(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

Easy

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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What is the rate of formation of $O_2$ for the reaction stated below?
$2 N_2O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$
Given: $\left| \frac{d[N_2O_5]}{dt} \right| = 0.02 \ mol \ dm^{-3} \ s^{-1}$

MediumMHT CET 2024

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In a pseudo first order hydrolysis of ester in water,the following results were obtained:

$t \ (s)$ $0$ $30$ $60$ $90$

$[\text{Ester}] \ (mol \ L^{-1})$ $0.55$ $0.31$ $0.17$ $0.085$

What will be the average rate of reaction between the time interval $30 \ s$ to $60 \ s$?

Medium

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Select the correct reaction for the given rate: $\text{rate} = -\frac{1}{6} \frac{d[A]}{dt} = -\frac{1}{4} \frac{d[B]}{dt} = \frac{1}{3} \frac{d[C]}{dt} = \frac{1}{4} \frac{d[D]}{dt}$

MediumGUJCET 2025

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For the reaction $2A + 3B \rightarrow 4C$,the rate of reaction is expressed as:

Easy

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For the reaction,$N_{2(g)} + 3 H_{2(g)} \longrightarrow 2 NH_{3(g)}$,$NH_{3}$ is formed at a rate of $0.088 \ mol \ dm^{-3} \ s^{-1}$. Calculate the consumption rate of $N_{2(g)}$.

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$t \ (s)$	$0$	$30$	$60$	$90$
$[\text{Ester}] \ (mol \ L^{-1})$	$0.55$	$0.31$	$0.17$	$0.085$

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

What is the rate of formation of $O_2$ for the reaction stated below?$2 N_2O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$Given: $\left| \frac{d[N_2O_5]}{dt} \right| = 0.02 \ mol \ dm^{-3} \ s^{-1}$

In a pseudo first order hydrolysis of ester in water,the following results were obtained: $t \ (s)$ $0$ $30$ $60$ $90$ $[\text{Ester}] \ (mol \ L^{-1})$ $0.55$ $0.31$ $0.17$ $0.085$ What will be the average rate of reaction between the time interval $30 \ s$ to $60 \ s$?

Select the correct reaction for the given rate: $\text{rate} = -\frac{1}{6} \frac{d[A]}{dt} = -\frac{1}{4} \frac{d[B]}{dt} = \frac{1}{3} \frac{d[C]}{dt} = \frac{1}{4} \frac{d[D]}{dt}$

For the reaction $2A + 3B \rightarrow 4C$,the rate of reaction is expressed as:

For the reaction,$N_{2(g)} + 3 H_{2(g)} \longrightarrow 2 NH_{3(g)}$,$NH_{3}$ is formed at a rate of $0.088 \ mol \ dm^{-3} \ s^{-1}$. Calculate the consumption rate of $N_{2(g)}$.

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What is the rate of formation of $O_2$ for the reaction stated below?
$2 N_2O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$
Given: $\left| \frac{d[N_2O_5]}{dt} \right| = 0.02 \ mol \ dm^{-3} \ s^{-1}$

In a pseudo first order hydrolysis of ester in water,the following results were obtained:

$t \ (s)$ $0$ $30$ $60$ $90$

$[\text{Ester}] \ (mol \ L^{-1})$ $0.55$ $0.31$ $0.17$ $0.085$

What will be the average rate of reaction between the time interval $30 \ s$ to $60 \ s$?