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(A) According to the Arrhenius equation,$k = A e^{-E_a/RT}$,the activation energy $(E_a)$ is a characteristic property of a reaction and is generally

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Activation energy of reaction decreases on decreasing temperature

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(A) According to the Arrhenius equation,$k = A e^{-E_a/RT}$,the activation energy $(E_a)$ is a characteristic property of a reaction and is generally considered independent of temperature. Therefore,the statement that activation energy decreases on decreasing temperature is incorrect. $(b)$ The order of reaction can change with temperature if the mechanism of the reaction changes. $(c)$ If the first step is the rate-determining step (slowest step),the rate law of the overall reaction is determined by the rate law of that step. $(d)$ The rate of a photochemical reaction is directly proportional to the intensity of the incident light (photons).

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Similar Questions

When temperature is increased from $27\,{}^{\circ}C$ to $127\,{}^{\circ}C$,the rate of reaction becomes doubled. The activation energy $E_a$ will be ........ $kCal$.

For the equilibrium $A_{(g)} \rightleftharpoons B_{(g)}$,$\Delta H$ is $-40 \ kJ/mol$. If the ratio of the activation energies of the forward $(E_f)$ and reverse $(E_b)$ reactions is $\frac{2}{3}$,then:

The rate constant of a reaction increases by five times on increase in temperature from $27^{\circ} C$ to $52^{\circ} C$. The value of activation energy in $kJ \, mol^{-1}$ is $....$ . (Rounded-off to the nearest integer) $[R = 8.314 \, J \, K^{-1} \, mol^{-1}]$

The variation of the rate constant with temperature is given by the Arrhenius equation $k = A e^{-E_a / (RT)}$. If $T \to \infty$,the rate constant $k$ will be equal to:

The activation energy of a forward reaction is $50 \, kcal$. What will be the activation energy of its reverse reaction?

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