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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The rate of a reaction $A$ doubles on increasing the temperature from $300 \, K$ to $310 \, K$. By how much should the temperature of reaction $B$ be increased from $300 \, K$ so that its rate doubles,if the activation energy of reaction $B$ is twice that of reaction $A$ (in $, K$)?

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The rate constant is given by the equation $k = p Z e^{-E_a/RT}$. Which factor should register a decrease for the reaction to proceed more rapidly?

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