The rate constant for the first order decomposition of N 2 O 5 is given by the following equation: log k=23 · 6-(2 × 10^4 K)/( T) Calculate E a for…

log k = log A - E a/(2·303 RT) -E a/(2·303 R) = -2 × 10^4 K E a = 2·303 × 8·314 J K^-1 mol^-1 × 2 × 10^4 K E a = 3.830 × 10^5 J mol^-1

CBSE 2023 · Region 4 · Set 1 · Q22 · 2 marks

The rate constant for the first order decomposition of $\displaystyle \mathrm{N}_{2} \mathrm{O}_{5}$ is given by the following equation : \[\log \mathrm{k}=23 \cdot 6-\frac{2 \times 10^{4} \mathrm{~K}}{\mathrm{~T}} \] Calculate $\displaystyle \mathrm{E}_{\mathrm{a}}$ for this reaction. \[\left[\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right] \]

Chemical KineticsTemperature Dependence of the Rate of a ReactionApplyvery_short_answermedium