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  • The rate of a reaction doubles when its temperature changes from 300 K to 310 K .Activation energy of such a reaction will be : (R = 8.314 JK-1 mol-1 and log 2 = 0.3

The rate of a reaction doubles when its temperature changes from 300 K to 310 K .Activation energy of such a reaction will be :

(R = 8.314 JK-1 mol-1 and log 2 = 0.301)

Option: 1

60.5 kJ mol-1


Option: 2

53.6 kJ mol-1


Option: 3

48.6 kJ mol-1


Option: 4

58.5 kJ mol-1


Answers (1)

best_answer

As we learned in

We know by Arrhenius equation

l_{n}\:\frac{k_{1}}{k_{2}}=\:\frac{E_{a}}{R}(\frac{1}{T_{1}}-\frac{1}{T_{2}})

=> 0.301 = \frac{E_{a}}{2.303\times8.314\times10^{-3}}\:(\frac{1}{300}-\frac{1}{310})

=> E_{a}\:=\:53.6\:kJ\:mol^{-1}

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