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?

Similar Questions

The relation between the rate constant and temperature according to the Arrhenius equation is:

For an endothermic reaction,the energy of activation is $E_a$ and the enthalpy of reaction is $\Delta H$ (both in $kJ/mol$). The minimum value of $E_a$ will be:

In a reaction,the rate constant $K_1$ is twice the rate constant $K_2$ of another reaction. Find the relationship between the activation energies $E_1$ and $E_2$ of the two reactions at the same temperature.

In a reaction,the rate of reaction doubles with a $10^\circ C$ rise in temperature. If the temperature is increased from $10^\circ C$ to $100^\circ C$,by how many times will the rate of reaction increase?

For the gaseous reactions,calculate the approximate value of temperature at which $k_1 = k_2$. $[ln\, 10 = 2.3]$.
$A \to B$ $k_1 = 10^{15} e^{-25000 / 8.314\, T}$
$C \to D$ $k_2 = 10^{14} e^{-15000 / 8.314\, T}$

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