For the reaction $C a C O_{3}$ (s) $⇋$ $C a O$ (s) + $C O_{2}$ (g) the partial pressure of $C O_{2}$ (at equilibrium) depends on:

the mass of $C a O$

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the mass of $C a C O_{3}$

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Both a and b

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temperature

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Solution

The correct option is D
temperature

CaCO₃(s) $⇋$ CaO (s) + CO₂ (g)
$K_{c}$ = $\frac{[C a O (s)] [C O_{2} (g)]}{[C a C O_{3} (s)]}$
Since concentration of $C a C O_{3}$ (s) and $C a O (s)$ are constant, therefore modified equilibrium
constant for the thermal decomposition of calcium carbonate will be $K_{c}$ = [ $C O_{2}$ (g)]

or $K_{p}$ = $p_{C O_{2}}$

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Similar questions

For the reaction $C a C O_{3}$ (s) $⇋$ $C a O$ (s) + $C O_{2}$ (g) the partial pressure of $C O_{2}$ (at equilibrium) depends on:

The equilibrium constant for the reaction,

CaCO₃(s) ⇌ CaO(s) + CO₂(g), is

C a C O_{3} (s) ⇋ C a O (s) + C O_{2} (g),

C O_{2} (g)

C a C O_{3} (s) ⇌ C a O (s) + C O_{2} (g)

C O_{2}

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