The rate coefficient $(k)$ for a particular reactions is $1.3 imes 10^{-4} \mathrm{M}^{-1} \mathrm{~s}^{-1}$ at $100^{\circ} \mathrm{C}$, and $1.3 imes 10^{-3}$ $\mathrm{M}^{-1} \mathrm{~s}^{-1}$ at $150^{\circ} \mathrm{C}$. What is the energy of activation…

Question

The rate coefficient $(k)$ for a particular reactions is $1.3 	imes 10^{-4} \mathrm{M}^{-1} \mathrm{~s}^{-1}$ at $100^{\circ} \mathrm{C}$, and $1.3 	imes 10^{-3}$ $\mathrm{M}^{-1} \mathrm{~s}^{-1}$ at $150^{\circ} \mathrm{C}$. What is the energy of activation $\left(\mathrm{E}_{\mathrm{A}}ight)$ (in $\left.\mathrm{kJ}ight)$ for this reaction? $(\mathrm{R}=$ molar gas constant $=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$ )

Aicharya · Accepted Answer

According to Arrhenius equation $ \begin{aligned} &\log \frac{k_2}{k_1}=\frac{E_a}{2.303 R}\left(\frac{1}{T_1}-\frac{1}{T_2}ight) \ &\log \frac{1.3 	imes 10^{-3}}{1.3 	imes 10^{-4}}=\frac{E_a}{2.303 	imes 8.314}\left[\frac{1}{373}-\frac{1}{423}ight] \ &1=\frac{E_a}{2.303 	imes 8.314}\left[\frac{1}{373}-\frac{1}{423}ight] \ &E_a=60 \mathrm{~kJ} / \mathrm{mole} \end{aligned} $

The rate coefficient $(k)$ for a particular reactions is $1.3 \times 10^{-4} \mathrm{M}^{-1}…

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