The half life period for catalytic decomposition of X Y 3 at 100 mm is found to be 8 hrs and at 200 mm it is 4 hrs. The order of reaction is

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The value of order of reaction using half life and pressure values can be find out by using this relation given below
$\frac{{(t \frac{1}{2})}_{1}}{{(t \frac{1}{2})}_{2}} = {(\frac{P_{2}}{P_{1}})}^{n - 1}$
or $\frac{8}{4} = {(\frac{200}{100})}^{n - 1}$
$(2)^{1} = (2)^{n - 1}$
or $1 = n - 1$
So, $n = 2$ .
Hence, it is second order reaction.

Chemistry - Chemical Kinetics Question with Solution | TestHub

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