The decomposition of NH_3 on platinum surface,2NH_ 3 (g) ^ Pt _ _ 2 (g)+3H_ 2 (g) is a zero order reaction with k=2.5 10^ -4 Ms^ -1 . what are the rates of production of N_2 and H_2?

2NH_ 3 (g) ^ Pt _ N_ 2 (g)+3H_ 2 (g) -d[NH_ 3 ] dt =k[NH_ 3 ]^ o =2.5 10^ -4 Ms^ -1 - 1 2 d[NH_ 3 ] dt =+ d[N_ 2 ] dt =+ 1 3 d[H_ 2 ] dt Rate of Production of N_2=+ d[N_ 2 ] dt =- 1 2 d[NH_ 3 ] dt = 1 2 (2.5 10^ -4 Ms^ -1 )=1.25 10^ -4 Ms^ -1 Rate of production of hydrogen= d[H_ 2 ] dt =- 3 2 d[NH_ 3 ] dt = 3 2 (2.5 10^ -4 Ms^ -1 ) =3.75 10^ -4 Ms^ -1

The decomposition of NH_3 on platinum surface,2NH_ 3 (g) ^ Pt _ _…

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The decomposition of $NH_3$ on platinum surface,$\text{2NH}_{3}\text{(g)}\text{ }^{Pt}_\rightarrow\text{N}_{2}\text{(g)}+\text{3H}_{2}\text{(g)}$ is a zero order reaction with k$=\text{2.5}\times\text{10}^{-4}\text{Ms}^{-1}$ . what are the rates of production of $N_2$ and $H_2?$

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Answer

$\text{2NH}_{3}\text{(g)}\text{ }^{Pt}_\rightarrow\text{ N}_{2}\text{(g)}+\text{3H}_{2}\text{(g)}$$\frac{\text{-d[NH}_{3}]}{\text{dt}}=\text{k[NH}_{3}]^{o}=\text{2.5}\times\text{10}^{-4}\text{Ms}^{-1}$
$-\frac{\text{1}}{\text{2}}\frac{\text{d[NH}_{3}]}{\text{dt}}=+\frac{\text{d[N}_{2}]}{\text{dt}}=+\frac{\text{1}}{\text{3}}\frac{\text{d[H}_{2}]}{\text{dt}}$
Rate of Production of $N_2=+\frac{\text{d[N}_{2}]}{\text{dt}}=-\frac{\text{1}}{\text{2}}\frac{\text{d[NH}_{3}]}{\text{dt}}$
$=\frac{\text{1}}{\text{2}}\times\text{(2.5}\times\text{10}^{-4}\text{Ms}^{-1})=\text{1.25}\times\text{10}^{-4}\text{Ms}^{-1}$
Rate of production of hydrogen$= \frac{\text{d[H}_{2}]}{\text{dt}}=-\frac{\text{3}}{\text{2}}\frac{\text{d[NH}_{3}]}{\text{dt}}$
$=\frac{\text{3}}{\text{2}}\times\text{(2.5}\times\text{10}^{-4}\text{ Ms}^{-1})$
$=3.75\times10^{-4}\ Ms^{-1}$

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