JEE Main · 2023 · 08 Apr 2023 · Shift 1 · Chemical Kinetics

The Arrhenius equation $k=A{e}^{-E_a/RT}$ governs how the rate constant responds to temperature. In logarithmic form $\ln k=\ln A-\frac{E_a}{R}\cdot \frac{1}{T}$, the slope against $1/T$ is $-E_a/R$, so a larger activation energy makes $k$ vary more steeply with temperature; statement (A) is correct. If $E_a=0$ the exponential becomes $e^0=1$ and $k=A$, independent of temperature, so statement (B) is correct. Statement (C) asserts the reverse of (A) and is wrong. Statement (D) is wrong, because no dependence of $k$ on temperature corresponds to $E_a=0$, not to a negative activation energy. Two of the statements are correct.