JEE Mains · Chemistry · STD 12 - 3. Chemical kinetics
The rate of a reaction quadruples when the temperature changes from \(300\) to \(310\, K\). The activation energy of this reaction is ........... \(kJ\, mol^{-1}\) (Assume activation energy and pre-exponential factor are independent of temperature ; \(ln\, 2\, = 0.693 ; R\, = 8.314\, J\, mol^{-1}\, K^{-1}\) )
- A \(107.2\)
- B \(53.6\)
- C \(26.8\)
- D \(214.4\)
Answer & Solution
Correct Answer
(A) \(107.2\)
Step-by-step Solution
Detailed explanation
\(\ln \,\frac{{{K_2}}}{{{K_1}}}\, = \,\frac{{{E_a}}}{R}\,\left( {\frac{1}{{{T_1}}}\, - \,\frac{1}{{{T_2}}}} \right)\) \(\ln \,\,4\, = \,\frac{{{E_a}}}{{8.314}}\left( {\frac{{310 - 300}}{{310 \times 300}}} \right)\)…
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