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Assertion : The kinetics of the reaction
\(m A+n B+p C \rightarrow m^{\prime} X+n^{\prime} Y+p^{\prime} Z\)
obeys the rate expression as -
\(\frac{d x}{d t}=k[A]^m[B]^n\)
Reason : The rate of reaction does not depend upon the concentration of \(C\).
Options:
\(m A+n B+p C \rightarrow m^{\prime} X+n^{\prime} Y+p^{\prime} Z\)
obeys the rate expression as -
\(\frac{d x}{d t}=k[A]^m[B]^n\)
Reason : The rate of reaction does not depend upon the concentration of \(C\).
Solution:
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Verified Answer
The correct answer is:
If both assertion and reason are true and reason is the correct explanation of assertion.
Rate expression \(\frac{d x}{d t}=k[A]^m[B]^n\) shows that the total order of reactions 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.
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