For a first-order reaction at 300 , ^circ C,t | vedclass

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(B) The Arrhenius equation is given by $k = A e^{-E_a / RT}$.Given values: $A = 1.45 	imes 10^{11} \, s^{-1}$,$E_a = 35 \, kcal \, mol^{-1} = 35000 \

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$7.96 	imes 10^{-3} \, s^{-1}$

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(B) The Arrhenius equation is given by $k = A e^{-E_a / RT}$.Given values: $A = 1.45 	imes 10^{11} \, s^{-1}$,$E_a = 35 \, kcal \, mol^{-1} = 35000 \, cal \, mol^{-1}$,$T = 300 + 273 = 573 \, K$,and $R = 1.987 \, cal \, K^{-1} \, mol^{-1}$.Calculate the exponent: $-E_a / RT = -35000 / (1.987 	imes 573) \approx -35000 / 1138.55 \approx -30.736$.Now,$k = 1.45 	imes 10^{11} 	imes e^{-30.736} \approx 1.45 	imes 10^{11} 	imes 4.975 	imes 10^{-14} \approx 7.21 	imes 10^{-3} \, s^{-1}$.Rounding to the nearest option,the correct value is $7.96 	imes 10^{-3} \, s^{-1}$.

For a first-order reaction at $300 \, ^\circ C$,the activation energy is $35 \, kcal \, mol^{-1}$ and the frequency factor is $1.45 \times 10^{11} \, s^{-1}$. Calculate the rate constant.

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