Assertion : In rate law,unlike in the express | vedclass

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(A) The rate law is determined experimentally and depends on the slowest step (rate-determining step) of the reaction mechanism.In contrast,the equili

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

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(A) The rate law is determined experimentally and depends on the slowest step (rate-determining step) of the reaction mechanism.In contrast,the equilibrium constant expression is derived from the stoichiometry of the overall balanced chemical equation.Therefore,the exponents in the rate law do not necessarily correspond to the stoichiometric coefficients of the reactants in the overall balanced equation.Since the reaction rate is governed by the reaction mechanism,the Reason correctly explains the Assertion.

Assertion : In rate law,unlike in the expression for equilibrium constants,the exponents for concentrations do not necessarily match the stoichiometric coefficients.
Reason : It is the mechanism and not the balanced chemical equation for the overall change that governs the reaction rate.

Similar Questions

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The rate constant of the reaction,$2 H_2O_2 \rightarrow 2 H_2O + O_2$ is $3 \times 10^{-3} \ min^{-1}$. At what concentration of $H_2O_2$ will the rate of reaction be $2 \times 10^{-4} \ M \ s^{-1}$?

The rate of the reaction: $2N_2O_5 \rightarrow 4NO_2 + O_2$ can be written in three ways.
$-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$
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Which one of the following statements is wrong?

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Assertion : In rate law,unlike in the expression for equilibrium constants,the exponents for concentrations do not necessarily match the stoichiometric coefficients.Reason : It is the mechanism and not the balanced chemical equation for the overall change that governs the reaction rate.