Question

The rate constant of a reaction is $1.5\times {10}^7{s}^{-1}$ at ${50}^{\circ }C$ and $4.5\times {10}^7{s}^{-1}$ at ${100}^{\circ }C$. Evaluate the Arrhenius parameter $\left(A\right)$ and the activation energy $\left(E_a\right)$.

• A. $A=5.42\times {10}^{10},E_a=2.2\times {10}^{4}J/mol$
• B. $A=5.42\times {10}^9,E_a=2.2\times {10}^{4}J/mol$
• C. $A=2.2\times {10}^4,E_a=5.42\times {10}^{9}J/mol$
• D. $A=5.42\times {10}^5,E_a=2.2\times {10}^{3}J/mol$

Answer 1

The correct option is A $A=5.42\times {10}^{10},E_a=2.2\times {10}^{4}J/mol$