(A) The rate expression for the reaction $2 NO_{(g)} + O_{2(g)} \rightarrow 2 NO_{2(g)}$ is given by: $-\frac{1}{2} \frac{d[NO]}{dt} = -\frac{d[O_2]}{

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(A) The rate expression for the reaction $2 NO_{(g)} + O_{2(g)} \rightarrow 2 NO_{2(g)}$ is given by: $-\frac{1}{2} \frac{d[NO]}{dt} = -\frac{d[O_2]}{dt} = \frac{1}{2} \frac{d[NO_2]}{dt}$ Given that the rate of formation of $NO_2$ is $\frac{d[NO_2]}{dt} = 0.052 \ mol \ dm^{-3} \ s^{-1}$. Equating the rate of disappearance of $O_2$ to the rate of formation of $NO_2$: $-\frac{d[O_2]}{dt} = \frac{1}{2} \times \frac{d[NO_2]}{dt}$ $-\frac{d[O_2]}{dt} = \frac{1}{2} \times 0.052 \ mol \ dm^{-3} \ s^{-1} = 0.026 \ mol \ dm^{-3} \ s^{-1}$.

Class 12 Chemistry Chemical Kinetics Rate of a reaction

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For the reaction $2 NO_{(g)} + O_{2(g)} \rightarrow 2 NO_{2(g)}$,the rate of formation of $NO_2$ is $\frac{d[NO_2]}{dt} = 0.052 \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate of disappearance of $O_2$,i.e.,$-\frac{d[O_2]}{dt}$.

MHT CET 2022 All MHT CET

A
$0.026$
B
$0.052$
C
$0.078$
D
$0.114$

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The following results are obtained in the hydrolysis of chlorobutane $(C_4H_9Cl)$:

Time $(s)$ $0$ $100$ $200$ $300$ $400$ $700$ $800$

$[C_4H_9Cl]$ $(mol \, L^{-1})$ $0.100$ $0.082$ $0.067$ $0.055$ $0.044$ $0.021$ $0.017$

Calculate the average rate $r_{av}$ of the reaction during different time intervals.

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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 $7.2 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$?

EasyAP EAMCET 2020

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Consider the graph given in the following diagram. Which of the following options does not show the instantaneous rate of reaction at the $40^{th}$ second?

Medium

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For the reaction $R \rightarrow P$,the concentration of a reactant changes from $0.03 \, M$ to $0.02 \, M$ in $25 \, minutes$. Calculate the average rate of reaction using units of time both in $minutes$ and $seconds$.

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Time $(s)$	$0$	$100$	$200$	$300$	$400$	$700$	$800$
$[C_4H_9Cl]$ $(mol \, L^{-1})$	$0.100$	$0.082$	$0.067$	$0.055$	$0.044$	$0.021$	$0.017$

For the reaction $2 NO_{(g)} + O_{2(g)} \rightarrow 2 NO_{2(g)}$,the rate of formation of $NO_2$ is $\frac{d[NO_2]}{dt} = 0.052 \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate of disappearance of $O_2$,i.e.,$-\frac{d[O_2]}{dt}$.

Similar Questions

$A$ 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 $7.2 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$?

Consider the graph given in the following diagram. Which of the following options does not show the instantaneous rate of reaction at the $40^{th}$ second?

Explain the difference between instantaneous rate of a reaction and average rate of a reaction.

For the reaction $R \rightarrow P$,the concentration of a reactant changes from $0.03 \, M$ to $0.02 \, M$ in $25 \, minutes$. Calculate the average rate of reaction using units of time both in $minutes$ and $seconds$.

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