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half-life of the reaction

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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.

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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.