Paper: CSIR-NET June 2021 · Subject: Physical Chemistry · Chapter: Chemical Kinetics · Topic: Chemical Kinetics – General · Marks: 2 · Difficulty: Medium
The rate constant for the reaction $\mathrm{A}_{2} \mathrm{B}_{4} \mathrm{O} \rightarrow \mathrm{AB}_{4}+\mathrm{AO}$, is described as, $\log \mathrm{k}=14.1-\frac{10000 \mathrm{K}}{\mathrm{T}}$ the activation energy (in $\mathrm{kJ} \mathrm{mol}^{-1}$ ) is closest to
(a)191.4
(b)83.14
(c)382.8
(d)166.28
Answer
Answer: A ✓ checked by 4AB · confidence high
The source book printed no answer; this one was worked out and checked — see the explanation.
Explanation
log k = log A − Ea/(2.303RT): Ea = 2.303 × 8.314 × 10000 = 191,400 J = 191.4 kJ mol⁻¹.