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MHT CET202616 April 2026Morning ShiftChemistryChemical KineticsActual

The rate constant of reaction is 1.5 10^7 s ⁻¹ at 300 K and 3.0 10^7 s ⁻¹ at 330 K. What is the activation energy for the reaction? [ R 2.303 = 19.15 JK ⁻¹ mol ⁻¹ ]

Options

  1. A18.02 kJ mol ⁻¹
  2. B20.1 kJ mol ⁻¹
  3. C19.02 kJ mol ⁻¹
  4. D21.5 kJ mol ⁻¹

Correct answer

C. 19.02 kJ mol ⁻¹

Step-by-step solution

Using the Arrhenius equation: ( k₂ k₁ ) = E_a 2.303 R ( T₂ - T₁ T₁ T₂ ) Substituting the given values: ( 3.0 10^7 1.5 10^7 ) = E_a 19.15 ( 330 - 300 300 330 ) (2) = E_a 19.15 ( 30 99000 ) 0.301 = E_a 19.15 ( 1 3300 ) E_a = 0.301 19.15 3300 E_a = 19021.695 J mol ⁻¹ E_a 19.02 kJ mol ⁻¹ Answer: 19.02 kJ mol ⁻¹

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