(B) The rate of reaction is given by the expression: $-\frac{1}{3} \frac{d[X]}{dt} = \frac{1}{2} \frac{d[Y]}{dt} = \frac{d[Z]}{dt}$ Given that the rat

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(B) The rate of reaction is given by the expression: $-\frac{1}{3} \frac{d[X]}{dt} = \frac{1}{2} \frac{d[Y]}{dt} = \frac{d[Z]}{dt}$ Given that the rate of disappearance of $X$ is $-\frac{d[X]}{dt} = 7.2 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$. From the rate expression,we have: $\frac{1}{2} \frac{d[Y]}{dt} = -\frac{1}{3} \frac{d[X]}{dt}$ Therefore,the rate of formation of $Y$ is: $\frac{d[Y]}{dt} = \frac{2}{3} \times (-\frac{d[X]}{dt}) = \frac{2}{3} \times 7.2 \times 10^{-3} = 4.8 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$.

Class 12 Chemistry Chemical Kinetics Rate of a reaction

Easy

$A$ reaction,$3 X_{(g)} \rightarrow 2 Y_{(g)} + Z_{(g)}$ takes place in a closed vessel. What is the rate of formation of $Y$ (in $mol \ L^{-1} \ s^{-1}$) if the rate of disappearance of $X$ is $7.2 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$?

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A
$3.6 \times 10^{-3}$
B
$4.8 \times 10^{-3}$
C
$2.4 \times 10^{-3}$
D
$1.2 \times 10^{-3}$

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The differential rate law for the reaction $H_2 + I_2 \to 2HI$ is

MediumAIEEE 2002

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For the reaction,$3 I_{(aq)}^{-} + S_2 O_{8_{(aq)}}^{2-} \longrightarrow 2 SO_{4_{(aq)}}^{2-} + I_{3_{(aq)}}^{-}$,the rate of formation of $SO_{4_{(aq)}}^{2-}$ is $0.044 \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate of consumption of $I_{(aq)}^{-}$.

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$A \rightarrow P$ is a first-order reaction. The following graph is obtained for this reaction ($x$-axis $=$ time,$y$-axis $=$ concentration of $A$). The instantaneous rate of the reaction at point $C$ is:

MediumAP EAMCET 2021

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For the reaction,$3 I_{(aq)}^{-} + S_2 O_{8_{(aq)}}^{2-} \longrightarrow I_{3_{(aq)}}^{-} + 2 SO_{4_{(aq)}}^{2-}$,the rate of formation of $SO_4^{2-}$ is $0.022 \ mol \ dm^{-3} \ sec^{-1}$. What is the rate of formation of $I_{3_{(aq)}}^{-}$?

MediumMHT CET 2021

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For the reaction,$2N_2O_{5(g)} \rightarrow 4NO_{2(g)} + O_{2(g)}$,the rate of formation of $O_2$ is $0.032 \ g \ h^{-1}$. What is the rate of conversion of $N_2O_5$ in $g \ h^{-1}$?

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$A$ reaction,$3 X_{(g)} \rightarrow 2 Y_{(g)} + Z_{(g)}$ takes place in a closed vessel. What is the rate of formation of $Y$ (in $mol \ L^{-1} \ s^{-1}$) if the rate of disappearance of $X$ is $7.2 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$?

Similar Questions

The differential rate law for the reaction $H_2 + I_2 \to 2HI$ is

For the reaction,$3 I_{(aq)}^{-} + S_2 O_{8_{(aq)}}^{2-} \longrightarrow 2 SO_{4_{(aq)}}^{2-} + I_{3_{(aq)}}^{-}$,the rate of formation of $SO_{4_{(aq)}}^{2-}$ is $0.044 \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate of consumption of $I_{(aq)}^{-}$.

$A \rightarrow P$ is a first-order reaction. The following graph is obtained for this reaction ($x$-axis $=$ time,$y$-axis $=$ concentration of $A$). The instantaneous rate of the reaction at point $C$ is:

For the reaction,$3 I_{(aq)}^{-} + S_2 O_{8_{(aq)}}^{2-} \longrightarrow I_{3_{(aq)}}^{-} + 2 SO_{4_{(aq)}}^{2-}$,the rate of formation of $SO_4^{2-}$ is $0.022 \ mol \ dm^{-3} \ sec^{-1}$. What is the rate of formation of $I_{3_{(aq)}}^{-}$?

For the reaction,$2N_2O_{5(g)} \rightarrow 4NO_{2(g)} + O_{2(g)}$,the rate of formation of $O_2$ is $0.032 \ g \ h^{-1}$. What is the rate of conversion of $N_2O_5$ in $g \ h^{-1}$?

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