$K_{p}$ for the reaction: $C a C O_{3} (s) ⇋ C a O (s) + C O_{2} (g)$ is correctly expressed as:

K_{p} = \frac{[P_{C a O} \times P_{C O_{2}}]}{[P_{C a C O_{3}}]}

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K_{p} = \frac{[P_{C a C O_{3}}]}{[P_{C a O} \times P_{C O_{2}}]}

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K_{p} = P_{C O_{2}}

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K_{p} = \frac{[P_{C O_{2}}]}{[P_{C a C O_{3}}]}

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Solution

The correct option is C $K_{p} = P_{C O_{2}}$
The reaction is $C a C O_{3} (s) ⇋ C a O (s) + C O_{2} (g)$ .
The concentration or partial pressure of solid reactants and products do not appear in the expression for the equilibrium constant.
Thus, the expression for the equilibrium constant becomes $K_{p} = P_{C O_{2}}$ .

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