(B) The rate of formation of $NH_3$ is given by: $\frac{d[NH_3]}{dt} = \frac{\Delta [NH_3]}{\Delta t} = \frac{0.04 \ M - 0.01 \ M}{20 \ s} = \frac{0.0

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$0.75 \times 10^{-3} \ M \ sec^{-1}$

(B) The rate of formation of $NH_3$ is given by: $\frac{d[NH_3]}{dt} = \frac{\Delta [NH_3]}{\Delta t} = \frac{0.04 \ M - 0.01 \ M}{20 \ s} = \frac{0.03 \ M}{20 \ s} = 1.5 \times 10^{-3} \ M \ s^{-1}$.For the reaction $N_2 + 3H_2 \to 2NH_3$,the rate of reaction $(r)$ is defined as: $r = \frac{1}{2} \frac{d[NH_3]}{dt}$.Substituting the value: $r = \frac{1}{2} \times 1.5 \times 10^{-3} \ M \ s^{-1} = 0.75 \times 10^{-3} \ M \ s^{-1}$.

Class 12 Chemistry Chemical Kinetics Rate of a reaction

Medium

$N_2 + 3H_2 \to 2NH_3$. If the concentration of $NH_3$ changes from $0.01 \ M$ to $0.04 \ M$ in $20 \ seconds$,then the rate of reaction will be:

A
$1.5 \times 10^{-3} \ M \ sec^{-1}$
B
$0.75 \times 10^{-3} \ M \ sec^{-1}$
C
$2 \times 10^{-3} \ M \ sec^{-1}$
D
$3 \times 10^{-3} \ M \ sec^{-1}$

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Chemical Kinetics

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Rate of a reaction

Write the following equations for the reaction $R \to P$: $(i)$ Average rate $(ii)$ Instantaneous rate.

Easy

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Find the rate of the following reaction: $2 \ N_2O_{5(g)} \rightarrow 4 \ NO_{2(g)} + O_{2(g)}$ if the concentration of $NO_2$ increases to $5.2 \times 10^{-3} \ M$ in $100 \ s$.

MediumMHT CET 2025

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For the reaction $2SO_2 + O_2 \to 2SO_3$,the rate of disappearance of $O_2$ is $2.0 \times 10^{-4} \ mol \ L^{-1}s^{-1}$. The rate of appearance of $SO_3$ is:

Medium

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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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For a reaction,$2A + B \rightarrow 2C$,the rate of disappearance of $A$ is $0.076 \ mol \ dm^{-3} \ s^{-1}$. What is the rate of disappearance of $B$?

MediumMHT CET 2022

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$N_2 + 3H_2 \to 2NH_3$. If the concentration of $NH_3$ changes from $0.01 \ M$ to $0.04 \ M$ in $20 \ seconds$,then the rate of reaction will be:

Similar Questions

Write the following equations for the reaction $R \to P$: $(i)$ Average rate $(ii)$ Instantaneous rate.

Find the rate of the following reaction: $2 \ N_2O_{5(g)} \rightarrow 4 \ NO_{2(g)} + O_{2(g)}$ if the concentration of $NO_2$ increases to $5.2 \times 10^{-3} \ M$ in $100 \ s$.

For the reaction $2SO_2 + O_2 \to 2SO_3$,the rate of disappearance of $O_2$ is $2.0 \times 10^{-4} \ mol \ L^{-1}s^{-1}$. The rate of appearance of $SO_3$ is:

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 $...... \times 10^{-2} \ M s^{-1}$.

For a reaction,$2A + B \rightarrow 2C$,the rate of disappearance of $A$ is $0.076 \ mol \ dm^{-3} \ s^{-1}$. What is the rate of disappearance of $B$?

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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 $...... \times 10^{-2} \ M s^{-1}$.