Answer:
ΔG° = 41.248 KJ/mol (298 K); the correct answer is a) 41 KJ
Explanation:
Ag+(aq) + 2NH3(aq) ↔ Ag(NH3)2+(aq)
⇒ Kf = 1.7 E7; T =298K
⇒ ΔG° = - RT Ln Kf.....for aqueous solutions
∴ R = 8.314 J/mol.K
⇒ ΔG° = - ( 8.314 J/mol.K ) * ( 278 K ) ln ( 1.7 E7 )
⇒ ΔG° = 41248.41 J/mol * ( KJ / 1000J )
⇒ ΔG° = 41.248 KJ/mol
Answer:
c. –41 kJ
Explanation:
Let's consider the following equation for the formation of a complex.
Ag⁺(aq) + 2NH₃(aq) ⇄ Ag(NH₃)₂⁺(aq)
The equilibrium constant (Kf) is 1.7 × 10⁷.
We can find the standard Gibbs free energy (ΔG°) using the following expression.
ΔG° = - R × T × ln Kf
where,
R: ideal gas constant
T: absolute temperature
ΔG° = - (8.314 J/K.mol) × 298 K × ln 1.7 × 10⁷ = - 4.1 × 10⁴ J/mol = -41 kJ/mol
This is the energy per mole of the balanced reaction.
