The Arrhenius equation $k = A\,e^{-E_a/RT}$ predicts that, at a given temperature, increasing the ACTIVATION ENERGY $E_a$ will

1. NCERT §3.5 introduces the Arrhenius equation: $k = A\,e^{-E_a/RT}$. 2. At fixed $T$, the exponential term $e^{-E_a/RT}$ DECREASES as $E_a$ increases, because the argument $-E_a/RT$ becomes more negative. 3. So a higher activation barrier makes the reaction slower at the same temperature — exponentially slower. 4. This is WHY a catalyst (which lowers $E_a$) speeds up reactions so dramatically: a modest drop in $E_a$ can change $k$ by orders of magnitude through the exponential. 5. Option A reverses the dependence. Option C ignores the $E_a$ term entirely. Option D would be a LINEAR (not exponential) dependence. _Source: NCERT Class 12 Chemistry Part 1, Ch 3, §3.5 (Temperature Dependence of the Rate — Arrhenius Equation), p. 18–19._