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 $



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