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Characteristics of Equilibrium Constant

If K C =7.5...

Question

If $K_{C} = 7.5 \times 10^{- 9}$ at $1000 K$ for the reaction $N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)$ . what is $K_{C}$ at $1000 K$ for the reaction $2 N O (g) ⇌ N_{2} (g) + O_{2} (g)$ ?

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Solution

${N_{2}}_{(g)} + {O_{2}}_{(g)} ⇌ 2 {N O}_{(g)}$
$K_{C} = \frac{{[N O]}^{2}}{[N_{2}] [O_{2}]} = 7.5 10^{- 9} (Given)$
$2 N O ⇌ {N_{2}}_{(g)} + {O_{2}}_{(g)}$
${K_{C}}^{'} = \frac{[N_{2}] [O_{2}]}{{[N O]}^{2}}$
${K_{C}}^{'} = \frac{1}{(\frac{{[N O]}^{2}}{[N_{2}] [O_{2}]})}$
${K_{C}}^{'} = \frac{1}{K_{C}} = \frac{1}{7.5 \times 10^{- 9}} = 1.3 \times 10^{8}$
Hence the required answer is $1.3 \times 10^{8}$ .

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For the reaction, $N_{2} (g) + O_{2} (g) ⇌ 2 NO (g)$ , equilibrium constant is $K_{c} = 2$ .

Degree of association is:

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