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Clicker Questions

Chapter 15

Barbara MoweryYork College

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At equilibrium, the rate of the forward reaction is _______ the rate of the reverse reaction.

a. equal tob. slower thanc. faster thand. the reverse of

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At equilibrium, the rate of the forward reaction is _______ the rate of the reverse reaction.

a. equal tob. slower thanc. faster thand. the reverse of

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The reaction quotient Q is usually represented by

a. [reactants] / [products].b. [products] / [reactants].c. [reactants] [products].d. [reactants] + [products].

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The reaction quotient Q is usually represented by

a. [reactants] / [products].b. [products] / [reactants].c. [reactants] [products].d. [reactants] + [products].

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Select the statement that best describes a system at equilibrium.a. The reaction is complete because all

reactants have become products.b. The reaction has stopped because all of the

catalyst has been used.c. As soon as product molecules form, other

molecules of product become reactants.d. The reaction stops when the amounts of

reactants and products reach equilibrium amounts.

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Select the statement that best describes a system at equilibrium.a. The reaction is complete because all

reactants have become products.b. The reaction has stopped because all of the

catalyst has been used.c. As soon as product molecules form, other

molecules of product become reactants.d. The reaction stops when the amounts of

reactants and products reach equilibrium amounts.

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Which reaction quotient represents the reaction shown?Co(s) + 2 H+(aq) Co2+(aq) + H2(g)

a. b.

c. d.

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Which reaction quotient represents the reaction shown?Co(s) + 2 H+(aq) Co2+(aq) + H2(g)

a. b.

c. d.

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If the value of the equilibrium constant is large, then at equilibrium mostly _______ will be present.

a. reactantsb. productsc. catalystsd. water

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If the value of the equilibrium constant is large, then at equilibrium mostly _______ will be present.

a. reactantsb. productsc. catalystsd. water

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If the value of the equilibrium constant is small, then at equilibrium mostly _______ will be present.

a. reactantsb. productsc. catalystsd. water

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If the value of the equilibrium constant is small, then at equilibrium mostly _______ will be present.

a. reactantsb. productsc. catalystsd. water

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Q = the reaction quotientK = the equilibrium constantAt equilibrium, which is true?

a. Q > Kb. Q < Kc. Q = Kd. Q2 = K

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Q = the reaction quotientK = the equilibrium constantAt equilibrium, which is true?

a. Q > Kb. Q < Kc. Q = Kd. Q2 = K

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K = 2.39 for the gaseous reaction SO2Cl2 SO2 + Cl2. For a mixture where Q = 5.21 to reach equilibrium, the concentration of SO2Cl2 must _____.

a. increase b. decreasec. remain the samed. change in a way that cannot be predicted

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K = 2.39 for the gaseous reaction SO2Cl2 SO2 + Cl2. For a mixture where Q = 5.21 to reach equilibrium, the concentration of SO2Cl2 must _____.

a. increase b. decreasec. remain the samed. change in a way that cannot be predicted

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Equilibrium constants typically have units of

a. M.b. M2.c. M1−.d. None of the above

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Equilibrium constants typically have units of

a. M.b. M2.c. M1−.d. None of the above

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Reaction quotients for heterogeneous equilibria do not include concentrations of

a. pure liquids.b. pure solids.c. Both of the aboved. Neither of the above

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Reaction quotients for heterogeneous equilibria do not include concentrations of

a. pure liquids.b. pure solids.c. Both of the aboved. Neither of the above

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HA H+ + A− [HA] = 1.65 10–2 M and [H+] = [A–] = 5.44 10–4 M at equilibrium. Kc = _______.

a. 1.79 10−2

b. 1.79 10−3

c. 1.79 10−4

d. 1.79 10−5

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HA H+ + A− [HA] = 1.65 10–2 M and [H+] = [A–] = 5.44 10–4 M at equilibrium. Kc = _______.

a. 1.79 10−2

b. 1.79 10−3

c. 1.79 10−4

d. 1.79 10−5

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KP = KC when

a. the reaction is at equilibrium.b. the reaction is exothermic.c. all of the gases present are at

the same pressure.d. the number of moles of gas

on both sides of the balanced equation is the same.

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KP = KC when

a. the reaction is at equilibrium.b. the reaction is exothermic.c. all of the gases present are at

the same pressure.d. the number of moles of gas

on both sides of the balanced equation is the same.

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CO2 + H2 CO + H2OIf all species are gases and H2 is added, the concentration of CO at equilibrium will

a. increase.b. decrease.c. remain unchanged.d. disappear.

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CO2 + H2 CO + H2OIf all species are gases and H2 is added, the concentration of CO at equilibrium will

a. increase.b. decrease.c. remain unchanged.d. disappear.

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CO2 + H2 CO + H2OIf all species are gases and H2O is added, the equilibrium concentration of CO

a. will increase.b. will decrease.c. will remain unchanged.d. will disappear.

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CO2 + H2 CO + H2OIf all species are gases and H2O is added, the equilibrium concentration of CO

a. will increase.b. will decrease.c. will remain unchanged.d. will disappear.

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CO2 + H2 CO + H2OIf all species are gases and CO2 is removed, the [CO] at equilibrium will

a. increase.b. decrease.c. remain unchanged.d. disappear.

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CO2 + H2 CO + H2OIf all species are gases and CO2 is removed, the [CO] at equilibrium will

a. increase.b. decrease.c. remain unchanged.d. disappear.

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CO2 + H2 CO + H2OIncreasing the temperature of this endothermic reaction will _______ [CO] at equilibrium.

a. increaseb. decreasec. not changed. eradicate

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CO2 + H2 CO + H2OIncreasing the temperature of this endothermic reaction will _______ [CO] at equilibrium.

a. increaseb. decreasec. not changed. eradicate

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CO2 + H2 CO + H2OIncreasing the temperature of this endothermic reaction will _______ the value of K.

a. decreaseb. increasec. not changed. change unpredictably

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CO2 + H2 CO + H2OIncreasing the temperature of this endothermic reaction will _______ the value of K.

a. decreaseb. increasec. not changed. change unpredictably

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CO2 + H2 CO + H2OIf all species are gases and the container is compressed, the amount of CO will

a. increase.b. decrease.c. remain unchanged.d. vanish.

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CO2 + H2 CO + H2OIf all species are gases and the container is compressed, the amount of CO will

a. increase.b. decrease.c. remain unchanged.d. vanish.

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CO2 + H2 CO + H2OAdding a catalyst to this reaction will cause the [CO] at equilibrium to

a. increase.b. decrease.c. remain unchanged.d. cease to exist.

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CO2 + H2 CO + H2OAdding a catalyst to this reaction will cause the [CO] at equilibrium to

a. increase.b. decrease.c. remain unchanged.d. cease to exist.

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Ni(CO)4(g) Ni(s) + 4 CO(g)Adding nickel to this reaction will cause the equilibrium to

a. shift toward products.b. shift toward reactants.c. remain unchanged.d. change based on the amount

added.

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Ni(CO)4(g) Ni(s) + 4 CO(g)Adding nickel to this reaction will cause the equilibrium to

a. shift toward products.b. shift toward reactants.c. remain unchanged.d. change based on the amount

added.