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Carbon monoxide and chlorine combine in an equilibrium reaction to produce the highly toxic product, phosgene (COCl2) . Carbon monoxide and chlorine combine in an equilibrium reaction to produce the highly toxic product, phosgene (COCl<sub>2</sub>) . If the equilibrium constant for this reaction is K<sub>c</sub> = 248, predict, if possible, what will happen when the reactants and product are combined with the concentrations shown. [CO] = [Cl<sub>2</sub>] = 0.0200 M; [COCl<sub>2</sub>] = 0.0992 M A) The reaction will proceed to the right. B) The reaction will proceed to the left. C) The reaction is at equilibrium, and no change in concentrations will occur. D) The container volume needs to be specified before a prediction can be made. E) The temperature needs to be specified before a prediction can be made. If the equilibrium constant for this reaction is Kc = 248, predict, if possible, what will happen when the reactants and product are combined with the concentrations shown. [CO] = [Cl2] = 0.0200 M; [COCl2] = 0.0992 M


A) The reaction will proceed to the right.
B) The reaction will proceed to the left.
C) The reaction is at equilibrium, and no change in concentrations will occur.
D) The container volume needs to be specified before a prediction can be made.
E) The temperature needs to be specified before a prediction can be made.

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Methanol can be synthesized by combining carbon monoxide and hydrogen. Methanol can be synthesized by combining carbon monoxide and hydrogen. A reaction vessel contains these compounds at equilibrium. What effect will be seen when equilibrium is reestablished after decreasing the temperature by 45 \degree 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. A reaction vessel contains these compounds at equilibrium. What effect will be seen when equilibrium is reestablished after decreasing the temperature by 45 °\degree 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.

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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.

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Methanol can be synthesized by combining carbon monoxide and hydrogen. Methanol can be synthesized by combining carbon monoxide and hydrogen. A reaction vessel contains the three gases at equilibrium with a total pressure of 1.00 atm. What will happen to the partial pressure of hydrogen if enough argon is added to raise the total pressure to 1.4 atm? A) The partial pressure of hydrogen will decrease. B) The partial pressure of hydrogen will increase. C) The partial pressure of hydrogen will be unchanged. D) K<sub>p</sub> needs to be known before a prediction can be made. E) Both K<sub>p</sub> and the temperature need to be known before a prediction can be made. A reaction vessel contains the three gases at equilibrium with a total pressure of 1.00 atm. What will happen to the partial pressure of hydrogen if enough argon is added to raise the total pressure to 1.4 atm?


A) The partial pressure of hydrogen will decrease.
B) The partial pressure of hydrogen will increase.
C) The partial pressure of hydrogen will be unchanged.
D) Kp needs to be known before a prediction can be made.
E) Both Kp and the temperature need to be known before a prediction can be made.

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Consider the equilibrium reaction: Consider the equilibrium reaction: 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 *K<sub>c</sub>) ¯<sup>1</sup> D) K<sub>p</sub> = K<sub>c</sub> /RT E) K<sub>p</sub> = RT/K<sub>c</sub> 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 *Kc) ¯1
D) Kp = Kc /RT
E) Kp = RT/Kc

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When 0.152 mol of solid PH3BCl3 is introduced into a 3.0 L container at a certain temperature, 8.44 *10¯3 mol of PH3 is present at equilibrium: PH3BCl3(s) When 0.152 mol of solid PH<sub>3</sub>BCl<sub>3</sub> is introduced into a 3.0 L container at a certain temperature, 8.44 *10¯<sup>3</sup> mol of PH<sub>3</sub> is present at equilibrium: PH<sub>3</sub>BCl<sub>3</sub>(s) PH<sub>3</sub>(g) + BCl<sub>3</sub>(g) Construct a reaction table for the process, and use it to calculate K<sub>c</sub> at this temperature. PH3(g) + BCl3(g) Construct a reaction table for the process, and use it to calculate Kc at this temperature. When 0.152 mol of solid PH<sub>3</sub>BCl<sub>3</sub> is introduced into a 3.0 L container at a certain temperature, 8.44 *10¯<sup>3</sup> mol of PH<sub>3</sub> is present at equilibrium: PH<sub>3</sub>BCl<sub>3</sub>(s) PH<sub>3</sub>(g) + BCl<sub>3</sub>(g) Construct a reaction table for the process, and use it to calculate K<sub>c</sub> at this temperature.

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Kc = (0.144...

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In water, the following equilibrium exists: In water, the following equilibrium exists: In pure water at 25 \degree C, the concentration of H<sup>+</sup> ions is 1.00 * 10¯<sup>7</sup> mol/L. Calculate the value of the equilibrium constant for the reaction as written above. A) 1.00 *10<sup>14</sup> B) 1.00 * 10<sup>12</sup> C) 1.00 * 10¯<sup>14</sup> D) 1.00 * 10¯<sup>12</sup> E) 5.55 * 10<sup>15</sup> In pure water at 25 °\degree C, the concentration of H+ ions is 1.00 * 10¯7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.


A) 1.00 *1014
B) 1.00 * 1012
C) 1.00 * 10¯14
D) 1.00 * 10¯12
E) 5.55 * 1015

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A

Consider the reactions of cadmium with the thiosulfate anion. Consider the reactions of cadmium with the thiosulfate anion. What is the value for the equilibrium constant for the following reaction? A) 0.030 B) 33 C) 8.1* 103 D) 8.6 * 103 E) 2.1 *106 What is the value for the equilibrium constant for the following reaction? Consider the reactions of cadmium with the thiosulfate anion. What is the value for the equilibrium constant for the following reaction? A) 0.030 B) 33 C) 8.1* 103 D) 8.6 * 103 E) 2.1 *106


A) 0.030
B) 33
C) 8.1* 103
D) 8.6 * 103
E) 2.1 *106

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Given this equilibrium constant data at 25 °\degree C, Given this equilibrium constant data at 25 \degree C, what is the value of K<sub>c</sub> at this temperature for the reaction 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 these choices is correct. what is the value of Kc at this temperature for the reaction Given this equilibrium constant data at 25 \degree C, what is the value of K<sub>c</sub> at this temperature for the reaction 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 these choices is correct.


A) 2.4 * 10¯31
B) 9.6 *10¯31
C) 1.0 * 1030
D) 4.2 * 1030
E) None of these choices is correct.

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Write the mass-action expression, Qc, for the following chemical reaction. Write the mass-action expression, Q<sub>c</sub>, for the following chemical reaction. A) B) C) D) E)


A) Write the mass-action expression, Q<sub>c</sub>, for the following chemical reaction. A) B) C) D) E)
B) Write the mass-action expression, Q<sub>c</sub>, for the following chemical reaction. A) B) C) D) E)
C) Write the mass-action expression, Q<sub>c</sub>, for the following chemical reaction. A) B) C) D) E)
D) Write the mass-action expression, Q<sub>c</sub>, for the following chemical reaction. A) B) C) D) E)
E) Write the mass-action expression, Q<sub>c</sub>, for the following chemical reaction. A) B) C) D) E)

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The two equilibrium constants for the same reaction, Kc and Kp, will always equal one another when


A) all of the reactants and products are gases.
B) in the reaction equation, the number of moles of gaseous products equals the number of moles of gaseous reactants.
C) in the reaction equation, the number of moles of gaseous products is greater than the number of moles of gaseous reactants.
D) in the reaction equation, the number of moles of gaseous products is smaller than the number of moles of gaseous reactants.
E) in the reaction equation, the total number of moles of reactants equals that of the products.

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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.

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An equilibrium is established in which both the forward (fwd) and the reverse (rev) reactions are elementary. If the equilibrium constant Kc = 1.6 *10¯2 and the rate constant kfwd = 8.0 * 10¯7 s¯1 what is the value of krev?


A) 1.3 *10¯8s¯1
B) 7.8 *107s¯1
C) 2 * 104 s¯1
D) 5.0 *10¯5s¯1
E) None of these choices is correct.

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For a solution equilibrium, a change in concentration of a reactant or product does not change Kc.

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Increasing the initial amount of the limiting reactant in a reaction will increase the value of the equilibrium constant, Kc.

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There is a direct correlation between the speed of a reaction and its equilibrium constant.

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At a high temperature, the following reaction has an equilibrium constant of 1.0 *102. At a high temperature, the following reaction has an equilibrium constant of 1.0 *10<sup>2</sup>.

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If 1.00 mol of each of H2 and F2 are allowed to come to equilibrium in a 10.0 L vessel, calculate the equilibrium amounts of H2 and HF. 0.17 mol of H2 and 1.7 mol of HF

The equilibrium constant, Kc, for the decomposition of COBr2 The equilibrium constant, K<sub>c</sub>, for the decomposition of COBr<sub>2</sub><sub> </sub> A) 0.0361 B) 2.63 C) 5.62 D) 10.5 E) 27.7


A) 0.0361
B) 2.63
C) 5.62
D) 10.5
E) 27.7

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Although a system may be at equilibrium, the rate constants of the forward and reverse reactions will in general be different.

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True

Write the mass-action expression, Qc, for the following chemical reaction. Write the mass-action expression, Q<sub>c</sub>, for the following chemical reaction. A) B) C) D) E)


A) Write the mass-action expression, Q<sub>c</sub>, for the following chemical reaction. A) B) C) D) E)
B) Write the mass-action expression, Q<sub>c</sub>, for the following chemical reaction. A) B) C) D) E)
C) Write the mass-action expression, Q<sub>c</sub>, for the following chemical reaction. A) B) C) D) E)
D) Write the mass-action expression, Q<sub>c</sub>, for the following chemical reaction. A) B) C) D) E)
E) Write the mass-action expression, Q<sub>c</sub>, for the following chemical reaction. A) B) C) D) E)

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