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5 Written questions

5 Matching questions

  1. The reaction of ICl with hydrogen : 2 ICl + H2 → I2 + 2 HCl
    is first order in ICl and second order in H2. In an experiment to determine the rate law, the rate constant was determined to be 2.24 M-2s-1. Using this value for the rate constant, the rate of the reaction when [ICl] = 0.314M and [H2] = 0.179M would be:
    a. 1.26 x 10-3 Ms-1
    b. 2.25 x 10-2 Ms-1
    c. 3.95 x 10-2 Ms-1
    d. 2.23 x 102 Ms-1
    e. 2.52 x 10-1 Ms-1
  2. Evaluate the specific rate constant at the temperature at which the data were collected. The rate-law expression is rate = k[NO]2[H2].
    H2(g) + NO(g) → N2O(g) + H2O(g)

    Experiment Initial [NO] (M) Initial [H2] (M) Initial Rate (M•s−1)
    1 0.30 0.35 2.835 × 10−3
    2 0.60 0.35 1.134 × 10−2
    3 0.60 0.70 2.268 × 10−2



    a. 9.4 × 10−3 M−2•s−1
    b. 2.7 × 10−2 M−2•s−1
    c. 1.6 × 10−4 M−2•s−1
    d. 8.1 × 10−3 M−2•s−1
    e. 9.0 × 10−2 M−2•s−1
  3. For a certain third-order reaction with the general form aA → products, the rate is 0.36 M·s−1 when the concentration of the reactant is 0.35 mol/L. What is the rate constant for this reaction?

    a. 0.042 M−2⋅s−1
    b. 8.4 M−2⋅s−1
    c. 0.36 M−2⋅s−1
    d. 0.34 M−2⋅s−1
    e. 24 M−2⋅s−1
  4. #128 graph
  5. Consider the following first order reaction.
    A2B → AB + A

    If it takes 87 seconds for the concentration of A2B to be reduced from 2.2 M to 0.12 M, what is the value of the specific rate constant?
    a. 0.0334 min−1
    b. 2.01 min−1
    c. 2.01 s−1
    d. 18.3 min−1
    e. 3.51 × 10−3 s−1
  1. a b. 8.4 M−2⋅s−1
  2. b b. 2.25 x 10-2 Ms-1
  3. c e. 9.0 × 10−2 M−2•s−1
  4. d b. 2.01 min−1
  5. e graph

5 Multiple choice questions

  1. a. 0.0016 mol/L
  2. c. Each enzyme catalyzes many different reactions in a living system.
  3. a. 280 s
  4. graph
  5. b. M−2•s−1

5 True/False questions

  1. Given the following data for the reaction below.
    NH4+ + NO2− → N2 + 2H2O

    Trial [NH4+] [NO2−] Rate
    1 0.010 M 0.030 M 0.020 M/s
    2 0.015 0.030 0.030
    3 0.010 0.015 0.005

    The rate law for the reaction is
    a. rate = k[NH4+][NO2−]
    b. rate = k[NH4+]2[NO2−]
    c. rate = k[NH4+][NO2−]2
    d. rate = k[NH4+]2[NO2−]2
    e. None of these
    c. first order in A and first order in C2

          

  2. In a reaction coordinate diagram, reacting molecules are most unstable ______.
    a. at their initial position c. right after they collide
    b. when they are about to collide d. at the transition state
    d. at the transition state

          

  3. What would be the activation energy of a reaction if its rate constant at 35°C was double the value of its rate constant at 25°C?
    a. 63.8 kJ/mol
    b. 75.1 kJ/mol
    c. 8.12 kJ/mol
    d. 52.9 kJ/mol
    e. 68.3 J/mol
    d. 52.9 kJ/mol

          

  4. Rate data have been determined at a particular temperature for the overall reaction
    2NO + 2H2 → N2 + 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

    The rate-law expression is ____.


    a. rate = k[NO]2[H2]2
    b. rate = k[NO][H2]2
    c. rate = k[NO]2[H2]
    d. rate = k[NO][H2]
    e. None of these is correct.
    c. A larger negative value of ΔG0 causes a faster reaction rate

          

  5. Cyclopropane rearranges to form propene in a reaction that is first order. If the rate constant is 2.74 × 10−3 s−1, how long would it take for 85.6% of the cyclopropane to rearrange if the initial concentration was 0.460 M?
    a. 51.0 s
    b. 62.0 s
    c. 707 s
    d. 2.74 × 10−3 s
    e. 3.83 × 10−4 s
    e. 8.5 min

          

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