Which of the following statements is incorrec | vedclass

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(D) Statement $A$ is correct because for elementary reactions,the order is equal to the molecularity.Statement $B$ is correct because the rate-determi

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The activation energy of a reaction decreases with an increase in temperature.

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(D) Statement $A$ is correct because for elementary reactions,the order is equal to the molecularity.Statement $B$ is correct because the rate-determining step is an elementary step,so its order equals its molecularity.Statement $C$ is correct because a catalyst provides an alternative pathway with lower activation energy but does not change the energy of reactants or products,hence $\Delta H$ remains unchanged.Statement $D$ is incorrect because the activation energy $(E_a)$ is a characteristic property of a reaction and is independent of temperature. It depends on the nature of the reactants and the catalyst used.

Which of the following statements is incorrect?

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From the given data for the reaction $H_2 + I_2 \rightarrow 2HI$,calculate the activation energy $(E_a)$:
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Explain the effect of an increase in temperature on the rate of reaction and the rate constant.

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