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Dalton's Law of Partial Pressures

n mole each o...

Question

$n$ mole each of $H_{2} O (g), H_{2} (g)$ and mixed at a suitable high temperature to attain the equilibrium $2 H_{2} O (g) ⇌ 2 H_{2} (g) + O_{2} (g)$ . If $y$ mole of $H_{2} O (g)$ are the dissociated and the total pressure maintained is $P$ , calculate the $K_{P}$ .

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Solution

$2 H_{2} O ⟶ 2 H_{2} + O_{2}$
$n$ $n$ $0$ at $t = 0$
$(n - y)$ $(n + y)$ $\frac{y}{2}$ at $t = t s e c$
Total moles at equilibrium = $2 n + \frac{y}{2}$

So $K_{p}$ = $P \times \frac{{\frac{n + y}{2 n + \frac{y}{2}}}^{2} \times \frac{\frac{y}{2}}{2 n + \frac{y}{2}}}{{\frac{n - y}{2 n + \frac{y}{2}}}^{2}}$

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