Q61 · CSIR-NET Chemistry, June 2018
Paper: CSIR-NET June 2018 · Subject: Physical Chemistry · Chapter: Chemical Kinetics · Topic: Steady State Approximation · Marks: 2 · Difficulty: Hard
Elementary steps of a reaction are as follows \[ \begin{array}{l} \mathrm{A}+\mathrm{B} \xrightarrow[\mathrm{k}_{-1}]{\mathrm{k}_{1}} 2 \mathrm{C} \\ 2 \mathrm{C} \xrightarrow{\mathrm{k}_{2}} \mathrm{D} \end{array} \]
If steady state approximation is applicable to C, the rate of product formation in the reaction is (a)proportional to [A][B]
(b)proportional to $[\mathrm{A}]^{2}[\mathrm{B}]^{2}$
(c)proportional to $[\mathrm{A}]^{1 / 2}[\mathrm{B}]^{1 / 2}$
(d)independent of $[\mathrm{A}][\mathrm{B}]$
Answer
Answer: A ✓ checked by 4AB · confidence high
The source book printed no answer; this one was worked out and checked — see the explanation.
Explanation
Applying the steady state to C gives 2k₁[A][B] = 2(k₋₁ + k₂)[C]², so [C]² ∝ [A][B]. Rate = k₂[C]² is proportional to [A][B] (a).
Study loop for Chemical Kinetics
· Browse this chapter in the app