Chemistry · 2015
JEE Main · 11 April 2015, Shift 1 · Q35
For the equilibrium, A ( g ) ⇌ B ( g ), Δ H is -40 kJ/mol. If the ratio of the activation energies of the forward ( E_f) and reverse ( E_b )…
For the equilibrium, $\displaystyle \mathrm{A}(\mathrm{g}) \rightleftharpoons \mathrm{B}(\mathrm{g}), \Delta \mathrm{H}$ is -$\displaystyle 40$ kJ/mol. If the ratio of the activation energies of the forward $\displaystyle \left(\mathrm{E}_f\right)$ and reverse $\displaystyle \left(\mathrm{E}_{\mathrm{b}}\right)$ reactions is $\displaystyle \frac{2}{3}$ then :
Official answer
(3)
$\displaystyle \mathrm{E}_f=80 \mathrm{~kJ} / \mathrm{mol} ; \mathrm{E}_{\mathrm{b}}=120 \mathrm{~kJ} / \mathrm{mol}$
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JEE Main 2015 Chemistry question, with the answer from NTA’s final answer key. Where our answers come from.