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JIPMER 2014
Exam
JIPMER
Year
2014
Subject
Chemistry
Chapter
Chemical Kinetics

JIPMER 2014 · Chemistry · Chemical Kinetics

Observe the following reaction 2 A+B C The rate of formation of C...

Observe the following reaction 2A+B⟶C2 A+B \longrightarrow C The rate of formation of CC is 2.2×10−3 mol L−13 min−12.2 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-13} \mathrm{~min}^{-1}. What is the value of −d[A]dt(-\frac{d[A]}{d t}\left(\right. in \left.\mathrm{mol} \mathrm{L}^{-1} \min ^{-1}\right) ?

Options

  1. A2.2×10−32.2 \times 10^{-3}
  2. B1.1×10−31.1 \times 10^{-3}
  3. C4.4×10−34.4 \times 10^{-3}
  4. D5.5×10−35.5 \times 10^{-3}

Correct answer

C. 4.4×10−34.4 \times 10^{-3}

Step-by-step solution

2A+B⟶C2 A+B \longrightarrow C Rate of reaction, =−12d[A]dt=−d[B]dt=d[C]dt=-\frac{1}{2} \frac{d[A]}{d t}=-\frac{d[B]}{d t}=\frac{d[C]}{d t}∴−d[A]dt=2d[C]dt=2×2.2×10−3=4.4×10−3 mol L−1 min−1\begin{aligned} \therefore & -\frac{d[A]}{d t}=2 \frac{d[C]}{d t} \\ & =2 \times 2.2 \times 10^{-3}=4.4 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~min}^{-1}\end{aligned}$$
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