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Decomposition of N2O5 follows first order kinetics and its instantaneous rate is 1.6 x 10^-6 mol/L/s. Calculate the rate constant of the reaction of 0.02M solution.

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Answer:

8×10^-5 s^-1

Explanation:

The decomposition of N2O5 is shown by the reaction equation;

N2O5(aq)⇄NO2(g) + NO3(g)

We have the following information;

Instantaneous rate of reaction = 1.6 x 10^-6 mol/L/s.

Concentration of the N2O5 = 0.02M

Now the rate of decomposition of N2O5 is given by;

R= k[N2O5] (first order reaction)

Hence;

1.6 x 10^-6 mol/L/s = k[0.02M]

k= 1.6 x 10^-6 mol/L/s / 0.02M

k= 8×10^-5 s^-1

Hence the rate of decomposition of N2O5 is 8×10^-5 s^-1

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