When creating an Arrhenius graphical plot of the natural logarithm of the rate constant () versus th — Chemical Kinetics Chemistry Question

💡 Solution & Explanation

Expanding the Arrhenius equation with natural logs yields $\ln k = \ln A - \frac{E_a}{R} \cdot \frac{1}{T}$. This linearly maps to $y = c + mx$. Since the variable on the x-axis is exactly $1/T$, the isolated mathematical slope ($m$) is strictly $-E_a / R$.