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half-life of the reaction

At 300 K the reaction below obeys the rate law Rate=k[NOCl]^2, where k=2.8 X .000010 M to the neg 1 times s to the neg 1.

2 NOCl >>>>>> 2NO + Cl2

Suppose 1.0 mole of NOCl is introduced into a 2.0-liter container at 300 K. Evaluate the half-life of the reaction.

Solution Preview

From the rat law, you should recognize that the reaction is of second order. We need to use the 2nd order integrated rate equation....

kt = 1/[A]t - ...

Solution Summary

It finds the half-life of the reaction given the rate law of the reaction.