`COCO_(3((s))hArrCaO_((s))+SO_(2(g))` with of the following expression is correct
or
For the equlibrium `CaCO_(3(s))hArrCaO_((s))+CO_(2(s))` the equlibrium constant is perpesented by the following from

Options

A. `K_(p)=(P_(CaO+P_(CO_(2)))//P_(CaCo_(3)))`
B. `K_(p)=P_(CO_(2))`
C. `K_(p)xx(P_(CaO)xxP_(CO_(2))).P_(CaCO_(3))`
D. `(K_(p)[CaP][CO_(2)])/([CaCO_(3)])`

Explanation

To solve the question regarding the equilibrium reaction of calcium carbonate (CaCO₃) dissociating into calcium oxide (CaO) and carbon dioxide (CO₂), we need to analyze the equilibrium expressions for both Kp and Kc.

### Step-by-Step Solution:

1. **Write the Balanced Equation:**
The given equilibrium reaction is:
\[ \text{CaCO}_3(s) \rightleftharpoons \text{CaO}(s) + \text{CO}_2(g) \]

2. **Identify the Phases of Each Component:**
- CaCO₃ is a solid (s).
- CaO is also a solid (s).
- CO₂ is a gas (g).

3. **Understanding the Equilibrium Constant (Kc):**
The equilibrium constant expression Kc is based on the concentrations of the gaseous and aqueous species only. Solids and liquids do not appear in the expression. Therefore, for the reaction:
\[ K_c = \frac{[\text{Products}]}{[\text{Reactants}]} \]
Since both CaCO₃ and CaO are solids, they will not be included in the Kc expression. Thus:
\[ K_c = [\text{CO}_2] \]

4. **Understanding the Equilibrium Constant (Kp):**
Kp is based on the partial pressures of the gaseous components. For the same reaction:
\[ K_p = \frac{P_{\text{Products}}}{P_{\text{Reactants}}} \]
Again, since CaCO₃ and CaO are solids, they do not appear in the Kp expression. Therefore:
\[ K_p = P_{\text{CO}_2} \]

5. **Conclusion:**
The correct expressions for the equilibrium constants are:
- For Kc: \( K_c = [\text{CO}_2] \)
- For Kp: \( K_p = P_{\text{CO}_2} \)

### Final Answer:
- The correct expression for Kp is the partial pressure of CO₂, and for Kc, it is the concentration of CO₂.