Consider the reaction:
`4NH_(3)(g) +5O_(2)(g) rarr 4NO(g) +6H_(2)O(l) DeltaG^(Theta) =- 1010.5 kJ`
Calculate `Delta_(f)G^(Theta) [NO(g)] if Delta_(f)G^(Theta) (NH_(3)) = -16.6 kJ mol^(-1)` and `Delta_(f)G^(Theta) [H_(2)O(l)] =- 237.2 kJ mol^(-1)`.

Explanation

To calculate the standard Gibbs free energy of formation (Δ_fG°) for NO(g) from the given reaction and data, we will follow these steps:

### Step-by-Step Solution:

1. **Write the Reaction**:
The reaction is given as:
\[
4 \text{NH}_3(g) + 5 \text{O}_2(g) \rightarrow 4 \text{NO}(g) + 6 \text{H}_2O(l)
...