For the reaction: 2(g) -> 4(g) + (g), the concentration of increases by 2.4 × 10^-2 M in 6 s. What w — Chemical Kinetics Chemistry Question

💡 Solution & Explanation

Average rate of appearance of $NO_2$ = Change in [$NO_2$] / dt = 2.4 × 10^-2 M / 6 s = 4 × 10^-3 M s^-1. From the stoichiometry of the reaction, rate of reaction = 1/4 d[$NO_2$]/dt = -1/2 d[$N_2O_5$]/dt. Thus, rate of disappearance of $N_2O_5$ = -d[$N_2O_5$]/dt = 1/2 (d[$NO_2$]/dt) = 1/2 * (4 × 10^-3) = 2 × 10^-3 M s^-1.