Chemistry · 2020
JEE Main · 6 September 2020, Shift 2 · Q48
The rate of a reaction decreased by 3.555 times when the temperature was changed from 40^° C to 30^° C. The activation energy (in kJ mol^-1 ) of the…
The rate of a reaction decreased by $\displaystyle 3.555$ times when the temperature was changed from $\displaystyle 40^{\circ} \mathrm{C}$ to $\displaystyle 30^{\circ} \mathrm{C}$. The activation energy (in $\displaystyle \mathrm{kJ} \mathrm{mol}^{-1}$ ) of the reaction is \_\_\_\_. Take; $\displaystyle \mathrm{R}=8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1} \ln 3.555=1.268$
Official answer
100 ± 0.1
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