Chemical Kinetics Part 1

Per the Arrhenius equation, $k = A\,e^{-E_a/(RT)}$, where $T$ is the absolute temperature in kelvin.Plot I (variation of $k$ with $E_a$): at a fixed temperature, $k$ decreases as $E_a$ increases, because a larger $E_a$ makes the exponent $-E_a/(RT)$ more negative.The curve therefore starts high on the vertical $k$ axis and falls steeply at first, then flattens out, approaching $k = 0$ only for infinitely large $E_a$; this is exactly the shape shown in plot I, so I is correct.Plot II (variation of $k$ with $T$ given in $^\circ\text{C}$): with $E_a$ fixed, raising $T$ increases $e^{-E_a/(RT)}$, so $k$ increases.The increase is gentle at low temperature and becomes steeper as $T$ rises, and at $0\,{}^\circ\text{C}$ the value of $k$ is very small though not zero, so the curve begins essentially near the origin, exactly as shown in plot II; hence II is also correct.Thus both plots correctly represent the behaviour of a reaction obeying the Arrhenius equation, and the correct option is 'Both I and II are correct'.The marked option 'I is right but II is wrong' is therefore incorrect.