A sample of `CaCO_(3)(s)` is introduced into a sealed container of volume `0.654 L` and heated to `1000 K` until equilibrium is reached. The equilibrium constant for the reaction
`CaCO_(3)(s)hArrCaO(s)+CO_(2)(g),`
is `3.9xx10^(-2)` atm at this temperature. Calculate the mass of `CaO` present at equilibrium.

Explanation

To solve the problem step by step, we will follow the outlined procedure:

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

The equilibrium constant \( K_p \) for this reaction at 1000 K is given as:
\[ K_p = 3.9 \times 10^{-2} \, \text{atm} \]
...