(D) The rate of reaction is given by the expression:$\text{Rate} = -\frac{1}{2} \frac{d[N_2 O_5]}{dt} = +\frac{1}{4} \frac{d[NO_2]}{dt} = \frac{d[O_2]

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$0.04 \ mol \ dm^{-3} \ s^{-1}$

(D) The rate of reaction is given by the expression:$\text{Rate} = -\frac{1}{2} \frac{d[N_2 O_5]}{dt} = +\frac{1}{4} \frac{d[NO_2]}{dt} = \frac{d[O_2]}{dt}$We are given that $-\frac{d[N_2 O_5]}{dt} = 0.02 \ mol \ dm^{-3} \ s^{-1}$.To find the rate of formation of $NO_2$,we use the relation:$\frac{1}{4} \frac{d[NO_2]}{dt} = -\frac{1}{2} \frac{d[N_2 O_5]}{dt}$$\frac{d[NO_2]}{dt} = 2 \times \left( -\frac{d[N_2 O_5]}{dt} \right)$$\frac{d[NO_2]}{dt} = 2 \times 0.02 \ mol \ dm^{-3} \ s^{-1} = 0.04 \ mol \ dm^{-3} \ s^{-1}$

Class 12 Chemistry Chemical Kinetics Rate of a reaction

Easy

Find the rate of formation of $NO_{2(g)}$ in the following reaction.
$2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
$\left[ \frac{-d[N_2 O_5]}{dt} = 0.02 \ mol \ dm^{-3} \ s^{-1} \right]$

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A
$0.01 \ mol \ dm^{-3} \ s^{-1}$
B
$0.02 \ mol \ dm^{-3} \ s^{-1}$
C
$0.03 \ mol \ dm^{-3} \ s^{-1}$
D
$0.04 \ mol \ dm^{-3} \ s^{-1}$

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For the chemical reaction $N_2 + 3H_2 \rightarrow 2NH_3$,the rate of reaction can be expressed in terms of the derivatives of the concentrations of $N_2$,$H_2$,or $NH_3$. Write the correct relationship between the rate expressions.

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For the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,the rate of reaction is expressed as:

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For the reaction $N_{2}O_{5(g)} \rightarrow 2NO_{2(g)} + \frac{1}{2} O_{2(g)}$,the rate of disappearance of $N_{2}O_{5}$ is given as $6.25 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$. The rate of formation of $NO_{2}$ and $O_{2}$ is given respectively as:

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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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$A$ 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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Find the rate of formation of $NO_{2(g)}$ in the following reaction.$2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$$\left[ \frac{-d[N_2 O_5]}{dt} = 0.02 \ mol \ dm^{-3} \ s^{-1} \right]$

Similar Questions

For the chemical reaction $N_2 + 3H_2 \rightarrow 2NH_3$,the rate of reaction can be expressed in terms of the derivatives of the concentrations of $N_2$,$H_2$,or $NH_3$. Write the correct relationship between the rate expressions.

For the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,the rate of reaction is expressed as:

For the reaction $N_{2}O_{5(g)} \rightarrow 2NO_{2(g)} + \frac{1}{2} O_{2(g)}$,the rate of disappearance of $N_{2}O_{5}$ is given as $6.25 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$. The rate of formation of $NO_{2}$ and $O_{2}$ is given respectively as:

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?

$A$ 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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Find the rate of formation of $NO_{2(g)}$ in the following reaction.
$2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
$\left[ \frac{-d[N_2 O_5]}{dt} = 0.02 \ mol \ dm^{-3} \ s^{-1} \right]$