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Consider A k ₁ ~B and C k ₂ D are two reactions. If the rate constant ( k ₁ ) of the A B reaction can be expressed by the following equation ₁₀ k =14.34- 1.5 10⁴ ~T / K and activation energy of C D reaction (E a₂ ) is 1 5 th of the A B reaction (E a₁ ) , then the value of (E a₂ ) is _ _ _ _ kJ mol ⁻¹ . (Nearest Integer)

Correct answer

0

Step-by-step solution

From the Arrhenius equation: ₁₀ k = ₁₀ A - E_a 2.303RT . Comparing with given equation ₁₀ k₁ = 14.34 - 1.5 10^4 T , we get: E_ a₁ 2.303R = 1.5 10^4 K E_ a₁ = 1.5 10^4 2.303 8.314 = 1.5 10^4 0.01913 = 287 kJ/mol Since E_ a₂ = 1 5 E_ a₁ : E_ a₂ = 287 5 = 57.4 57 kJ/mol

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