TS EAMCET · Chemistry · Chemical Kinetics

The rate constant of a reaction is increased $4$ times after addition of catalyst to the reaction mixture at the same temperature of $27 ° C$ . The change in the activation energy of this reaction is
(Take $\ln (\frac{1}{4}) = - 1.386, R = 8.314$ )

A $- 15 kJ / mol$
B $- 1.5 kJ / mol$
C $- 3.45 kJ / mol$
D $- 34.5 kJ / mol$

Verified Solution

Answer & Solution

Correct Answer

(C) $- 3.45 kJ / mol$

Step-by-step Solution

Detailed explanation

According to arrhenius equation k=Ae-Ea/RTe-Ea/RT= Boltzmann factor k=Ae-Ea1/RT.......1 Where, k=rate constant A=pre-exponential factor Ea=Activation energy R=Universal gas constant T=temperature When catalyst is added reaction rate constant increases by 4 times…

Apply the relevant identity from the chapter and substitute the values established in the previous step, keeping the original constraint in view.

Use the simplified expression to isolate the unknown, then plug the result back into the question setup to confirm the working is internally consistent.

Cross-check against a boundary or limiting case. Both the dimensional balance and the qualitative behaviour at the extreme should agree with the candidate answer.

Combine the steps above to identify the correct option. The remaining choices each fail at least one of the consistency, dimensional, or boundary checks.

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The rate constant of a reaction is increased 4 times after addition of catalyst to the reaction mixture at the same temperature of 27 °C. The change in the activation energy of this reaction is(Take ln14=-1.386,R=8.314)

Step-by-step Solution

The rate constant of a reaction is increased $4$ times after addition of catalyst to the reaction mixture at the same temperature of $27 ° C$ . The change in the activation energy of this reaction is
(Take $\ln (\frac{1}{4}) = - 1.386, R = 8.314$ )