 45°C? A) All the partial pressures will decrease. B) The partial pressure of methanol will decrease. C) The partial pressures of hydrogen and methanol will decrease. D) The partial pressure of hydrogen will increase. E) The partial pressure of carbon monoxide will decrease. CH3OH(g) H°rxn = -90.7 kJ A reaction vessel contains these compounds at equilibrium. What effect will be seen when equilibrium is re-established after decreasing the temperature by 45°C?


A) All the partial pressures will decrease.
B) The partial pressure of methanol will decrease.
C) The partial pressures of hydrogen and methanol will decrease.
D) The partial pressure of hydrogen will increase.
E) The partial pressure of carbon monoxide will decrease.

F) B) and D)
G) None of the above

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The Haber process for ammonia synthesis is exothermic: N2(g) + 3H2(g) The Haber process for ammonia synthesis is exothermic: N<sub>2</sub>(g) + 3H<sub>2</sub>(g) 2NH<sub>3</sub>(g) <font face= symbol ></font>H° = -92 kJ If the equilibrium constant K<sub>c</sub> for this process at 500.°C is 6.0 × 10<sup>-2</sup>, what is its value at 300.°C? 2NH3(g) H° = -92 kJ If the equilibrium constant Kc for this process at 500.°C is 6.0 × 10-2, what is its value at 300.°C?

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a. State Le Chatelier's principle b. The following reaction is at equilibrium in a closed container: 2Fe(OH)3(s) a. State Le Chatelier's principle b. The following reaction is at equilibrium in a closed container: 2Fe(OH)<sub>3</sub>(s) Fe<sub>2</sub>O<sub>3</sub>(s) + 3H<sub>2</sub>O(g) <font face= symbol ></font>H°<sub>rxn</sub> > 0 What effects, if any, will the following actions have on the position of equilibrium? In each case, state the direction of any shift in equilibrium, and give your reasons in one sentence. (i) adding more Fe(OH)<sub>3</sub> (ii) raising the temperature (iii) adding a catalyst Fe2O3(s) + 3H2O(g) H°rxn > 0 What effects, if any, will the following actions have on the position of equilibrium? In each case, state the direction of any shift in equilibrium, and give your reasons in one sentence. (i) adding more Fe(OH)3 (ii) raising the temperature (iii) adding a catalyst

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a. If a stress is applied to a system at...

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Consider the equilibrium reaction: H2(g) + Br2(g) Consider the equilibrium reaction: H<sub>2</sub>(g) + Br<sub>2</sub>(g) 2HBr(g) Which of the following correctly describes the relationship between K<sub>c</sub> and K<sub>p</sub> for the reaction? A) K<sub>p</sub> = K<sub>c</sub> B) K<sub>p</sub> = (RT) K<sub>c</sub> C) K<sub>p</sub> = (RT) <sup>2</sup>K<sub>c</sub> D) K<sub>p</sub> = K<sub>c</sub>/RT E) K<sub>p</sub> = K<sub>c</sub>/(RT) <sup>2</sup> 2HBr(g) Which of the following correctly describes the relationship between Kc and Kp for the reaction?


A) Kp = Kc
B) Kp = (RT) Kc
C) Kp = (RT) 2Kc
D) Kp = Kc/RT
E) Kp = Kc/(RT) 2

F) A) and C)
G) A) and E)

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