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5 November, 08:36

The gas phase reaction between NO2 and F2 is first order in [NO2] and first order in [F2l. What would happen to the reaction rate if the concentrations of both reactants were halved with everything else held constant? a. It would decrease by a factor of 2. b. It would increase by a factor of 4. c. It would increase by a factor of 2. d. It would remain unchanged. e. It would decrease by a factor of 4.

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  1. 5 November, 09:13
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    e. It would decrease by a factor of 4.

    Explanation:

    first order in [NO2]

    first order in [F2]

    The rate is then given as;

    Rate = k [NO2][F2]

    where k = rate constant = And is constant for a reaction.

    Let's insert some dummy values (Any values work, just be consistent);

    [NO2] = 2

    [F2] = 2

    K = 3

    Rate = 3*2*2

    Rate = 12

    What would happen to the reaction rate if the concentrations of both reactants were halved with everything else held constant?

    [NO2] = 2 / 2 = 1

    [F2] = 2 / 2 = 1

    K = 3

    Rate = 3*1*1

    Rate = 3

    Comparing both rates (12 and 3); the correct option is;

    e. It would decrease by a factor of 4.
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