TS EAMCET · Chemistry · Chemical Kinetics

For a hypothetical reaction, \(A \rightarrow C\) \[ \begin{aligned} & A \underset{k_2}{\stackrel{k_1}{\rightleftharpoons}} B(\text { Fast }) \ & A+B \stackrel{k_1}{\underset{k_2}{\rightleftharpoons}} C \text { (Slow) } \end{aligned} \] Rate law for this reaction is

A \(\propto[A][B]\)
B \(\propto[A]^2\)
C \(\propto[A]^2[B]^2\)
D \(\propto[A]^2[B]\)

Verified Solution

Answer & Solution

Correct Answer

(A) \(\propto[A][B]\)

Step-by-step Solution

Detailed explanation

Rate of reaction is directly proportional to the product of concentration of reactants. Rate law is always written for slow step in the reaction. For \(A+B \stackrel{k_3}{\longrightarrow} C\) (slow) \[ R=k_3[A][B] \] So, rate law for the reaction will be directly proportional to…

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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