When limestone is heated, quick lime is formed according to the equation,
`CaCO_3 (s) hArr CaO(s) +CO_2 (g)`
The experiment was carried out in the temperature range `800 -900 ^@C` . Equilibrium constant `K_p` follows the relation, `log_(10) K_p=7.282-8500//T` where T is temperature in kelvin . At what temperature the decomposition will give `CO_2(g)` at 1 atm ?

Explanation

To solve the problem, we need to determine the temperature at which the decomposition of limestone (CaCO3) will yield CO2 at a pressure of 1 atm. We will use the provided relationship for the equilibrium constant \( K_p \).

### Step-by-Step Solution:

1. **Understanding the Reaction**:
The decomposition of limestone can be represented by the equation:
\[
\text{CaCO}_3 (s) \rightleftharpoons \text{CaO} (s) + \text{CO}_2 (g)
...