The decomposition reaction 2 NOCl → 2 NO + Cl_2 has a rate law that is second order with respect to [NOCl], where k = 3.2 M^{-1}s^{-1} at a certain temperature. If the initial concentration of NOCl is 0.076 M, how many seconds will it take for [NOCl] to decrease to 0.042 M at this temperature? Do not enter units with your numerical answer.

It will take 3.3 s for [NOCl] to decrease to 0.042 M.

Explanation:

Integrated rate law for this second order reaction-

where, [NOCl] is concentration of NOCl after "t" time, is initial concentration of NOCl and k is rate constant.

Here, = 0.076 M, k = 3.2 and [NOCl] = 0.042 M

So,

or, t = 3.3 s

So, it will take 3.3 s for [NOCl] to decrease to 0.042 M.

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