Calculate the equilibrium constant for the following reaction at `298K` and `1` atmospheric pressure:
`C(graphite) +H_(2)O(l) rarr CO(g) +H_(2)(g)`
Given `Delta_(f)H^(Theta) at 298 K` for `H_(2)O(l) =- 286.0 kJ mol^(-1)`
for `CO(g) =- 110.5 kJ mol^(-1)`
`DeltaS^(Theta)` at `298K` for the reaction `= 252.6 J K^(-1) mol^(-1)`

Explanation

To calculate the equilibrium constant for the reaction:

\[ C(\text{graphite}) + H_2O(l) \rightleftharpoons CO(g) + H_2(g) \]

at \( 298 \, K \) and \( 1 \, atm \), we will follow these steps:

### Step 1: Determine the standard enthalpy change (\( \Delta H^\circ \)) for the reaction.

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