Assertion : The kinetics of the reaction -
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Rate expression $ \frac {dX}{dt}= k[A]^m[B]^n$ shows that the total order of reaction is $m + n + 0 = m + n$ As the rate of reaction is independent of

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If both Assertion and Reason are correct and the Reason is a correct explanation of the Assertion.

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Rate expression $ \frac {dX}{dt}= k[A]^m[B]^n$ shows that the total order of reaction is $m + n + 0 = m + n$ As the rate of reaction is independent of concentration of  $C$, i.e., the order with respect to $C$ is zero. This is the reason that $C$ does not figure in the rate expression.

Assertion : The kinetics of the reaction -

$mA + nB + pC \to m' X + n 'Y + p 'Z$

obey the rate expression as $\frac{{dX}}{{dt}} = k{[A]^m}{[B]^n}$.

Reason : The rate of the reaction does not depend upon the concentration of $C$.

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Assertion : The kinetics of the reaction - $mA + nB + pC \to m' X + n 'Y + p 'Z$ obey the rate expression as $\frac{{dX}}{{dt}} = k{[A]^m}{[B]^n}$. Reason : The rate of the reaction does not depend upon the concentration of $C$.