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(D) The Arrhenius equation is given by: $\log \left(\frac{k_2}{k_1}\right) = \frac{E_a}{2.303 R} \left(\frac{1}{T_1} - \frac{1}{T_2}\right)$Given: $k_

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$38.04 \ kJ \ mol^{-1}$

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(D) The Arrhenius equation is given by: $\log \left(\frac{k_2}{k_1}ight) = \frac{E_a}{2.303 R} \left(\frac{1}{T_1} - \frac{1}{T_2}ight)$Given: $k_2 = 4k_1$,$T_1 = 27 + 273 = 300 \ K$,$T_2 = 57 + 273 = 330 \ K$,$R = 8.314 \ J \ K^{-1} \ mol^{-1}$,$\log 4 = 0.6021$Substituting the values:$\log 4 = \frac{E_a}{2.303 	imes 8.314} \left(\frac{1}{300} - \frac{1}{330}ight)$$0.6021 = \frac{E_a}{19.147} \left(\frac{330 - 300}{300 	imes 330}ight)$$0.6021 = \frac{E_a}{19.147} \left(\frac{30}{99000}ight)$$E_a = \frac{0.6021 	imes 19.147 	imes 99000}{30} \approx 38040 \ J \ mol^{-1}$$E_a = 38.04 \ kJ \ mol^{-1}$

The rate of a reaction quadruples when temperature changes from $27^{\circ} C$ to $57^{\circ} C$. Calculate the energy of activation.
Given $R=8.314 \ J \ K^{-1} \ mol^{-1}, \log 4=0.6021$

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The rate of a reaction quadruples when temperature changes from $27^{\circ} C$ to $57^{\circ} C$. Calculate the energy of activation.Given $R=8.314 \ J \ K^{-1} \ mol^{-1}, \log 4=0.6021$