STATEMENT-1: `CaCo_(3)(s)hArrCaO(s)+CO_(2)(g),` for given equlibrium `K_(rho)=pCO_(2).`
STATEMENT-2: If we add `CaCO_(3),` equlibrium will shift in forward direction

Options

A. Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for Statement-8
B. Statement-1 is True, Statement-2 is True, Statement-2 is NOT a correct explanation for Statement-8
C. Statement-1 is True, Statement-2 is False
D. Statement-1 is False, Statement-2 is True

Answer

To solve the given question, we will analyze both statements one by one and determine their validity based on the principles of chemical equilibrium.

### Step 1: Analyze Statement 1
The first statement describes the equilibrium reaction:
\[ \text{CaCO}_3(s) \rightleftharpoons \text{CaO}(s) + \text{CO}_2(g) \]

For this equilibrium, the equilibrium constant \( K_p \) is defined in terms of the partial pressures of the gaseous products and reactants. Since calcium carbonate (CaCO3) and calcium oxide (CaO) are solids, they do not appear in the expression for \( K_p \). Therefore, the equilibrium constant can be expressed as:
\[ K_p = P_{\text{CO}_2} \]
where \( P_{\text{CO}_2} \) is the partial pressure of carbon dioxide gas.

**Conclusion for Statement 1:** This statement is true.

### Step 2: Analyze Statement 2
The second statement claims that if we add more calcium carbonate (CaCO3) to the system, the equilibrium will shift in the forward direction (towards the production of CaO and CO2).

According to Le Chatelier's principle, the addition of a solid reactant does not affect the position of equilibrium because the concentration (or amount) of solids does not change in the equilibrium expression. Therefore, adding more CaCO3 will not shift the equilibrium position in either direction.

**Conclusion for Statement 2:** This statement is false.

### Final Conclusion
- **Statement 1:** True
- **Statement 2:** False

Thus, the correct answer is that Statement 1 is true and Statement 2 is false.