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Homework answers / question archive / Chapter 12: Reaction Rates and Chemical Equilibrium 1) The rate of a reaction can be increased by all of the following except:             A)      increasing the temperature

Chapter 12: Reaction Rates and Chemical Equilibrium 1) The rate of a reaction can be increased by all of the following except:             A)      increasing the temperature

Chemistry

Chapter 12: Reaction Rates and Chemical Equilibrium

1) The rate of a reaction can be increased by all of the following except:

            A)      increasing the temperature.

            B)      increasing the concentration of the reactants.

            C)      increasing the surface area of the reactants.

            D)      adding a catalyst.

            E)      increasing the volume of the reaction vessel.

        2.  Which of the following will not increase the rate of a reaction?

            A)      decreasing the temperature

            B)      decreasing the concentration of the reactants

            C)      decreasing the surface area of the reactants

            D)      removing a catalyst

            E)      all of these choices are correct

 

        3.  Factors that influence reaction rates include all of the following except the

            A)      magnitude of the equilibrium constant. D)      size of solid reactant particles.

            B)      reaction temperature.                             E)      concentration of reactants.

            C)      presence of a catalyst.                                    

 

        4.  According to collision theory, the increase in the rate constant with increasing temperature is due mostly to the fact that

            A)      the activation energy decreases with increasing temperature.

            B)      the fraction of the collisions having sufficient energy to react increases with increasing temperature.

            C)      the pressure of the reactants increases with increasing temperature.

            D)      the heat change for most reactions is negative.

            E)      the fraction of the collisions that have the proper orientation for reaction increases with increasing temperature.

 

        5.  Which of the images shows the molecules in a proper orientation for an effective collision for the reaction:

            2HI(g) ® H2(g) + I2(g)

           

            A)  I only    B)  II only    C)  III only    D)  I and II    E)  II and III

        6.  Which of the following changes will increase the average kinetic energy of the reactants?

            A)      increasing the surface area of the reactants

            B)      increasing the concentration of the reactants

            C)      adding a catalyst

            D)      increasing the temperature

            E)      none of these choices

 

        7.  Which of the following changes will increase the fraction of collisions that are effective collisions?

            A)      increasing the temperature

            B)      increasing the concentration of the reactants

            C)      decreasing the concentration of the reactants

            D)      increasing the surface area of the reactants

            E)      all of these choices are correct

 

        8.  The kinetics of a reaction is studied at 25°C and at 50°C.  Which of the following statements is correct?

            A)      The rate of the reaction at 50°C will be lower than the rate at 25°C, since the molecules will be moving too fast to collide effectively.

            B)      The rate of the reaction at 50°C will be twice that of the rate at 25°C, since the temperature has doubled.

            C)      The rate of the reaction at 50°C will be greater than the rate at 25°C, since the activation energy will be lower at the higher temperature.

            D)      The rate of the reaction at 50°C will be greater than the rate at 25°C, since a greater fraction of the molecules will possess sufficient energy to react at the higher temperature.

            E)      None of these statements is correct.

 

        9.  Which of the following statements regarding catalysts is incorrect?

            A)      A catalyst increases the rate of a reaction by giving the reaction an alternate pathway with a lower activation energy.

            B)      Catalysts need not be present in large amounts because they are regenerated during the reaction.

            C)      Enzymes act as catalysts in our bodies.

            D)      In a chemical reaction, the catalyst is shown on the reactant side of the equation.

            E)      The shape of an active site on an enzyme is unique, allowing it to react with only one substrate.

 

      10.  Which of the following statements regarding catalysts is incorrect?

            A)      A catalyst increases the rate of a reaction by giving the reaction an alternate pathway with lower activation energy.

            B)      A catalyst is formed temporarily in an early step of a reaction.

            C)      Most enzymes are large protein molecules.

            D)      In a chemical equation the catalyst is shown above the reaction arrow of the equation.

            E)      The shape of an active site on an enzyme is unique, allowing it to react with only one substrate.

      11.  Identify any intermediates in the following three-step reaction:

            H2C=CH2 + H3O+ ® H3C=CH2+ + H2O

            H3C=CH2+ + H2O ® CH3CH2OH2+

                CH3CH2OH2+ + H2O ® CH3CH2OH + H3O+

            A)      H3O+ is an intermediate.

            B)      H3C=CH2+ is an intermediate.

            C)      H3C=CH2+, CH3CH2OH2+, and H2O are intermediates.

            D)      CH3CH2OH2+ is an intermediate.

            E)      H2O is an intermediate.

 

      12.  A catalyst speeds up a chemical reaction by

            A)      providing an alternate reaction pathway.

            B)      increasing the activation energy.

            C)      shifting the equilibrium.

            D)      increasing the heat of the reaction.

            E)      decreasing the heat of the reaction.

 

      13.  In a chemical reaction at constant temperature, the addition of a catalyst

            A)      affects the equilibrium constant.

            B)      increases the fraction of molecules with high kinetic energy.

            C)      provides an alternate reaction pathway with a different activation energy.

            D)      decreases the energy released in the chemical reaction.

            E)      increases the concentration of the products at equilibrium.

 

      14.  Identify an intermediate in the following two-step reaction.

            Sn2+ + Fe3+ ® Sn3+ + Fe2+

                Sn3+ + Fe3+ ® Sn4+ + Fe2+

            A)  Sn2+    B)  Fe3+    C)  Sn3+    D)  Fe2+    E)  Sn4+

 

      15.  Identify the intermediate(s) in the following two-step reaction.

            O3(g)  O2(g) + O(g)

            O(g) + O3(g) ® 2O2(g)

            A)  O(g)    B)  O3(g)    C)  O2(g)    D)  O2(g) and O(g)    E)  O3(g) and O2(g)

      16.  Identify the intermediate in the following two-step reaction.

            Cr2+(aq) + Sn4+(aq)  Cr3+(aq) + Sn3+(aq

            Cr2+(aq) + Sn3+(aq) ® Cr3+(aq) + Sn2+(aq)

            A)  Sn3+(aq)    B)  Sn4+(aq)    C)  Sn2+(aq)    D)  Cr2+(aq)    E)  Cr3+(aq)

 

      17.  Identify the intermediate(s) in the following three-step reaction.

            Cl2(g)  2Cl(g

            CHCl3(g) + Cl(g) ® HCl(g) + CCl3(g)

            CCl3(g)  + Cl(g) ® CCl4(g)

            A)  CHCl3(g)    B)  HCl(g)    C)  Cl2(g)    D)  Cl(g)    E)  Cl(g) and CCl3(g)

 

      18.  Identify any intermediates or catalysts in the following two-step reaction:

            S2O82- + I- ® 2SO42- + I+

                I+ + I- ® I2

               

            A)      S2O82- is an intermediate.                      D)      I+ is an intermediate.

            B)      S2O82- is a catalyst.                               E)      SO42- is a catalyst.

            C)      I- is a catalyst.                                                

 

      19.  Identify any intermediates or catalysts in the following two-step reaction:

            H2O2 + 2Br- + 2H+® 2H2O + Br2

                H2O2 + Br2 ® 2H+ + O2 + 2Br-

            A)      H2O2 is an intermediate.

            B)      H2O2 is a catalyst, Br- is an intermediate.

            C)      Br- is a catalyst, Br2 is an intermediate.

            D)      H+ is a catalyst.

            E)      Br- and H+ are catalysts, Br2 is an intermediate.

 

      20.  Identify any intermediates or catalysts in the following two-step reaction:

            Cu2+ + H2 ® CuH+ + H+

                CuH+ + H+ + H2C=CH2 ® Cu2+ + H3C-CH3

            A)      CuH+ is an intermediate.

            B)      Cu2+ is a catalyst, H+ is an intermediate.

            C)      Cu2+ is a catalyst,  CuH+ is an intermediate.

            D)      Cu2+ is a catalyst,  CuH+ and H+ are intermediates.

            E)      CuH+ and H+ are catalysts, Cu2+ is an intermediate.

 

      21.  Identify the catalyst in the following three-step process for the decomposition of ozone.

            O3(g)  O2(g) + O(g)

            NO(g) + O3(g) ® NO2(g) + O2(g)

            O(g) + NO2(g) ® O2(g) + NO(g)

            A)  O(g)    B)  O3(g)    C)  O2(g)    D)  NO(g)    E)  NO2(g)

 

      22.  Identify the catalyst in the following three-step reaction.

            NO(g) + O2(g) ® NO3(g)

            NO3(g) + NO(g) ® 2NO2(g)

            NO2(g) + SO2(g) ® NO(g) + SO3(g)

            A)  SO2(g)    B)  NO3(g)    C)  O2(g)    D)  NO(g)    E)  NO2(g)

      23.  Activated complexes are:

            A)      stable molecules that are formed during an early step of a reaction, and consumed in a later step.

            B)      materials which act to increase the rate of a reaction without themselves being consumed.

            C)      substances which form during a reaction that have a definite, well-known structure.

            D)      short-lived, high-energy chemical species that are produced during a reaction.

            E)      a molecular species with normal chemical bonds that is produced during a reaction.

 

      24.  When a chemical system has reached equilibrium:

            A)      the forward and reverse reactions have stopped.

            B)      the rate of the forward reaction is greater than the rate of the reverse reaction.

            C)      the rate of the forward reaction is less than the rate of the reverse reaction.

            D)      the rate of the forward reaction is equal to the rate of the reverse reaction.

            E)      the equilibrium constant has reached a minimum.

 

      25.  In order to write the equilibrium constant expression for a reaction, you must:

            A)      know the mechanism for the reaction.

            B)      know the rate of the forward and reverse reactions.

            C)      know the concentrations of all reactants and products.

            D)      have the balanced chemical equation for the reaction.

            E)      know the conditions of pressure, temperature, and concentration for the system.

 

      26.  The graph shows the change in concentration of reactant and product as a reaction proceeds.  At what point is equilibrium first reached?

           

            A)  I    B)  II    C)  III    D)  IV    E)  V

 

      27.  If the following reaction is carried out in a sealed container:

            2SO3(g)  2SO2(g) + O2(g)

            a state of equilibrium can be reached if the container initially contains:

            A)      SO3 only.

            B)      SO2 and O2 only.

            C)      SO3 and O2 only.

            D)      SO3, SO2, and O2.

            E)      any of these combinations of reactants and products.

 

      28.  If the following reaction is carried out in a sealed container:

            N2(g) + 3H2(g  2NH3(g)

            a state of equilibrium can be reached if the container initially contains:

            A)      NH3 only.

            B)      N2 and H2 only.

            C)      NH3 and N2 only.

            D)      NH3, N2, and H2.

            E)      any of these combinations of reactants and product.

 

      29.  A chemical reaction can reach a state of equilibrium

            A)      only from the reactants side.

            B)      only from the products side.

            C)      only when both products and reactants are present initially.

            D)      by starting from either the reactant or the product side.

            E)      from all reactants and at least one product.

 

      30.  Consider the sublimation of solid iodine in a closed container:

            I2(s)  I2(g)

            What kind of measurements could you make to determine if this physical change has reached a state of equilibrium?

            A)      measure changes in the volume of the container

            B)      measure changes in the mass of the contents of the container

            C)      measure changes in pressure inside the container

            D)      measure changes in temperature inside the container

 

      31.  Consider the following equilibrium to form the brown gas NO2:

            N2O4(g 2NO2(g)

            colorless       brown

            What observation would indicate that the reaction is at equilibrium in a closed container?

            A)      There is no change in mass of the container and its contents.

            B)      The intensity of the color of the gas in the container does not change.

            C)      The volume of the container does not change.

            D)      The temperature in the container does not change.

 

      32.  Consider the sublimation of liquid bromine in a closed container:

            Br2(s)  Br2(g)

            What kind of measurements could you make to determine if this physical change has reached a state of equilibrium?

            A)      measure changes in the volume of the container

            B)      measure a change of mass in the container and its contents

            C)      measure changes in pressure inside the container

            D)      measure changes in the temperature inside the container

 

      33.  Select the correct equilibrium constant expression for the reaction:

            H2(g) + I2(g)  2HI(g)

            A)                                            D)     

            B)      Keq = [HI]2 [H2][I2]                                E)     

            C)      Keq = [HI]2 + [H2] + [I2]                                 

 

      34.  Select the correct equilibrium constant expression for the reaction:

            CH4(g) + 2H2S(g)  CS2(g) + 4H2(g)

            A)                                      D)      Keq = [CS2][H2]4 - [CH4][H2S]2

            B)                                      E)      Keq = [CS2][H2]4 + [CH4][H2S]2

            C)                                             

 

      35.  Select the correct equilibrium constant expression for the reaction

            4NH3(g) + 3O2(g)  2N2(g) + 6H2O(g)

            A)                                        D)      Keq = 6[H2O]2[N2] - 4[NH3]3[O2]

            B)                                        E)      Keq= [N2]2[H2O]6 + [NH3]4[O2]3

            C)                                              

 

      36.  For the reaction, CoO(s) + H2(g)  Co(s) + H2O(g), at 550°C, the value of K is 67.  The equilibrium constant expression is

            A)                                          D)     

            B)                                          E)     

            C)                                                   

 

      37.  What is the balanced chemical equation that corresponds to the equilibrium constant expression (assuming a homogeneous equilibrium in the gas state)?

           

            A)      A + B  C                                          D)      A + B  2C

            B)      2A + 2B  C                                      E)      2C  A + B

            C)      C  A + B                                                   

 

      38.  What is the balanced chemical equation that corresponds to the equilibrium constant expression (assuming a homogeneous equilibrium in the gas state)?

           

            A)      A2 + B  C                                         D)      C   A2 + B

            B)      2A + B  C                                        E)      C  2A + B

            C)      C   A + B                                                  

 

      39.  What is the balanced chemical equation that corresponds to the equilibrium constant expression (assuming a homogeneous equilibrium in the gas state)?

           

            A)      A + B2  C + D                                 D)      C + D  A + B2

            B)      A + 2B  C + D                                 E)      C + D   A + 2B

            C)      C + D  A + B                                           

 

      40.  The process, 2NH3(g) + heat  N2(g) + 3H2(g), is at equilibrium at a given temperature.  Which of the following changes will change the equilibrium constant for the process?

            A)      Adding more NH3 to the system, with the volume held constant.

            B)      Increasing the pressure by reducing the volume of the system.

            C)      Adding an effective catalyst for the process.

            D)      Raising the temperature of the system.

            E)      Adding some neon to the system.

 

      41.  For a given reaction, which of the following statements can be made about the value of the equilibrium constant?

            A)      It always remains the same.

            B)      It increases when the concentration of one of the products is increased.

            C)      It increases when the concentration of one of the reactants is increased.

            D)      It changes with changes in the temperature.

            E)      It can be changed by addition of a catalyst.

      42.  The value of the equilibrium constant at a given temperature for the reaction:

            2HI(g)  H2(g) + I2(g)

            is 0.200.  Find the value of the equilibrium constant for the reaction:

            H2(g) + I2(g)  2HI(g)

            A)  0.200    B)  0.0400    C)  5.00    D)  0.500    E)  -0.200

 

      43.  The value of the equilibrium constant at a given temperature for the reaction:

            CO(g) + H2O(g)  CO2(g) + H2(g)

            is 16.  Find the value of the equilibrium constant for the reaction:

            H2(g) + CO2(g)  CO(g) + H2O(g)

            A)  16    B)  4.0    C)  8.0    D)  0.062    E)  -16

 

      44.  The value of the equilibrium constant at a given temperature for the reaction:

            N2(g) + 3H2(g)  2NH3(g)

            is 224.  Find the value of the equilibrium constant for the reaction:

            2NH3(g)  N2(g) + 3H2(g)

            A)  224    B)  0.00446    C)  448    D)  5.02 ´ 104    E)  -224

 

      45.  If the value of the equilibrium constant at a given temperature for the reaction:

            2A  B

            is 5.0, what is the value of the equilibrium constant for the reaction:

            B   2A

            A)  5.0    B)  25    C)  0.20    D)  0.040    E)  -5.0

 

      46.  If the value of the equilibrium constant at a given temperature for the reaction:

            A  2B

            is 4.0, what is the value of the equilibrium constant for the reaction:

            2B A

            A)  4.0    B)  0.25    C)  16    D)  0.062    E)  -4.0

 

      47.  Which equilibrium constant represents a reaction that is product favored?

            A)      Keq = 0.025                                            D)      Keq = 6.3 ´ 105

            B)      Keq = 5.2                                                E)      not enough information

            C)      Keq = 8.4 ´ 10-5                                              

 

      48.  Which equilibrium constant represents a reaction that is reactant favored?

            A)      Keq = 0.025                                            D)      Keq = 6.3 ´ 105

            B)      Keq  = 5.2                                               E)      not enough information

            C)      Keq = 8.4 ´ 10-5                                              

 

      49.  Which of the following statements is correct for a reaction that has K << 1?

            A)      The forward reaction is faster than the reverse reaction.

            B)      The reverse reaction is faster than the forward reaction.

            C)      The equilibrium favors the products.

            D)      The equilibrium favors the reactants.

            E)      None of these statements is correct.

 

      50.  Which of the following statements is correct for a reaction that has K >> 1?

            A)      The forward reaction is faster than the reverse reaction.

            B)      The reverse reaction is faster than the forward reaction.

            C)      The equilibrium favors the products.

            D)      The equilibrium favors the reactants.

            E)      None of these statements is correct.

 

      51.  Consider the reaction and its equilibrium constant:

            S2Cl2(g) + Cl2(g)  2SCl2(gKeq = 4

           

            Examine the figure, and determine if the system is at equilibrium. If it is not, in which direction will it proceed to reach equilibrium?

            A)      The reaction is at equilibrium.

            B)      The reaction is not at equilibrium, it will shift to the left.

            C)      The reaction is not at equilibrium, it will shift to the right.

            D)      It is not possible to tell if the reaction is at equilibrium.

            E)      To reach equilibrium, the value of Keq must change.

 

      52.  Consider the reaction CO(g) + H2O(g)  CO2(g) + H2(g), represented by the following diagram:

           

            What is the composition of this system when the reaction reaches equilibrium?

            A)      3 CO, 3 H2O, 7 CO2, 7 H2                    D)      8 CO, 8 H2O, 2 CO2, 2 H2

            B)      1 CO, 1 H2O, 4 CO2, 4 H2                    E)      4 CO, 6 H2O, 4 CO2, 6 H2

            C)      2 CO, 2 H2O, 8 CO2, 8 H2                             

 

      53.  The reaction S2Cl2(g) + Cl2(g)  2SCl2(g) has an equilibrium constant of K = 8.  The image shows a partially reacted system.  What is the composition of this system when the reaction reaches equilibrium?

           

            A)      1 S2Cl2, 3 Cl2, 10 SCl2                           D)      4 S2Cl2, 6 Cl2, 4 SCl2

            B)      2 S2Cl2, 4 Cl2, 8 SCl2                             E)      5 S2Cl2, 7 Cl2, 2 SCl2

            C)      3 S2Cl2, 5 Cl2, 6 SCl2                                     

 

      54.  The value of the equilibrium constant at a given temperature for the reaction:

            2HI(g)  H2(g) + I2(g)

            is 0.200.  If [HI] = 0.200 M, [H2] = 0.200 M, and [I2] = 0.200 M, determine if the reaction is at equilibrium. If it is not, in which direction will it proceed to reach equilibrium?

            A)      The reaction is at equilibrium.

            B)      The reaction is not at equilibrium, it will shift to the left.

            C)      The reaction is not at equilibrium, it will shift to the right.

            D)      It is not possible to tell if the reaction is at equilibrium.

            E)      To reach equilibrium, the value of Keq must change.

 

      55.  The value of the equilibrium constant at a given temperature for the reaction:

            CO(g) + H2O(g)  CO2(g) + H2(g)

            is 16.  If [CO] = 4.0 M, [H2O] = 4.0 M, [CO2] = 4.0 M, and [H2] = 4.0 M, determine if the reaction is at equilibrium. If it is not, in which direction will it proceed to reach equilibrium?

            A)      The reaction is at equilibrium.

            B)      The reaction is not at equilibrium, it will shift to the left.

            C)      The reaction is not at equilibrium, it will shift to the right.

            D)      It is not possible to tell if the reaction is at equilibrium.

            E)      To reach equilibrium, the value of Keq must change.

 

      56.  The value of the equilibrium constant at a given temperature for the reaction:

            N2(g) + 3H2(g)  2NH3(g)

            is 224.  If [N2] = 10.0 M, [H2] = 10.0 M, and [NH3] = 10.0 M, determine if the reaction is at equilibrium.  If it is not, in which direction will it proceed to reach equilibrium?

            A)      The reaction is at equilibrium.

            B)      The reaction is not at equilibrium, it will shift to the left.

            C)      The reaction is not at equilibrium, it will shift to the right.

            D)      It is not possible to tell if the reaction is at equilibrium>

            E)      To reach equilibrium, the value of Keq must change.

 

      57.  Consider the following reaction at a specific temperature:

            2HI(g)  H2(g) + I2(g)

            If [HI] = 0.447 M, [H2] = 0.200 M, and [I2] = 0.200 M at equilibrium, calculate the value of the equilibrium constant under these conditions.

            A)  0.200    B)  0.0400    C)  0.0895    D)  0.407    E)  0.0447

 

      58.  Consider the following reaction at a specific temperature:

            CO2(g) + H2(g)  CO(g) + H2O(g)

            If [CO2] = 3.60 M, [H2] = 4.00 M, [CO] = 1.18 M, and [H2O] = 2.40 M at equilibrium, calculate the value of the equilibrium constant under these conditions.

            A)  0.471    B)  0.197    C)  5.08    D)  2.12    E)  0.444

 

      59.  Consider the following reaction at a specific temperature:

            2HI(g)  H2(g) + I2(g)

            If [HI] = 1.17 M, [H2] = 1.37 M, and [I2] = 0.100 M at equilibrium, calculate the value of the equilibrium constant under these conditions.

            A)  1.17    B)  1.26    C)  0.100    D)  10.0    E)  8.54

 

      60.  Consider the following reaction at a specific temperature:

            CO2(g) + H2(g)  CO(g) + H2O(g)

            If [CO2] = 1.80 M, [H2] = 2.00 M, [CO] = 0.590 M, and [H2O] = 1.20 M at equilibrium, calculate the value of the equilibrium constant under these conditions.

            A)  0.471    B)  0.197    C)  5.08    D)  2.12    E)  0.444

 

      61.  Write the equilibrium constant expression for the reaction:

            2HgO(s)  2Hg(l) + O2(g)

            A)                                         D)      Keq = [Hg]2[O2]

            B)                                         E)     

            C)      Keq = [O2]                                                       

 

      62.  Write the equilibrium constant expression for the reaction:

            PbCl2(s)  Pb2+(aq) + 2Cl-(aq)

            A)                                      D)     

            B)      Keq = [Pb2+][ Cl-]2                                  E)     

            C)                                              

      63.  Write the equilibrium constant expression for the reaction:

            Pb2+(aq) + 2Cl-(aq)  PbCl2(s)

            A)                                      D)     

            B)      Keq = [Pb2+][ Cl-]2                                  E)     

            C)                                               

 

      64.  Write the equilibrium constant expression for the reaction:

            CH3NH2(g) + H2O(l)  CH3NH3+(aq) + OH-(aq)

            A)      Keq = [CH3NH3+][OH-]                         D)     

            B)                             E)     

            C)                                     

 

      65.  Write the equilibrium constant expression for the reaction:

            CH3NH3+(aq) + OH-(aq)  CH3NH2(g) + H2O(l)

            A)      Keq = [CH3NH3+][OH-]                         D)     

            B)                             E)     

            C)                                     

 

      66.  Consider the following reaction and its equilibrium constant:

            FeO(s) + CO(g)  Fe(s) + CO2(gKeq = 0.67

            If the equilibrium concentration of CO is measured at 0.40 M, what is the equilibrium concentration of CO2?

            A)  0.40 M    B)  1.1 M    C)  0.67 M    D)  0.27 M    E)  1.7 M

 

      67.  Consider the following reaction and its equilibrium constant:

            FeO(s) + CO(g)  Fe(s) + CO2(gKeq = 0.67

            If the equilibrium concentration of CO is measured at 0.50 M, what is the equilibrium concentration of CO2?

            A)  0.50 M    B)  1.2 M    C)  0.34 M    D)  0.27 M    E)  1.3 M

 

      68.  Consider the following reaction and its equilibrium constant:

            FeO(s) + CO(g)  Fe(s) + CO2(gKeq = 0.67

            If the equilibrium concentration of CO is measured at 0.15 M, what is the equilibrium concentration of CO2?

            A)  0.10 M    B)  1.2 M    C)  0.15 M    D)  0.52 M    E)  0.22 M

 

      69.  Consider the following reaction and its equilibrium constant:

            H2O(g) + Cl2O(g)  2HOCl(gKeq = 0.090

            If the equilibrium concentration of HOCl is measured at 0.15 M, what are the equilibrium concentrations of H2O and Cl2O, assuming that they are equal?

            A)  0.15 M    B)  0.090 M    C)  0.50 M    D)  0.25 M    E)  0.60 M

 

      70.  Consider the following reaction and its equilibrium constant:

            H2O(g) + Cl2O(g)  2HOCl(gKeq = 0.090

            If the equilibrium concentration of HOCl is measured at 0.20 M, what are the equilibrium concentrations of H2O and Cl2O, assuming that they are equal?

            A)  0.67    B)  0.20    C)  0.87    D)  0.44    E)  0.49

 

      71.  Which one of the following changes has no effect on the position of the equilibrium?

            A)      concentration change                            D)      temperature change

            B)      volume change                                      E)      addition of a catalyst

            C)      pressure change                                              

 

      72.  The position of equilibrium would not be appreciably affected by changes in the volume of the container for

            A)      NiO(s) + CO(g)  Ni(s) + CO2(g)     D)      2CO(g) + O2(g)  2CO2(g)

            B)      BaCO3(s)  BaO(s) + CO2(g)            E)      PCl5(s)  PCl3(g) + Cl2(g)

            C)      2H2O(g)  2H2(g) + O2(g)                          

 

      73.  Consider the following system at equilibrium:

            CH4(g) + 2H2O(g CO2(g) + 4H2(g)

            What change will cause the equilibrium to shift to form more CO2?

            A)      increase [H2]

            B)      decrease [H2O]

            C)      decrease the volume of the reaction vessel

            D)      decrease [CH4]

            E)      decrease [H2]

 

      74.  Consider the following system at equilibrium:

            CH4(g) + 2H2O(g)  CO2(g) + 4H2(g)

            What change will cause the equilibrium to shift to form more H2?

            A)      increase [H2]

            B)      decrease [H2O]

            C)      decrease the volume of the reaction vessel

            D)      decrease [CH4]

            E)      decrease [CO2]

 

      75.  Consider the following system at equilibrium:

            CH4(g) + 2H2O(g CO2(g) + 4H2(g)

            What change will cause the equilibrium to shift to form more CH4?

            A)      decrease [H2]

            B)      increase [H2O]

            C)      decrease the volume of the reaction vessel

            D)      increase [CH4]

            E)      decrease [CO2]

 

      76.  Consider the following system at equilibrium:

            NO(g) + SO3(g)  NO2(g) + SO2(g)

            What change will cause the equilibrium to shift to form more SO2?

            A)      decrease [NO]

            B)      increase [NO2]

            C)      decrease the volume of the reaction vessel

            D)      decrease [NO2]

            E)      decrease [SO3]

 

      77.  Consider the following system at equilibrium:

            NO(g) + SO3(g NO2(g) + SO2(g)

            What change will cause the equilibrium to shift to form more NO?

            A)      increase [SO3]

            B)      decrease [SO2]

            C)      decrease the volume of the reaction vessel

            D)      decrease [NO2]

            E)      decrease [SO3]

 

      78.  Consider the following reaction:

            N2(g) + 3H2(g)  2NH3(g) + heat

            Which conditions would favor maximum conversion of the reactants to the products?

            A)      high temperature and high pressure

            B)      low pressure; temperature is not important

            C)      high temperature and low pressure

            D)      low temperature and high pressure

            E)      low temperature and low pressure

      79.  Consider the reaction

            3Fe(s) + 4H2O(g)  4H2(g) + Fe3O4(s)

            If the total pressure is increased by reducing the volume,

            A)      the equilibrium constant increases.        D)      more H2(g) is produced.

            B)      no change occurs.                                  E)      more H2O(g) is produced.

            C)      more Fe(s) is produced.                                 

 

      80.  For the reaction

            CO(g) + 3H2(g)  CH4(g) + H2O(g)          q = -206 kJ

            What conditions favor maximum conversion of reactants to products?

            A)      low pressure and low temperature

            B)      removal of H2(g) and low temperature

            C)      high pressure and high temperature

            D)      high pressure and low temperature

            E)      low pressure and high temperature

 

      81.  Consider the following reaction:

            N2O4(g)  2NO2(g)     q = +58.2 kJ

            What will cause an increase in the concentration of NO2 at equilibrium?

            A)      The NO2 concentration can never change because the reaction is at equilibrium.

            B)      an increase in temperature

            C)      an increase in pressure

            D)      a decrease in volume

            E)      adding a catalyst

 

      82.  Consider the following reaction:

            N2(g) + 3H2(g)  2NH3(g)     q = -92 kJ

            All of the following will lead to production of more NH3 except

            A)      removal of NH3(g).

            B)      a decrease in the volume of the container.

            C)      an increase in pressure by addition of N2(g).

            D)      an increase in pressure by addition of argon.

            E)      a decrease in temperature.

 

      83.  Ethane, C2H6, can be formed by reacting acetylene, C2H2, with hydrogen gas as follows:

            C2H2(g) + H2(g)  C2H6(g)   Exothermic

            What change will be observed if the temperature of the reaction mixture at equilibrium were increased?

            A)      The concentration of C2H6 will increase.

            B)      The concentration of both C2H2 and H2 will increase.

            C)      The concentration of both C2H2 and H2 will decrease.

            D)      The concentration of H2 only will decrease.

            E)      There will be no change in the equilibrium concentrations.

 

      84.  Consider the following reaction initially at equilibrium:

            NO(g) + Cl2(g)  NOCl2(g)   Endothermic

            What change will be observed if the temperature of the reaction mixture at equilibrium were decreased?

            A)      The concentration of NOCl2 will be unchanged.

            B)      The concentration of NOCl2 will decrease.

            C)      The concentration of NOCl2 will increase.

            D)      The concentrations of NO and Cl2 will be unchanged.

            E)      The concentration of NO and Cl2 will double.

 

      85.  The high-energy chemical species that is produced when an effective collision occurs is called a catalyst.

      86.  The amount of energy that reactant molecules must possess in order to react is the activation energy.

      87.  A reaction that has a high activation energy will have a high rate of reaction.

 

      88.  A catalyst increases the rate of a reaction by increasing the kinetic energy of the reactants.

 

      89.  A catalyst gives an alternate pathway for a reaction that has a lower activation energy.

 

      90.  The enzyme sucrase catalyzes the metabolism of sucrose.

 

      91.  Catalysts are not included in an overall chemical reaction because they are regenerated during the reaction.

 

      92.  An activated complex is a short-lived, high-energy species that is formed during the process of a chemical reaction.

 

      93.  An intermediate in a chemical reaction is a species that the reactant molecules interact with during an early step in a reaction that is regenerated during a later step in the reaction.

 

      94.  If the average energy of the products of a chemical reaction is greater than the average energy of the reactants, then the reaction is exothermic.

 

      95.  When we say that an equilibrium lies to the left, it means that the concentration of the reactants is less than that of the products.

 

      96.  When square brackets are placed around the formula for a substance, such as [NaOH], it indicates that we are working with the percent-by-mass concentration of the solution.

 

      97.  The only condition under which the equilibrium constant for a specific reaction will change is if the temperature changes.

 

      98.  The reaction CaCO3(s)  CaO(s) + CO2(g) is an example of a heterogeneous equilibrium.

 

      99.  If heat is added to the system of an endothermic reaction, the equilibrium will shift to make more reactants.

 

    100.  Using collision theory, explain why reaction rates generally increase when the temperature increases.

    101.  Using collision theory, explain why reaction rates generally increase when the concentration of one or more of the reactants increases.

 

    102.  Consider the reaction shown in the figure.  If the initial conditions are the same in both flasks, with the exception of the concentration of the acetic acid, explain why there is a difference in the size of the balloons after the reaction has progressed for 10 seconds.

           

 

    103.  What is the relationship between the following two equilibrium constant expressions?

           

 

    104.  Is the system shown in the figure at equilibrium?  If not, in which direction must the reaction proceed?

           

 

    105.  If the initial concentrations of reactants and products are substituted into the equilibrium constant expression, and the value obtained is less than the equilibrium constant, is the system in a state of equilibrium, and if not, in which direction will the reaction shift to reach equilibrium?  Explain your answer.

 

    106.  The value of the equilibrium constant at a given temperature for the reaction:

            N2(g) + 3H2(g)  2NH3(g)

            is 224.  If [N2] = 5.00 M, [H2] = 5.00 M, and [NH3] = 5.00 M, is the reaction at equilibrium, and if not, in which direction will it shift?

 

    107.  Why are the concentrations of pure liquids and solids not included in the equilibrium constant expression for a given reaction?

 

    108.  When yeast bread dough is placed in the freezer, it can be stored for a long period of time without the dough “rising.”  Explain why this is so.

 

    109.  If the equilibrium constant at 25°C is 45, and 6.7 ´ 103 at 80°C, is the reaction endothermic or exothermic?  Explain.

 

    110.  Consider the reaction and its equilibrium constant:

            Examine the molecular-level diagram and determine if the reaction is at equilibrium, and if not, in which direction it must proceed in order to reach equilibrium.

 

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