Arrange the following reactions in increasing order of the value of t…

The correct answer is Option (2) → (B), (A), (C), (D)

Core Formula (Arrhenius Ratio):

$\ln \left( \frac{k_{310}}{k_{300}} \right) = \frac{E_a}{R} \left( \frac{1}{300} - \frac{1}{310} \right)$

$\frac{1}{300} - \frac{1}{310} = \frac{10}{93000} = 1.075 \times 10^{-4}$

$R = 8.314 \, \text{J mol}^{-1} \text{K}^{-1}$

(A) $E_a = 70 \, \text{kJ} = 70000 \, \text{J}$:

$\ln \left( \frac{k_{310}}{k_{300}} \right) = \frac{70000}{8.314} \times 1.075 \times 10^{-4}$

$= 8421 \times 1.075 \times 10^{-4} = 0.905$

$\frac{k_{310}}{k_{300}} = e^{0.905} \approx 2.47$

(B) $E_a = 45 \text{ kJ} = 45000 \text{ J}$

$\ln\left(\frac{k_{310}}{k_{300}}\right) = \frac{45000}{8.314} \times 1.075 \times 10^{-4}$

$= 5413 \times 1.075 \times 10^{-4} = 0.582$

$\frac{k_{310}}{k_{300}} = e^{0.582} \approx 1.79$

(C) $E_a = 95 \text{ kJ} = 95000 \text{ J}$

$\ln\left(\frac{k_{310}}{k_{300}}\right) = \frac{95000}{8.314} \times 1.075 \times 10^{-4}$

$= 11428 \times 1.075 \times 10^{-4} = 1.229$

$\frac{k_{310}}{k_{300}} = e^{1.229} \approx 3.42$

(D) $E_a = 100 \text{ kJ} = 100000 \text{ J}$

$\ln\left(\frac{k_{310}}{k_{300}}\right) = \frac{100000}{8.314} \times 1.075 \times 10^{-4}$

$= 12027 \times 1.075 \times 10^{-4} = 1.293$

$\frac{k_{310}}{k_{300}} = e^{1.293} \approx 3.64$

Comparison:

Reaction	Ratio $k_{310}/k_{300}$
B	1.79
A	2.47
C	3.42
D	3.64