Chemistry - Chemical Kinetics Question with Solution | TestHub

Dinitrogen pentoxide decomposes on heating to nitrogen dioxide and oxygen following first-order kinetics:

$2N_2{O}_5(g)⟶4N{O}_2(g)+O_2(g)$

Initially, $0.2$ mole of $N_2{O}_5$ was taken in a vessel of capacity 1 L and heated to a Certain temperature of$T$ (Kelvin), at which the reaction begins. The concentration of $N_2{O}_5$ is measured at different time intervals by withdrawing samples of the reaction mixture. A plot of $\ln [N_2{O}_5]$ vs time is shown in Figure 1. The rate constant ($k$) of the reaction is determined from the slope of this linear plot. The experiment was repeated at five different temperatures, and the rate constants were calculated for each temperature. A plot of $\ln k$ versus $(temperature{)}^{-1}$ is shown in Figure 2.