Subject: Physical Chemistry · Chapter: Chemical Kinetics · Topic: Arrhenius Activation · Exam: NET DEC 2016 · Marks: 2 · Difficulty: Medium
For a reaction with an activation energy of $49.8 \mathrm{kJ} \mathrm{mol}^{-1}$, the ratio of the rate constants at 600 K and $300 \mathrm{K},\left(\mathrm{k}_{600} / \mathrm{k}_{300}\right)$, is approximately $\left(\mathrm{R}=8.3 \mathrm{J} \mathrm{mol}^{-1} \mathrm{K}^{-1}\right)$
(a)$\ln 10$
(b)10
(c)10+e
(d)$\mathrm{e}^{10}$
Answer
SELF-PRACTICE — the source book printed no answer.
Nothing is invented here, so this question has no answer on record.