The decomposition of N2O into N2 and O2 in presence of gaseous argon follows second order kinetics with k=5.0×1011Lmol−1s−1e The energy of activation of the reaction is :

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The decomposition of $N_{2} O$ into $N_{2}$ and $O_{2}$ in presence of gaseous argon follows second order kinetics with $k = (5.0 \times 10^{11} L {mol}^{- 1} s^{- 1}) e$ The energy of activation of the reaction is :

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$41570 J$

$5.0 \times 10^{11} J$

$5000 J$

$345612.98 J$

answer is D.

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Detailed Solution

The energy of activation of the reaction is :

$\frac{E_{a}}{R} = 41570 E_{a} = 41570 \times R E_{a} = 41570 \times 8.31 E_{a} = 345612.98 J$

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