Consider the given plots for a reaction obeying Arrhenius equation $\left(0^{\circ} \mathrm{C}<\mathrm{T}<300^{\circ} \mathrm{C}\right)$ : ( k and $\mathrm{E}_{\mathrm{a}}$ are rate constant and activation energy respectively) Choose the correct option:

JEE Main · 2019 · 10 Jan 2019 · Shift 1 · Chemical Kinetics

Consider the given plots for a reaction obeying Arrhenius equation

(0^{\circ} C < T < 30 0^{\circ} C)

: ( k and

E_{a}

are rate constant and activation energy respectively)

Choose the correct option:

(A)I is right but II is wrong✓ Correct
(B)Both I and li are correct
(C)I is wrong but II is right
(D)Both I and II are wrong

Answer: (A)

Solution

Taking logs of the Arrhenius equation gives

ln k = ln A - \frac{E _{a}}{R} \cdot \frac{1}{T}

, a straight line only when

ln k

is plotted against

1/ T

, with slope

- E_{a} / R

. The first plot, drawn that way, is correct, while the second plot's axes do not give the linear form the equation demands and so misrepresent it. Hence the first statement holds and the second does not.

JEE Main · 2019 · 10 Jan 2019 · Shift 1 · Single correct option

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