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5 Written questions

5 Matching questions

  1. #126 go to graph
  2. The rate constant for the second order reaction below is 2.79 L/mol •min at 48°C. If the initial concentration of NO2 is 1.05 M , what is the half-life?
    2NO2 → N2O4

    a. 20.5 s
    b. 10.3 s
    c. 0.341 min
    d. 176 s
    e. 14.9 s
  3. 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
  4. The rate constant for a first-order reaction is 1.4 × 10-2 s-1 at 716 K and 5.5 × 10-2 s-1 at 864 K. What is the activation energy?
    a. 27 kJ/mol
    b. 21 kJ/mol
    c. 47 kJ/mol
    d. 5700 kJ/mol
    e. 48 kJ/mol
  5. Calculate the activation energy of a reaction if the rate constant is 0.75 s−1 at 25°C and 11.5 s−1 at 75°C.
    a. 681 J/mol
    b. 20.4 kJ/mol
    c. 15.8 kJ/mol
    d. 47.1 kJ/mol
    e. 31.4 kJ/mol
  1. a e. 48 kJ/mol
  2. b go to graph
  3. c d. 47.1 kJ/mol
  4. d a. second
  5. e b. 10.3 s

5 Multiple choice questions

  1. d. 1 and 2
  2. a. decrease by 3/4
  3. a. 5.0 × 102 min
  4. graph
  5. d. 2.4 × 10−5 M

5 True/False questions

  1. Which of the following statements regarding the rate constant in the rate law expression is incorrect?
    a. Its value increases with temperature.
    b. Its value is independent of initial concentration at a given temperature.
    c. Its units depend on the overall order of reaction.
    d. Its value is experimentally determined.
    e. The larger its value, the slower the reaction rate.
    e. Reactions involving simultaneous trimolecular collisions are very common in gases.


  2. For a certain reaction, a plot of reactant concentration as a function of time gave a straight line. What is the order of this reaction?
    a. Zero order
    b. First order
    c. Second order
    d. Pseudo-first order
    e. Impossible to tell from the given information
    a. 280 s


  3. The gas phase reaction A + B + C → D has a reaction rate which is experimentally observed to follow the relationship rate = k[A]2[C]. The reaction is ____ order in A, ____ order in B, and ____ order in C.
    a. first; second; third
    b. first; second; zero
    c. second; zero; first
    d. second; first; zero
    e. second; zero; zero
    c. second; zero; first


  4. The rate constant for the first order reaction below is k = 3.3 × 10−2 min−1 at 57 K. What is the half-life for this reaction at 57 K?
    A → B + C

    a. 21 min
    b. 30 min
    c. 61 min
    d. 9.1 min
    e. 1200 min
    b. 54.5 s−1


  5. The half-life of the zero order reaction below is 0.56 minutes. If the initial concentration of A is 3.4 M, what is the rate constant?
    A → B

    a. 6.07 mol/L•min
    b. 1.24 mol/L•min
    c. 3.04 mol/L•min
    d. 0.619 mol/L•min
    e. 1.79 mol/L•min
    c. 3.04 mol/L•min


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