AP EAMCET · Chemistry · Chemical Kinetics
The rate constant, k of a zero order reaction \(2 \mathrm{NH}_3(\mathrm{~g})\) \(\underset{1130 \mathrm{~K}}{\stackrel{\mathrm{Pt}}{\longrightarrow}} \mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g})\) is \(\mathrm{y} \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\). The rate of formation of hydrogen (in \(\mathrm{mol} \mathrm{L}^{-1} \mathrm{~s}^{-1}\) ) is
- A \(\mathrm{y} \times 10^{-4}\)
- B \(2 y \times 10^{-4}\)
- C \(3 y \times 10^{-4}\)
- D \(\frac{y}{3} \times 10^{-4}\)
Answer & Solution
Correct Answer
(C) \(3 y \times 10^{-4}\)
Step-by-step Solution
Detailed explanation
\(\mathrm{r}=\mathrm{K}\left[\mathrm{NH}_3\right]^{\circ}=\mathrm{K}=\mathrm{y} \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\) Now,…
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