Calculate the standard free energy change for the reaction
`4NH_3(g) + 5O_2(g) to 4NO(g) + 6H_2O(l)`
Given that the standard free energy of formation `(Delta_f G^@)" for " NH_3(g) NO(g) and H_2O (l)` are -16.8, + 86.7 and `-237.2 kJ mol^(-1)` respectively. Predict the feasibility of the above reaction at the standard state.

Explanation

To calculate the standard free energy change (ΔG°) for the reaction:

\[ 4 \text{NH}_3(g) + 5 \text{O}_2(g) \rightarrow 4 \text{NO}(g) + 6 \text{H}_2O(l) \]

we will use the standard free energy of formation (ΔG°_f) values provided for the reactants and products.

### Step-by-Step Solution:

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