QJEEM17Ch42e2: JEE Main 2017 Chemistry - Class 12 JEEM17Ch42e2 Solution: The rate of a reaction quadruples when the temperature changes…

According to Arrhenius equation,

$\log {{{k_2}} \over {{k_1}}} = {{{E_a}} \over {2.303R}}\left( {{{{T_2} - {T_1}} \over {{T_1}{T_2}}}} \right)$

Substituting the given values in the equation, we get

$\log 4 = {{{E_a}} \over {2.303 \times 8.314\,J\,{K^{ - 1}}mo{l^{ - 1}}}}\left( {{{310 - 300} \over {300 \times 310}}} \right)$

${E_a} = {{0.602 \times 2.303 \times 8.314 \times 300 \times 310} \over {10}}$

= 107197.12 J/mol ^{$-$ 1} or 107.2 kJ/mol ^{$-$ 1}