AP EAMCET · Chemistry · Chemical Kinetics
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.
- A \(0.02\)
- B \(50\)
- C \(0.06\)
- D \(0.04\)
Answer & Solution
Correct Answer
(C) \(0.06\)
Step-by-step Solution
Detailed explanation
\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…
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