Following data is given for the reaction : `CaCO_3 (s) to CaO(s) +CO_2(g)`
Given that `Delta_fH^(@) [CaO(s)]=-635.1 "kJ mol"^(-1)`
`Delta_f H^@[CO_2(g)]=-393.5 "kJ mol"^(-1)`
`Delta_fH^@[CaCO_3(s)]=-1206.9 "kJ mol"^(-1)`
Predict the effect of temperature on the equilibrium constant of the above reaction.

Explanation

To predict the effect of temperature on the equilibrium constant for the reaction:

\[ \text{CaCO}_3 (s) \rightleftharpoons \text{CaO}(s) + \text{CO}_2(g) \]

we need to determine whether the reaction is endothermic or exothermic using the provided standard formation enthalpies.

### Step 1: Write down the formation enthalpy values.
- \( \Delta_f H^\circ [\text{CaO}(s)] = -635.1 \, \text{kJ/mol} \)
...