For the reaction, `NH_4Cl(s) to NH_3(g) + HCl(g)` at `25^@C`, enthalpy change `DeltaH = + 177 kJ mol^(-1)` and entropy change `Delta S = + 285 J mol^(-1) K^(-1)`. Calculate the free energy change `DeltaG" at " 25^@C` and predict whether the reaction is spontaneous or not.

Explanation

To solve the problem, we need to calculate the free energy change (ΔG) for the reaction using the given values for enthalpy change (ΔH) and entropy change (ΔS). We will also determine if the reaction is spontaneous based on the value of ΔG.

### Step-by-Step Solution:

1. **Identify the given values:**
- Enthalpy change (ΔH) = +177 kJ/mol
- Entropy change (ΔS) = +285 J/(mol·K)
- Temperature (T) = 25°C
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