🧪 Chemistry · Chemical Kinetics · NEET & JEE

For a reaction with k₁ = 0.005 s⁻¹ at 300 K and k₂ = 0.020 s⁻¹ at 320 K, the activation energy is approximately:

Answer: 55 kJ/mol.

A 45 kJ/mol
B 55 kJ/mol
C 35 kJ/mol
D 65 kJ/mol

Correct answer: B. 55 kJ/mol

Explanation: Ea = 2.303R × (T₁T₂/(T₂-T₁)) × log(k₂/k₁) = 2.303×8.314×(300×320/20)×log(4) ≈ 55,300 J/mol ≈ 55 kJ/mol.

First-order decay curve: concentration halves every t½, and that half-life is constant - a defining test for first-order kinetics.

Concept context

Study the speed of reactions and what affects it: concentration, temperature, and catalysts. Covers rate law, order of reaction, the Arrhenius equation, and reaction mechanisms step by step.

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For a reaction with k₁ = 0.005 s⁻¹ at 300 K and k₂ = 0.020 s⁻¹ at 320 K, the activation energy is approximately:

Concept context

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