(C) For the reaction $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$,the rate of reaction is given by: Rate $= -\frac{d[N_2]}{dt} = -\frac{1}{3} \fr

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(C) For the reaction $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$,the rate of reaction is given by: Rate $= -\frac{d[N_2]}{dt} = -\frac{1}{3} \frac{d[H_2]}{dt} = \frac{1}{2} \frac{d[NH_3]}{dt}$. Given that $-\frac{d[N_2]}{dt} = 0.02 \ mol \ L^{-1} \ s^{-1}$. Equating the terms for $N_2$ and $H_2$: $-\frac{d[N_2]}{dt} = -\frac{1}{3} \frac{d[H_2]}{dt}$. Therefore,$-\frac{d[H_2]}{dt} = 3 \times (-\frac{d[N_2]}{dt})$. $-\frac{d[H_2]}{dt} = 3 \times 0.02 = 0.06 \ mol \ L^{-1} \ s^{-1}$.

Class 12 Chemistry Chemical Kinetics Rate of a reaction

Medium

Consider the following reaction: $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$. The rate of this reaction in terms of $N_2$ at $T \ K$ is $\frac{-d[N_2]}{dt} = 0.02 \ mol \ L^{-1} \ s^{-1}$. What is the value of $\frac{-d[H_2]}{dt}$ (in units of $mol \ L^{-1} \ s^{-1}$) at the same temperature?

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A
$0.02$
B
$50$
C
$0.06$
D
$0.04$

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Consider the following reaction: $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$. The rate of this reaction in terms of $N_2$ at $T \ K$ is $\frac{-d[N_2]}{dt} = 0.02 \ mol \ L^{-1} \ s^{-1}$. What is the value of $\frac{-d[H_2]}{dt}$ (in units of $mol \ L^{-1} \ s^{-1}$) at the same temperature?

Similar Questions

For the reaction $N_2 + 3H_2 \to 2NH_3$,if $\frac{\Delta [NH_3]}{\Delta t} = 2 \times 10^{-4} \ mol \ L^{-1} s^{-1}$,the value of $\frac{-\Delta [H_2]}{\Delta t}$ would be

For the reaction $H_2 + I_2 \rightarrow 2HI$,state the correct differential rate law.

For the reaction,$CH_3Br_{(aq)} + OH_{(aq)}^{-} \longrightarrow CH_3OH_{(aq)} + Br_{(aq)}^{-}$,the rate of consumption of $OH_{(aq)}^{-}$ is $x \ mol \ dm^{-3} \ s^{-1}$. What is the rate of formation of $Br_{(aq)}^{-}$ (in $mol \ dm^{-3} \ s^{-1}$)?

The concentration of a reactant changes from $0.1 \, mol \, L^{-1}$ to $0.095 \, mol \, L^{-1}$ in $10 \, s$. Calculate the rate of reaction.

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