CUET · CHEMISTRY · PYQ PAPER 2025
\(2 A+B \rightarrow A_2 B\)
For the above reaction, the rate law equation is, rate \(=k[A][ B ]^2\) with \(k=2.0 \times 10^{-6} mol^{-2} L^2 s^{-1}\). If the initial concentrations of \(A\) and \(B\) were \(0.1 mol L ^{-1}\) and \(0.2 mol L ^{-1}\), respectively, the rate of reaction after \([A]\) is reduced to 0.06 \(mol L ^{-1}\) will be
- A \(3.07 \times 10^{-9} \text{ mol } L^{-1} s^{-1}\)
- B \(3.89 \times 10^{-9} \text{ mol } L^{-1} s^{-1}\)
- C \(4.80 \times 10^{-9} \text{ mol } L^{-1} s^{-1}\)
- D \(8.0 \times 10^{-9} \text{ mol } L^{-1} s^{-1}\)
Answer & Solution
Correct Answer
(B) \(3.89 \times 10^{-9} \text{ mol } L^{-1} s^{-1}\)
Step-by-step Solution
Detailed explanation
\(\Delta [A] = 0.1 - 0.06 = 0.04 \text{ mol L}^{-1}\) \(\Delta [B] = \frac{1}{2} \Delta [A] = \frac{1}{2} \times 0.04 = 0.02 \text{ mol L}^{-1}\) \([B]_f = 0.2 - 0.02 = 0.18 \text{ mol L}^{-1}\) \(\text{rate} = k[A][B]^2 = (2.0 \times 10^{-6})(0.06)(0.18)^2\)…
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