Show that the reaction
`CO(g) +(1//2)O_(2)(g) rarr CO_(2)(g)`
at `300K` is spontaneous and exothermic, when the standard entropy change is `-0.094 k J mol^(-1) K^(-1)`. The standard Gibbs free energies of formation for `CO_(2)`and `CO` are `-394.4`and `-137.2kJ mol^(-1)`, respectively.

Explanation

To show that the reaction

\[ \text{CO(g)} + \frac{1}{2} \text{O}_2(g) \rightarrow \text{CO}_2(g) \]

at \( 300 \, \text{K} \) is spontaneous and exothermic, we will follow these steps:

### Step 1: Calculate the Standard Gibbs Free Energy Change (\( \Delta G^\circ \))

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