Chemical Kinetics Question 349
Question: The rate coefficient (K) for a particular reactions is $ 1.3\times {10^{-4}}{M^{-1}}{s^{-1}} $ at $ 100{}^\circ C $ , and $ 1.3\times {10^{-3}}{M^{-1}}{s^{-1}} $ at $ 150{}^\circ C $ . What is the energy of activation $ ( E_{a} ) $ (in kJ) for this reaction- (R = molar gas constant $ =8.314J{K^{-1}}mo{l^{-1}} $ )
Options:
A) 16
B) 60
C) 99
D) 132
Show Answer
Answer:
Correct Answer: B
Solution:
[b] According to Arrhenius equation $ \log \frac{k_2}{k_1}=\frac{E_{a}}{2.303R}( \frac{1}{T_1}-\frac{1}{T_2} ) $
$ \log \frac{1.3\times {10^{-3}}}{1.3\times {10^{-4}}}=\frac{E_{a}}{2.303\times 8.314}[ \frac{1}{373}-\frac{1}{423} ] $
$ I=\frac{E_{a}}{2.303\times 8.314}[ \frac{1}{373}-\frac{1}{423} ] $
$ E_{a}=60kJ/mol $
