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  4. What is the activation energy (KJ/mol) for a reaction if its rate constant doubles when the temperature is raised from 300 K to 400 K ? (R = 8.314 J mol-1 K-1)

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Q. What is the activation energy (KJ/mol) for a reaction if its rate constant doubles when the temperature is raised from 300 K to 400 K ? (R = 8.314 J $mol^{-1} K^-1$)

AIIMSAIIMS 2019Chemical Kinetics

Solution:

log $\frac{K_{2}}{K_{1}}=\frac{E_{a}}{2.3R}\left(\frac{1}{T_{1}}-\frac{1}{T_{2}}\right)$
log $\frac{2}{1}=\frac{E_{a}}{2.33\times8.31}\quad\quad\left(\frac{1}{300}-\frac{1}{400}\right)$
= 0.3 x 2.3 x 8.31 x 3 x 400 = Ea
Ea = 6.88 kJ