Q77 · CSIR NET Chemistry, December 2016
Paper: CSIR NET December 2016 · Subject: Physical Chemistry · Chapter: Chemical Kinetics · Topic: Arrhenius Activation · Marks: 2 · Difficulty: Medium
For a reaction with an activation energy of $49.8\,\mathrm{kJ\,mol^{-1}}$, the ratio of the rate constants at 600 K and 300 K, ($k_{600}/k_{300}$), is approximately ($R = 8.3\,\mathrm{J\,mol^{-1}K^{-1}}$)
(a)$\ln 10$
(b)10
(c)10+e
(d)$e^{10}$
Answer
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Explanation
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Study loop for Chemical Kinetics