Achemist fills a reaction vessel with a 0.105g mercurous chloride hg2cl2 solid, 0.926 m mercury (i) (hg2^2+) aqueous solution, and 0.573 m chloride (cl^-) aqueous solution at a temperature of 25.0°c.
under these conditions, calculate the reaction free energy δg for the following chemical reaction:
hg2cl2(s) > hg2^2+ (aq) + 2cl^- (aq)

ΔG = 98.67 kJ/mol

Explanation:

Let' s consider the following reaction.

Hg₂Cl₂(s) → Hg₂²⁺(aq) + 2Cl⁻(aq)

The standard Gibbs free energy (ΔG°) for the reaction is:

ΔG° = 1 mol × ΔG°f(Hg₂²⁺(aq)) + 2 mol × ΔG°f(Cl⁻(aq)) - 1 mol × ΔG°f(Hg₂Cl₂(s))

where,

ΔG°f: standard Gibbs free energy of formation

ΔG° = 1 mol × (154.72 kJ/mol) + 2 mol × (-134.08 kJ/mol) - 1 mol × (-215.06 kJ/mol)

ΔG° = 101.62 kJ

This is standard Gibbs free energy change per mole of reaction.

The Gibbs free energy of the reaction (ΔG) can be calculated using the following expression.

ΔG = ΔG° - R.T.lnQ

where,

R: ideal gas constant

T: absolute temperature

Q: reaction quotient

ΔG = ΔG° - R.T.ln([Hg₂²⁺].[Cl⁻]²)

ΔG = 101.62 kJ/mol + (8.314 × 10⁻³ kJ/mol.K) . (298.2 K) . ln [(0.926).(0.573)²]

ΔG = 98.67 kJ/mol

sodium (na), for example, has one electron in its valence shell. this is an unstable state because that valence shell needs eight electrons to be full. in order to fill its valence shell, find a way to add seven electrons to its valence shell