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Kinetics

Quiz by Natalie Wieland

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13 questions
Show answers
  • Q1
    The rate law of a reaction is determined to be rate = k[A][B]2. Which statement would most likely describe the reaction?
    The stoichiometry of the overall reaction must be A+2B--> products
    The reaction involves a one-step, termolecular mechanism
    The reaction involves the formation of intermediates
    The reaction is catalyzed by an enzyme
    60s
  • Q2
    In the reaction NO3(g) + CO(g) <=> NOw(g) + CO2(g), the carbon in CO must collide with an oxygen in NO3 with sufficient energy to react. Which of the diagrams below would most likely result in the formation of products?
    60 C and right orientation
    80 C and wrong orienation
    100 C somewhat right orientation
    -40 C and right orientation
    60s
  • Q3
    The graph above shows the number of molecules that have sufficient energy to overcome Ea for a given reaction. How would adding an enzyme change the appearance of the graph?
    Question Image
    no change in the graph
    lowers the height of the graph
    same shape but the activation energy has been lowered
    shifts the graph further to the right
    60s
  • Q4
    The values for the change in enthalpy, dH, and the activation energy, Ea, for a given reaction are known. The value of Ea for the reverse reaction equals
    the sum of dH and Ea
    the sum of -dH and Ea
    -(Ea) for the forward reaction
    Ea for the forward reaction
    60s
  • Q5
    For two first-order reactions of different substances A and X, A-->B t1/2 = 30.0 min, X-->Y t1/2 = 60.0 min. This means that
    the rate constant for A-->B is lower than the rate constant of X-->Y
    3 moles of A will react more rapidly than 3 moles of X
    a certain number of grams of A will react twice as fast as the same number of grams of X
    a certain number of grams of X will react twice as fast as the same number of grams of A
    60s
  • Q6
    A reaction is first order with respect to [X] and second order with respect to [Y]. When [X] is 0.20M and [Y]=0.20M the rate is 8.00x10-3Mmin-1. The value of the rate constant, including correct units, is
    2.0 M-2min-1
    1.00 Mmin-1
    2.00 M-1min-1
    1.00 M-2min-1
    60s
  • Q7
    The activation energy for this reaction, X+2Y-->3Z, shown in the potential energy diagram, could be
    Question Image
    increased by increasing [X] and [Y]
    decreased by adding a suitable catalyst
    decreased by removing Z from the system as it forms
    increased by increasing the temperature
    60s
  • Q8
    For all zero-order reactions
    the rate is independent of time
    Ea is very low
    a plot of time vs. concentration squared is linear
    the concentration of reactants is constant
    60s
  • Q9
    Use the following information. Carbon monoxide reacts with oxygen according to the equation CO(g) + 1/2O2(g) --> CO2(g). The rate law for the reaction is: Rate = k[CO]m[O2]n. Experimental information for the reaction is given in the following table. Which values correspond to the reaction orders m and n for CO and O2?
    Question Image
    m = 2, n = 1
    m = 1, n = 1/2
    m = 1, n = 1
    m = 4, n = 2
    60s
  • Q10
    What is the overall reaction order?
    Question Image
    2
    1
    0
    3
    60s
  • Q11
    What is the numerical value of the rate constant, k, for this reaction?
    Question Image
    1.54x10 4 min-1
    3.68x10-5 molL-1min-1
    2.93x10-25 molmin-1
    4.60 L2mol-2min-1
    60s
  • Q12
    Which of the following statements would be correct regarding the following reaction? 2H2(g) + Ox(g) --> 2H2O(g)
    The rate of H2O disappearance is equal to the rate of O2 disappearance
    The rate of H2 disappearance is twice the rate of O2 disappearance
    The rate of H2O disappearance is twice the rate of O2 disappearance
    The rate of O2 disappearance is twice the rate of H2 disappearance
    60s
  • Q13
    According to the collision theory of kinetics, which statement best describes the rate of a chemical reaction?
    The greater the difference in energy between the reactants and the products, the faster is the raction
    All collisions result in a chemical reaction
    All collisions between molecules with at least a minimum kinetic energy and the proper orientation result in reaction
    All collisions between molecules with at least a minimum kinetic energy result in reaction
    60s

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