Consider A \stackrel{ k _1}{\\xrightarrow } B and C \stackrel{ k _2}{\\xrightarrow } D are two reactions. If the rate constant ( k _1) of the A \to B reaction can be expressed by the following equation \log _{10} k =14.34-\frac{1.5 \times 10^4}{T \/ K } and activation energy of C \to D reaction (E a_2) is \frac{1}{5} th of the A \to B reaction (E a_1), then the value of (E a_2) is \_\_\_\_ kJmol ^{-1}. (Nearest Integer) [22 Jan 2026 Shift 2]

Chemical Kinetics Part 2

Section: Chemistry

Question : 10 of 111

Marks: +1, -0

Consider A

‌───────▶‌

B and C

‌───────▶‌

D are two reactions. If the rate constant (k1) of the A→B reaction can be expressed by the following equation log10k=14.34−‌

1.5×104

T∕K

and activation energy of C→D reaction (Ea2) is ‌

th of the A→B reaction (Ea1), then the value of (Ea2) is ____ kJmol−1. (Nearest Integer)

[22 Jan 2026 Shift 2]

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