(C) For the reaction $2 A + B \longrightarrow C$,the rate of reaction is given by: $-\frac{1}{2} \frac{d[A]}{d t} = -\frac{d[B]}{d t} = \frac{d[C]}{d

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(C) For the reaction $2 A + B \longrightarrow C$,the rate of reaction is given by: $-\frac{1}{2} \frac{d[A]}{d t} = -\frac{d[B]}{d t} = \frac{d[C]}{d t}$.Given that the rate of formation of $C$ is $\frac{d[C]}{d t} = 2.2 \times 10^{-3} \ mol \ L^{-1} \ min^{-1}$.From the rate expression,we have $-\frac{1}{2} \frac{d[A]}{d t} = \frac{d[C]}{d t}$.Therefore,$-\frac{d[A]}{d t} = 2 \times \frac{d[C]}{d t}$.Substituting the value: $-\frac{d[A]}{d t} = 2 \times 2.2 \times 10^{-3} = 4.4 \times 10^{-3} \ mol \ L^{-1} \ min^{-1}$.

Class 12 Chemistry Chemical Kinetics Rate of a reaction

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Observe the following reaction: $2 A + B \longrightarrow C$. The rate of formation of $C$ is $2.2 \times 10^{-3} \ mol \ L^{-1} \ min^{-1}$. What is the value of $-\frac{d[A]}{d t}$ (in $mol \ L^{-1} \ min^{-1}$)?

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A
$2.2 \times 10^{-3}$
B
$1.1 \times 10^{-3}$
C
$4.4 \times 10^{-3}$
D
$5.5 \times 10^{-3}$

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Observe the following reaction: $2 A + B \longrightarrow C$. The rate of formation of $C$ is $2.2 \times 10^{-3} \ mol \ L^{-1} \ min^{-1}$. What is the value of $-\frac{d[A]}{d t}$ (in $mol \ L^{-1} \ min^{-1}$)?

Similar Questions

For the elementary reaction,$3 H_{2(g)} + N_{2(g)} \rightarrow 2 NH_{3(g)}$,identify the correct relation among the following relations:

Explain the average rate of reaction for a hypothetical $R \longrightarrow P$ reaction.

In a reaction,$n_1A + n_2B \to m_1C + m_2D$,$5 \ M$ of reactant $A$ are allowed to react with $3 \ M$ of reactant $B$. After $5 \ sec$,the concentration of $A$ was found to be $4 \ M$. What are the rate of decomposition of $A$ and the rate of formation of $D$,respectively?

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