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

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(D) The rate expression for the given reaction $2 \ NO_{(g)} + O_{2_{(g)}} \rightarrow 2 \ NO_{2_{(g)}}$ is given by: $-\frac{1}{2} \frac{d[NO]}{dt} = \frac{1}{2} \frac{d[NO_2]}{dt}$. The rate of consumption of $NO_{(g)}$ is defined as $-\frac{d[NO]}{dt}$. From the expression,$-\frac{d[NO]}{dt} = \frac{d[NO_2]}{dt}$. Given that $\frac{d[NO_2]}{dt} = 0.052 \ mol \ dm^{-3} \ s^{-1}$,Therefore,$-\frac{d[NO]}{dt} = 0.052 \ mol \ dm^{-3} \ s^{-1}$.

Class 12 Chemistry Chemical Kinetics Rate of a reaction

Easy

For the reaction,$2 \ NO_{(g)} + O_{2_{(g)}} \rightarrow 2 \ NO_{2_{(g)}}$. If $\frac{d[NO_2]}{dt} = 0.052 \ mol \ dm^{-3} \ s^{-1}$,calculate the rate of consumption of $NO_{(g)}$.

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A
$0.114 \ mol \ dm^{-3} \ s^{-1}$
B
$0.078 \ mol \ dm^{-3} \ s^{-1}$
C
$0.026 \ mol \ dm^{-3} \ s^{-1}$
D
$0.052 \ mol \ dm^{-3} \ s^{-1}$

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For the chemical reaction: $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the rate of reaction can be expressed in terms of the concentration of $N_{2(g)}$,$H_{2(g)}$,or $NH_{3(g)}$ with respect to time. Identify the correct relationship between these rates.

Medium

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Write the rate equation for the following reactions:
$1.$ $2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
$2.$ $2 HI_{(g)} \rightarrow H_{2(g)} + I_{2(g)}$

Medium

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In a reaction $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$,the rate of appearance of $NH_3$ is $2.5 \times 10^{-4} \ mol \ L^{-1} s^{-1}$. The rate of reaction and rate of disappearance of $H_2$ will be (in $mol \ L^{-1} s^{-1}$):

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In a reaction,$n_1 A + n_2 B \rightarrow m_1 C + m_2 D$,$5 \ M$ solution of reactant $A$ is allowed to react with $3 \ M$ solution of reactant $B$. After $5 \ s$,the concentration of $A$ was found to be $4 \ M$. The rate of decomposition of $A$ and the rate of formation of $D$ are respectively $:-$

Medium

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For the reaction $2A + B \rightarrow 3C + D$,which of the following options does not represent the correct rate of the reaction?

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For the reaction,$2 \ NO_{(g)} + O_{2_{(g)}} \rightarrow 2 \ NO_{2_{(g)}}$. If $\frac{d[NO_2]}{dt} = 0.052 \ mol \ dm^{-3} \ s^{-1}$,calculate the rate of consumption of $NO_{(g)}$.

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For the chemical reaction: $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the rate of reaction can be expressed in terms of the concentration of $N_{2(g)}$,$H_{2(g)}$,or $NH_{3(g)}$ with respect to time. Identify the correct relationship between these rates.

Write the rate equation for the following reactions:$1.$ $2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$$2.$ $2 HI_{(g)} \rightarrow H_{2(g)} + I_{2(g)}$

In a reaction $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$,the rate of appearance of $NH_3$ is $2.5 \times 10^{-4} \ mol \ L^{-1} s^{-1}$. The rate of reaction and rate of disappearance of $H_2$ will be (in $mol \ L^{-1} s^{-1}$):

In a reaction,$n_1 A + n_2 B \rightarrow m_1 C + m_2 D$,$5 \ M$ solution of reactant $A$ is allowed to react with $3 \ M$ solution of reactant $B$. After $5 \ s$,the concentration of $A$ was found to be $4 \ M$. The rate of decomposition of $A$ and the rate of formation of $D$ are respectively $:-$

For the reaction $2A + B \rightarrow 3C + D$,which of the following options does not represent the correct rate of the reaction?

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Write the rate equation for the following reactions:
$1.$ $2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
$2.$ $2 HI_{(g)} \rightarrow H_{2(g)} + I_{2(g)}$