(D) For the reaction: $4 NH_{3(g)} + 5 O_{2(g)} \longrightarrow 4 NO_{(g)} + 6 H_2 O_{(g)}$The rate of reaction is given by the expression:$Rate = -\f

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(D) For the reaction: $4 NH_{3(g)} + 5 O_{2(g)} \longrightarrow 4 NO_{(g)} + 6 H_2 O_{(g)}$The rate of reaction is given by the expression:$Rate = -\frac{1}{4} \frac{d[NH_3]}{dt} = -\frac{1}{5} \frac{d[O_2]}{dt} = \frac{1}{4} \frac{d[NO]}{dt} = \frac{1}{6} \frac{d[H_2O]}{dt}$Given that the rate of formation of $NO$ is $\frac{d[NO]}{dt} = 3.6 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$.From the rate expression,we have:$-\frac{1}{4} \frac{d[NH_3]}{dt} = \frac{1}{4} \frac{d[NO]}{dt}$Therefore,the rate of disappearance of $NH_3$ is:$-\frac{d[NH_3]}{dt} = \frac{d[NO]}{dt} = 3.6 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$.

Class 12 Chemistry Chemical Kinetics Rate of a reaction

Medium

Ammonia and oxygen react at high temperature as $4 NH_{3(g)} + 5 O_{2(g)} \longrightarrow 4 NO_{(g)} + 6 H_2 O_{(g)}$. If the rate of formation of $NO_{(g)}$ is $3.6 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$,then the rate of disappearance of ammonia is:

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A
$7.2 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$
B
$1.2 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$
C
$2.4 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$
D
$3.6 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$

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In the reaction $2N_2O_5(g) \rightarrow 4 NO_2(g) + O_2(g)$, $N_2O_5$ disappears at a rate of $0.06 \text{ mol dm}^{-3} \text{s}^{-1}$. Calculate the rate of formation of $O_2(g)$.

DifficultMHT CET 2026

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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 $I_{3_{(aq)}}^{-}$?

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Ammonia and oxygen react at high temperature as $4 NH_{3(g)} + 5 O_{2(g)} \longrightarrow 4 NO_{(g)} + 6 H_2 O_{(g)}$. If the rate of formation of $NO_{(g)}$ is $3.6 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$,then the rate of disappearance of ammonia is:

Similar Questions

For the reaction,$3 I^{-} + S_2 O_8^{2-} \rightarrow I_3^{-} + 2 SO_4^{2-}$,at a particular time $t$,$\frac{d[SO_4^{2-}]}{dt}$ is $2.2 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$. What is the value of $-\frac{d[I^{-}]}{dt}$?

$A \rightarrow B$ is a first order reaction. The concentration of $A$ is decreased from $x \ mol \ L^{-1}$ to $y \ mol \ L^{-1}$ in $100 \ \min$. What is the average velocity of the reaction in $mol \ L^{-1} \ \min^{-1}$?

In the reaction $2N_2O_5(g) \rightarrow 4 NO_2(g) + O_2(g)$, $N_2O_5$ disappears at a rate of $0.06 \text{ mol dm}^{-3} \text{s}^{-1}$. Calculate the rate of formation of $O_2(g)$.

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 $I_{3_{(aq)}}^{-}$?

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