The decomposition of N2O into N2 O2 in presence of gaseous argon follow second order kinetics with k =(41570-/T) (5.0 × 1011 L mol-1 s-1) e The energy of activation of the reaction is

Question

The decomposition of N2O into N2 O2 in presence of gaseous argon follow second order kinetics with k =(41570-/T) (5.0 × 1011 L mol-1 s-1) e The energy of activation of the reaction is (A) 5.0 × 1011 J (B) 41570 J (C) 5000 J (D) 345612.98 J

Tardigrade Admin · Accepted Answer

Ea = 41570 × R = 41570 × 8.31 =345612.98 J

Q. The decomposition of $N_{2} O$ into $N_{2}$ & $O_{2}$ in presence of gaseous argon follow second order kinetics with $k = \frac{41570}{-} T$ $(5.0 \times 1 0^{11} L m o l^{- 1} s^{- 1}) e$ The energy of activation of the reaction is

$5.0 \times 1 0^{11} J$

$41570 J$

$5000 J$

$345612.98 J$

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

Q. The decomposition of N2​O into N2​ & O2​ in presence of gaseous argon follow second order kinetics with k=−41570​T (5.0×1011Lmol−1s−1)e The energy of activation of the reaction is

5.0×1011J

41570J

5000J

345612.98J