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5 Written questions

5 Matching questions

  1. Which of the following statements about reaction orders in the rate law expression is incorrect?
    a. Their values may equal the stoichiometric coefficients in the balanced equation.
    b. Their values may or may not equal the stoichiometric coefficients in the balanced equation.
    c. Their values must be experimentally determined.
    d. Their values get larger as the temperature is increased.
    e. An order equal to zero means there is no concentration dependence with rate.
  2. Consider the reaction below and its observed rate law expression. Which proposed mechanisms are consistent with the rate law expression?
    2NO2 → 2NO + O2 rate = k[NO2]2

    I. NO2 + NO2 → N2O4 slow
    N2O4 → N2 + 2O2 fast
    N2 + O2 → 2NO fast
    2NO2 → 2NO + O2 overall

    II. NO2 → N + O2 slow
    NO2 + N → N2O2 fast
    N2O2 → 2NO fast
    2NO2 → 2NO + O2 overall

    III. NO2 → NO + O slow
    O + NO2 → NO + O2 fast
    2NO2 → 2NO + O2 overall

    a. I
    b. II
    c. III
    d. I and III
    e. another combination
  3. For which of the following hypothetical rate laws would the units of the rate constant have the general form M⋅time−1?
    a. rate = k
    b. rate = k[A]
    c. rate = k[A]3
    d. rate = k[A]2
    e. rate = k[A]4
  4. The gas phase reaction A + B → C has a reaction rate which is experimentally observed to follow the relationship rate = k[A][B]2. The overall order of the reaction
    a. is first.
    b. is second.
    c. is third.
    d. is zero.
    e. cannot be determined.
  5. Consider the hypothetical reaction shown below.
    2A + C2 → A2C + C

    Assume that the following proposed mechanism is consistent with the rate data.

    A + C2 → AC + C slow
    AC + A → A2C fast
    2A + C2 → A2C + C overall


    Which one of the following statements must be true? The reaction is ____.
    a. first order in A, first order in B, and third order overall
    b. second order in C2 and second order overall
    c. first order in A and first order in C2
    d. second order in C2, zero order in A, and third order overall
    e. second order in A and second order overall
  1. a c. first order in A and first order in C2
  2. b a. I
  3. c c. is third.
  4. d d. Their values get larger as the temperature is increased.
  5. e a. rate = k

5 Multiple choice questions

  1. d. both (a) and (b) are correct
  2. b. 54.5 s−1
  3. c. 2.75 hrs
  4. b. All reactant collisions result in product formation.
  5. d. 1 and 2

5 True/False questions

  1. For the gas phase decomposition of ethyl chloroformate, ClCOOC2H5 → C2H5Cl + CO2
    The rate constant has been determined at several different temperatures. When the data is graphed as ln k vs. 1/T, the slope of the line is -1.48 x 104 and the y-intercept is 24.6.
    What is the activation energy, Ea, for this reaction?
    a. 9.62 kJ b. 15.0 kJ c. 123 kJ d. 205 kJ e. 1214 kJ
    d. both (a) and (b) are correct

          

  2. A troublesome reaction that is responsible in part for acid rain is
    SO3 + H2O → H2SO4

    Rate data have been determined at a particular temperature for the reaction in which all reactants and products are gases.

    Trial Run Initial [SO3] Initial [H2O] Initial Rate (M•s−1)
    1 0.35 M 0.35 M 0.150
    2 0.70 M 0.35 M 0.600
    3 0.35 M 0.70 M 0.300
    4 0.70 M 0.70 M 1.20

    The rate-law expression is ____.
    a. rate = k[SO3]2[H2O]2
    b. rate = k[SO3]2[H2O]
    c. rate = k[SO3][H2O]2
    d. rate = k[SO3]2
    e. rate = k[SO3][H2O]
    d. k[H2][CO]

          

  3. 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

          

  4. 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
    c. 4.0 × 10−1 M−2•min−1

          

  5. 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

          

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