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5 Written Questions

5 Matching Questions

  1. If the half-life of a reaction is independent of concentration, the reaction is:
    a. Zero order
    b. First order
    c. Second order
    d. Zero and first order
    e. First and second order
  2. The following data were collected for the following reaction at a particular temperature. What is the rate-law expression for this reaction? rate = ____.
    NH3 + O2 → N2O + H2O

    Experiment Initial [NH3] Initial [O2] Initial Rate
    1 1.10 M 1.10 M 5.5 × 10−3 M/s
    2 2.20 M 2.20 M 4.4 × 10−2 M/s
    3 1.10 M 2.20 M 2.2 × 10−2 M/s

    a. k[NH3]
    b. k[NH3]2
    c. k[NH3][O2]
    d. k[O2]
    e. k[NH3][O2]2
  3. A catalyst ____.
    a. is used up in a chemical reaction
    b. changes the value of ΔG0 of the reaction
    c. is always a solid
    d. does not influence the reaction in any way
    e. changes the activation energy of the reaction
  4. Determine the rate-law expression for the reaction below at the temperature at which the tabulated initial rate data were obtained. rate = ____
    A + 2B + 3C → Products

    Experiment Initial [A] Initial [B] Initial [C] Initial Rate of Loss of A
    1 0.10 M 0.20 M 0.10 M 4.0 × 10−2 M•min−1
    2 0.40 M 0.20 M 0.10 M 4.0 × 10−2 M•min−1
    3 0.20 M 0.20 M 0.25 M 1.0 × 10−1 M•min−1
    4 0.20 M 0.40 M 0.10 M 1.6 × 10−1 M•min−1

    a. k[A][B]
    b. k[A]2[C]
    c. k[C]2
    d. k[B]2[C]
    e. none of these
  5. Calculate the activation energy of a reaction if its rate constant is 2.8 × 106 s−1 at 24°C and 1.5 × 107 s−1 at 48°C.
    a. 26 kJ/mol
    b. 80. kJ/mol
    c. 55 kJ/mol
    d. 67 J/mol
    e. 3.51 J/mol
  1. a e. changes the activation energy of the reaction
  2. b a. Zero order
  3. c e. k[NH3][O2]2
  4. d d. k[B]2[C]
  5. e c. 55 kJ/mol

5 Multiple Choice Questions

  1. graph
  2. a. k[AB][C2]
  3. a. 5.0 × 102 min
  4. b. 2.01 min−1
  5. b. difficult to verify experimentally.

5 True/False Questions

  1. A reaction A + 2B → C is found to be first order in A and first order in B. What are the units of the rate constant, k, if the rate is expressed in units of moles per liter per minute?
    a. M−1•min−1
    b. M
    c. M•min−1
    d. min−1
    e. M2•min−1
    a. M−1•min−1

          

  2. For a certain reaction of the general form aA → products, a plot of the experimental data as 1/[A] versus time is linear. What is the reaction order with respect to reactant A?
    a. second
    b. zero
    c. first
    d. fourth
    e. third
    a. zero order graph

          

  3. A plot of ln [C] versus time is linear for the reaction C → D. What is the kinetic order of the reaction?
    a. second
    b. first
    c. zero
    d. one-half
    e. negative one
    b. first

          

  4. Rate data have been determined at a particular temperature for the overall reaction
    2NO + 2H2 → Ν2 + 2H2O
    in which all reactants and products are gases.

    Trial Run Initial [NO] Initial [H2] Initial Rate (M•s−1)
    1 0.10 M 0.20 M 0.0150
    2 0.10 M 0.30 M 0.0225
    3 0.20 M 0.20 M 0.0600

    What would be the initial rate of the reaction if the initial molar concentration of NO = 0.30 M and the initial molar concentration of H2 = 0.10 M?
    a. 0.068 M•s−1
    b. 0.22 M•s−1
    c. 0.022 M•s−1
    d. 0.040 M•s−1
    e. 0.10 M•s−1
    a. 0.068 M•s−1

          

  5. The rate constant for a reaction at 40.0°C is exactly 4 times that at 20.0°C. Calculate the Arrhenius energy of activation for the reaction.
    a. 4.00 kJ/mol
    b. 6.36 kJ/mol
    c. 52.8 kJ/mol
    d. 11.5 kJ/mol
    e. none of these
    b. 300°K

          

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