(D) For the reaction $2 \ A \rightarrow 4 \ B + C$,the rate expression is given by: $-\frac{1}{2} \frac{d[A]}{dt} = \frac{1}{4} \frac{d[B]}{dt}$.We ne

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(D) For the reaction $2 \ A \rightarrow 4 \ B + C$,the rate expression is given by: $-\frac{1}{2} \frac{d[A]}{dt} = \frac{1}{4} \frac{d[B]}{dt}$.We need to find the rate of disappearance of $A$,which is $-\frac{d[A]}{dt}$.From the expression: $-\frac{d[A]}{dt} = \frac{2}{4} \frac{d[B]}{dt} = \frac{1}{2} \frac{d[B]}{dt}$.Given $\frac{\Delta [B]}{\Delta t} = \frac{5 \times 10^{-3} \ mol \ L^{-1}}{10 \ s} = 5 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$.Therefore,$-\frac{d[A]}{dt} = \frac{1}{2} \times (5 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}) = 2.5 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$.

Class 12 Chemistry Chemical Kinetics Rate of a reaction

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Consider a gas phase reaction which occurs in a closed vessel: $2 \ A \rightarrow 4 \ B + C$. The concentration of $B$ is found to be increased by $5 \times 10^{-3} \ mol \ L^{-1}$ in $10 \ s$. The rate of disappearance of $A$ (in $mol \ L^{-1} \ s^{-1}$) is:

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A
$4.75 \times 10^{-4}$
B
$7.5 \times 10^{-4}$
C
$1.25 \times 10^{-4}$
D
$2.5 \times 10^{-4}$

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Chemical Kinetics

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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 $mol \ L^{-1} \ min^{-1}$)?

EasyTS EAMCET 2005

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For the decomposition reaction $N_2O_{4(g)} \rightarrow 2NO_{2(g)}$,the initial pressure of $N_2O_4$ decreases from $0.46 \ atm$ to $0.28 \ atm$ in $30 \ minutes$. What is the rate of formation of $NO_2$?

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The instantaneous rate of disappearance of $MnO_4^-$ ion in the following reaction is $4.56 \times 10^{-3} \ M s^{-1}$.
$2MnO_4^- + 10I^{-} + 16H^{+} \to 2Mn^{2+} + 5I_2 + 8H_2O$
The rate of appearance of $I_2$ is $...... \times 10^{-2} \ M s^{-1}$.

DifficultJEE MAIN 2013

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$5 Br^{-}_{(aq)} + BrO^{-}_{3(aq)} + 6 H^{+}_{(aq)} \rightarrow 3 Br_{2(aq)} + 3 H_{2}O_{(l)}$
The rate of consumption of $H^{+}$ is $x \ mol \ L^{-1} \ s^{-1}$.
$(a)$ What is the rate of consumption of $Br^{-}$?
$(b)$ What is the rate of formation of $Br_{2}$?

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In a gaseous reaction $A_{2(g)} \longrightarrow B_{(g)} + \frac{1}{2} C_{(g)}$,the increase in pressure from $100 \text{ mm}$ to $120 \text{ mm}$ is noticed in $5 \text{ min}$. The rate of disappearance of $A_2$ in $\text{mm min}^{-1}$ is

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Consider a gas phase reaction which occurs in a closed vessel: $2 \ A \rightarrow 4 \ B + C$. The concentration of $B$ is found to be increased by $5 \times 10^{-3} \ mol \ L^{-1}$ in $10 \ s$. The rate of disappearance of $A$ (in $mol \ L^{-1} \ s^{-1}$) is:

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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 $mol \ L^{-1} \ min^{-1}$)?

For the decomposition reaction $N_2O_{4(g)} \rightarrow 2NO_{2(g)}$,the initial pressure of $N_2O_4$ decreases from $0.46 \ atm$ to $0.28 \ atm$ in $30 \ minutes$. What is the rate of formation of $NO_2$?

The instantaneous rate of disappearance of $MnO_4^-$ ion in the following reaction is $4.56 \times 10^{-3} \ M s^{-1}$.$2MnO_4^- + 10I^{-} + 16H^{+} \to 2Mn^{2+} + 5I_2 + 8H_2O$The rate of appearance of $I_2$ is $...... \times 10^{-2} \ M s^{-1}$.

$5 Br^{-}_{(aq)} + BrO^{-}_{3(aq)} + 6 H^{+}_{(aq)} \rightarrow 3 Br_{2(aq)} + 3 H_{2}O_{(l)}$The rate of consumption of $H^{+}$ is $x \ mol \ L^{-1} \ s^{-1}$.$(a)$ What is the rate of consumption of $Br^{-}$?$(b)$ What is the rate of formation of $Br_{2}$?

In a gaseous reaction $A_{2(g)} \longrightarrow B_{(g)} + \frac{1}{2} C_{(g)}$,the increase in pressure from $100 \text{ mm}$ to $120 \text{ mm}$ is noticed in $5 \text{ min}$. The rate of disappearance of $A_2$ in $\text{mm min}^{-1}$ is

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The instantaneous rate of disappearance of $MnO_4^-$ ion in the following reaction is $4.56 \times 10^{-3} \ M s^{-1}$.
$2MnO_4^- + 10I^{-} + 16H^{+} \to 2Mn^{2+} + 5I_2 + 8H_2O$
The rate of appearance of $I_2$ is $...... \times 10^{-2} \ M s^{-1}$.

$5 Br^{-}_{(aq)} + BrO^{-}_{3(aq)} + 6 H^{+}_{(aq)} \rightarrow 3 Br_{2(aq)} + 3 H_{2}O_{(l)}$
The rate of consumption of $H^{+}$ is $x \ mol \ L^{-1} \ s^{-1}$.
$(a)$ What is the rate of consumption of $Br^{-}$?
$(b)$ What is the rate of formation of $Br_{2}$?