Q. When is the activation energy for the decomposition of $N_{2}O_{5}$ as, $N_{2}O_{5} \rightleftharpoons 2{NO}_{2} + \frac{1}{2}O_{2}$ If the values of rate constant $= 3.45 \times 10^{- 5}\$at $27℃$ and rate constant $= 6.9 \times 10^{- 3}\ at\ 67℃?$

A) 112.5 kJ
B) 200 kJ
C) 149.5 kJ
D) 11.25 kJ
Explanation

(a)
To be solved with the help of formula,
$\ \log\frac{k_{2}}{k_{1}} = \frac{E_{a}}{2.303\ R}\left\lbrack \frac{T_{2} - T_{1}}{T_{1}T_{2}} \right\rbrack$
$\ T_{1} = 273 + 27 = 300\ K$
$\ T_{2} = 273 + 67 = 340\ K$
$\log\frac{6.9 \times 10^{- 3}}{3.45 \times 10^{- 5}} = \frac{E_{a}}{2.303 \times 8.31}\left\lbrack \frac{340 - 300}{340 \times 300} \right\rbrack$
$\log 200 = \frac{E_{a}}{19.1379} \times \frac{40}{102000}$
$2.3010 = \frac{E_{a}}{19.14} \times \frac{4}{10200},$
$\ E_{a} = \frac{19.14 \times 10200 \times 2.3010}{4}$
$= 112304.907\ J = 112.3\ kJ$

Dr. Abubacker
Reviewed by Dr. Abubacker

Physics Educator & NEET/JEE Specialist

Ph.D. in Physics with 19+ years of teaching experience.