Chemistry: Acertain reaction has an activation energy of 66.41 kj/mol. at what kelvin temperature will the reaction proceed 3.00 times faster than it did at 293 k?

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Acertain reaction has an activation energy of - id66411799237, culbertchristi6111

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31.12.2021

Answer : The temperature will be, 392.462 K

Explanation :

According to the Arrhenius equation,

$K=A\times e^{\frac{-Ea}{RT}}$

or,

$\log (\frac{K_2}{K_1})=\frac{Ea}{2.303\times R}[\frac{1}{T_1}-\frac{1}{T_2}]$

where,

K_1 = rate constant at T_1 = K_1

K_2 = rate constant at T_2 = 3K_1

= activation energy for the reaction = 66.41 kJ/mole = 66410 J/mole

R = gas constant = 8.314 J/mole.K

T_1 = initial temperature = 293 K

T_2 = final temperature = ?

Now put all the given values in this formula, we get:

$\log (\frac{3K_1}{K_1})=\frac{66410J/mole}{2.303\times 8.314J/mole.K}[\frac{1}{293K}-\frac{1}{T_2}]$

T_2=392.462K

Therefore, the temperature will be, 392.462 K

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