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What is the equilibrium constant expression for the reaction?
$P_{4} (s) + 5 O_{2} (g) ⇌ P_{4} O_{10} (s) ?$

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K_{C} = \frac{[P_{4} O_{10}]}{[P_{4}] {[O_{2}]}^{5}}

K_{C} = \frac{1}{{[O_{2}]}^{5}}

K_{C} = {[O_{2}]}^{5}

K_{C} = \frac{[P_{4} O_{10}]}{5 [P_{4}] [O_{2}]}

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detailed solution

Correct option is B

$P_{4} (s) + 5 O_{2} (g) \overset{k_{c}}{⇌} P_{4} O_{10} (g)$

As we know, during. writing equilibrium expression, concentration of pure solid and liquid are taken as unity.

So,

$[P_{4}] = 1, [P_{4} O_{10}] = 1$

$\Rightarrow K_{c} = \frac{[P_{4} O_{10}]}{[P_{4}] {[O_{2}]}^{5}}$

$= \frac{1}{1 {[O_{2}]}^{5}}$

$K_{c} = \frac{1}{{[O_{2}]}^{5}}$

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What is the equilibrium constant expression for the reaction?P4(s)+5O2(g)⇌P4O10(s)?

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What is the equilibrium constant expression for the reaction?
$P_{4} (s) + 5 O_{2} (g) ⇌ P_{4} O_{10} (s) ?$