(A) Using the Arrhenius equation: $\ln \frac{k_2}{k_1} = \frac{E_a}{R} \left( \frac{1}{T_1} - \frac{1}{T_2} \right)$ Given: $\frac{k_2}{k_1} = 4$,$T_1

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(A) Using the Arrhenius equation: $\ln \frac{k_2}{k_1} = \frac{E_a}{R} \left( \frac{1}{T_1} - \frac{1}{T_2} \right)$ Given: $\frac{k_2}{k_1} = 4$,$T_1 = 300 \, K$,$T_2 = 310 \, K$,$R = 8.314 \, J \, mol^{-1} \, K^{-1}$,$\ln 2 = 0.693$. $\ln 4 = \frac{E_a}{8.314} \left( \frac{310 - 300}{310 \times 300} \right)$ $2 \ln 2 = \frac{E_a}{8.314} \left( \frac{10}{93000} \right)$ $2 \times 0.693 = \frac{E_a}{8.314} \times \frac{1}{9300}$ $E_a = 1.386 \times 8.314 \times 9300 \, J \, mol^{-1} \approx 107200 \, J \, mol^{-1} = 107.2 \, kJ \, mol^{-1}$.

Class 12 Chemistry Chemical Kinetics Collision theory, Energy of activation and Arrhenius equation

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The rate of a reaction quadruples when the temperature changes from $300 \, K$ to $310 \, K$. The activation energy of this reaction is ........... $kJ \, mol^{-1}$ (Assume activation energy and pre-exponential factor are independent of temperature; $\ln 2 = 0.693$; $R = 8.314 \, J \, mol^{-1} \, K^{-1}$)

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$107.2$
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$53.6$
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$26.8$
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$214.4$

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Class 12

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Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

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Which of the following statements is not true according to the collision theory of reaction rates?

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When a biochemical reaction is carried out in a laboratory without the presence of enzymes,the rate of reaction is $10^{-6}$ times slower. What will be the activation energy $(E_a)$ in the presence of enzymes?

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Rate constant of a reaction is given as $\log_{10} K = -\frac{2000}{T} + 6.0$. Activation energy is ....... $kcal$.

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The temperature dependence of the rate constant $(k)$ of a chemical reaction is expressed by the Arrhenius equation,$k = A \cdot e^{-E^/RT}$. The activation energy $(E^)$ of the reaction can be calculated by plotting:

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For reaction $A \to B$,rate constant $K_1 = A_1 e^{-E_{a_1}/RT}$ and for the reaction $X \to Y$,rate constant $K_2 = A_2 e^{-E_{a_2}/RT}$. If $A_1 = 10^8, A_2 = 10^{10}$ and $E_{a_1} = 600 \ cal \ mol^{-1}$,$E_{a_2} = 1800 \ cal \ mol^{-1}$,then the temperature at which $K_1 = K_2$ is (given: $R = 2 \ cal \ K^{-1} \ mol^{-1}$):

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Which of the following statements is not true according to the collision theory of reaction rates?

When a biochemical reaction is carried out in a laboratory without the presence of enzymes,the rate of reaction is $10^{-6}$ times slower. What will be the activation energy $(E_a)$ in the presence of enzymes?

Rate constant of a reaction is given as $\log_{10} K = -\frac{2000}{T} + 6.0$. Activation energy is ....... $kcal$.

The temperature dependence of the rate constant $(k)$ of a chemical reaction is expressed by the Arrhenius equation,$k = A \cdot e^{-E^*/RT}$. The activation energy $(E^*)$ of the reaction can be calculated by plotting:

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The temperature dependence of the rate constant $(k)$ of a chemical reaction is expressed by the Arrhenius equation,$k = A \cdot e^{-E^/RT}$. The activation energy $(E^)$ of the reaction can be calculated by plotting: