What is the activation energy for a reaction if its rate doubles when the temperature is raised from $20^{\circ} \mathrm{C}$ to $35^{\circ} \mathrm{C}$? $\left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right)$

$269 \mathrm{~kJ} \mathrm{~mol}^{-1}$

$15.1 \mathrm{~kJ} \mathrm{~mol}^{-1}$

$342 \mathrm{~kJ} \mathrm{~mol}^{-1}$

NEET UG CHEMISTRY MCQ: CHEMICAL KINETICS

1 Hard

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Application +4 | -1

What is the activation energy for a reaction if its rate doubles when the temperature is raised from

20^{\circ} \mathrm{C}

35^{\circ} \mathrm{C}

\left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right)

View answer and explanation

Correct option: B

34.5 \mathrm{~kJ} \mathrm{~mol}^{-1}

Option B (

34.5 \mathrm{~kJ} \mathrm{~mol}^{-1}

) is correct because it is calculated using the Arrhenius equation relating rate constants and temperatures.