The rate constant of a reaction at 500 ~K and 700 ~K are 0.02 ~s ⁻¹ and 0.2 ~s ⁻¹ respectively. The activation energy of the reaction (in . kJ mol ⁻¹ ) is (R=8.3 JK ⁻¹ ~mol ⁻¹ )

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Correct answer: B. 33.45

Given, k₁=0.02 ~s ⁻¹ aligned & k₂=0.2 ~s ⁻¹ & E_a=? & R=8.3 & T₁=500 ~K & T₂=700 ~K aligned aligned & In k₂ k₁ =- E_a R ( 1 T₂ - 1 T₁ ) & In 0.2 0.02 =- E_a 8.3 [ 1 700 - 1 500 ] & In 10= -E_a 8.3 ( 500-700 700 500 ) aligned 2.302 8.3 700 500=200 E_a E_a= 2.302 8.3 700 500 200 aligned & =33436 ~J / mol & 33.44 ~kJ / mol aligned

The rate constant of a reaction at 500 ~K and 700 ~K are 0.02 ~s ⁻¹ and 0.2 ~s ⁻¹ respectively. The activation energy of the reaction (in . kJ mol ⁻¹ ) is (R=8.3 JK ⁻¹ ~mol ⁻¹ )

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