Q. Observe the following reaction, $2A + B \rightarrow C$ The rate of formation of C is $2.2 \times 10^{- 3}$𝑚𝑜𝑙 $L^{- 1}\min^{- 1}.$ What is the value of $- \frac{d\lbrack A\rbrack}{dt}(mol\ L^{- 1}\min^{- 1})$ ?
A) $2.2 \times 10^{- 3}$
B) $1.1 \times 10^{- 3}$
C) $4.4 \times 10^{- 3}$
D) $5.5 \times 10^{- 3}$
Explanation
(c)
$2A + B \rightarrow C$
Rate of reaction,
$= - \frac{1}{2}\frac{d\lbrack A\rbrack}{dt} = - \frac{d\lbrack B\rbrack}{dt} = \frac{d\lbrack C\rbrack}{dt}$
$\therefore - \frac{d\lbrack A\rbrack}{dt} = 2\frac{d\lbrack C\rbrack}{dt}$
$= 2 \times 2.2 \times 10^{- 3}$
$= 4.4 \times 10^{- 3}mol\ L^{- 1}\min^{- 1}$
Reviewed by Dr. Abubacker
Physics Educator & NEET/JEE Specialist
Ph.D. in Physics with 19+ years of teaching experience.