Calculate `DeltaG^@` for the reaction
`2HCl (g) + F_2(g) to 2HF (g) + Cl_2(g) `at `25^@C`
at Given : `Delta_f G^@ [ HCl (g)] = -95.30 kJ mol^(-1)`.
`Delta_fG^@ [ HF(g)] = -273 kJ mol^(-1)`. Also calculate the equilibrium constant the reacton at `25^@C`. Given, gas constant `R = 8.314 JK^(-1) mol^(-1)`.

Explanation

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

\[ 2 \text{HCl} (g) + \text{F}_2(g) \rightarrow 2 \text{HF} (g) + \text{Cl}_2(g) \]

at 25°C, we will use the following formula:

\[
\Delta G^\circ = \sum \Delta G_f^\circ \text{(products)} - \sum \Delta G_f^\circ \text{(reactants)}
...