Consider the following reaction $\mathrm{N}_2(g)+3 \mathrm{H}_2(g) \longrightarrow 2 \mathrm{NH}_3(g)$ The…

Consider the following reaction $\mathrm{N}_2(g)+3 \mathrm{H}_2(g) \longrightarrow 2 \mathrm{NH}_3(g)$ The rate of this reaction in terms of $\mathrm{N}_2$ at $T \mathrm{~K}$ is $\frac{-d\left[\mathrm{~N}_2\right]}{d t}=0.02 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$. What is the value of $-d\left[\mathrm{H}_2\right] / d t$ (in units of $\mathrm{mol} \mathrm{L}^{-1} \mathrm{~s}^{-1}$ ) at the same temperature.
  1. $0.02$
  2. $50$
  3. $0.06$
  4. $0.04$

Solution

$\begin{aligned} \frac{-d\left[\mathrm{~N}_2\right]}{d t} & =-\frac{1}{3} \frac{d\left[\mathrm{H}_2\right]}{d t} \\ \frac{-3 d\left[\mathrm{~N}_2\right]}{d t} & =\frac{-d\left[\mathrm{H}_2\right]}{d t} \\ 3 \times 0.02 & =\frac{d\left[\mathrm{H}_2\right]}{d t} \\ \therefore \frac{d\left[\mathrm{H}_2\right]}{d t} & =0.06 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\end{aligned}$

Asked in: TEST SERIES MHT-CET Full Test 6

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