Chemical Kinetics Question 305
Question: For the first order reaction $ A\xrightarrow{{}}B+C $ is carried out at $ 27{}^\circ C $ . If $ 3.8\times {10^{-16}} $ % of the reactant molecules exists in the activated state, the $ E_4 $ (activation energy) of the reaction is:
Options:
A) 12 kJ/mol
B) 831.4 kJ/mol
C) 100 kJ/mol
D) 88.57 kJ/mol
Show Answer
Answer:
Correct Answer: C
Solution:
[c] $ {e^{-\frac{E_{a}}{RT}}}=3.8\times -\frac{{10^{-16}}}{100} $
$ -\frac{E_{a}}{RT}=\ln ,3.8\times {10^{-18}}E_{a}=100kJ/mol $
