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 $=8.314J{K}^{-1}mo{l}^{-1})$

• A. 16
• B. 60
• C. 99
• D. 132

Answer 1

Answer: (B)

According to Arrhenius equation

$log\frac{k_2}{k_1}=\frac{E_a}{2.303R}\left(\frac{1}{T_1}-\frac{1}{T_2}\right)$

$log\frac{1.3\times 10^{-3}}{1.3\times 10^{-4}}=\frac{E_a}{2.303\times 8.314}\left[\frac{1}{373}-\frac{1}{423}\right]$

$1==\frac{E_a}{2.303\times 8.314}\left[\frac{1}{373}-\frac{1}{423}\right]$

$E_a=60kJ/mole$