The partial pressure of `CO_(2)` in the reaction
`CaCO_(3)(s) hArr CaO(s)+CO_(2)(g)`
Is `0.773` mm at `500^(@)C`. Calculate `K_(p)` at `600^(@)C` for the above reaction, `DeltaH` of the reaction is `43.2` kcal per mole and does not change in the given range of temperature.

Explanation

To solve the problem, we will follow these steps:

### Step 1: Write the reaction and identify the components
The reaction given is:
\[ \text{CaCO}_3(s) \rightleftharpoons \text{CaO}(s) + \text{CO}_2(g) \]

In this reaction, calcium carbonate (CaCO₃) and calcium oxide (CaO) are solids, while carbon dioxide (CO₂) is a gas. The equilibrium constant \( K_p \) for this reaction depends only on the partial pressure of the gaseous product, CO₂.

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