Chemistry: We know that for a given reaction when the temperature increases from 100 k to 200 k the rate constant doubles. what is the activation energy in kj/mol

Compressed spring has kinetic energy...

We know that for a given reaction when the temperature

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11.03.2022

The activation energy of the reaction is 1.152 kJ/mol.

Explanation:

Activation energy is the minimum amount which is absorbed by the reactant molecules to undergo chemical reaction.

Initial temperature of reaction = T_1=100 K

Final temperature of reaction = T_2=200 K

Initial rate of the reaction at 100 k = K_1=k

Final rate of the reaction at 200 k = K_2=2k

Activation energy is calculated from the formula:

$\log\frac{K_2}{K_1}=\frac{E_a}{2.303\times R}(\frac{T_2-T_1}{T_1T_2})$

R = Universal gas constant = 8.314 J/ K mol

$\log\frac{2k}{k}=\frac{E_a}{2.303\times 8.314 J/K mol}(\frac{200 K-100K}{200 K\times 100K})$

E_a=1,152.772 J/mol=1.152 kJ/mol

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