Gibbs Free Energy (G)

Define is Gibb’s free energy.

The equilibrium constant of a reaction is 10, what will be the sign of ∆G? Will this reaction be spontaneous?

What are the conditions for the spontaneity of a process?

List the characteristics of Gibbs free energy.

For the reaction \[\ce{Ag2O_{(s)} -> 2Ag_{(s)} + 1/2O2_{(g)}}\]: ΔH = 30.56 kJ mol⁻¹ and ΔS = 6.66 JK⁻¹ mol⁻¹ (at 1 atm). Calculate the temperature at which ΔG is equal to zero. Also predict the direction of the reaction

1. at this temperature and
2. below this temperature.

What is the equilibrium constant K_eq for the following reaction at 400 K?

\[\ce{2NOCl_{(g)} ⇌ 2NO_{(g)} + Cl2_{(g)}}\], given that H⁰ = 77.2 kJ mol⁻¹ and ∆S⁰ = 122 JK⁻¹ mol⁻¹

When 1-pentyne (A) is treated with 4N alcoholic KOH at 175°C, it is converted slowly into an equilibrium mixture of 1.3% 1-pentyne (A), 95.2% 2-pentyne (B) and 3.5% of 1, 2 pentadiene (C) the equilibrium was maintained at 175°C, calculate ΔG⁰ for the following equilibria.

\[\ce{B ⇌ A}\] `Δ"G"_1^0` = ?

\[\ce{B ⇌ C}\] `Δ"G"_2^0` = ?

At 33K, N₂O₄ is fifty percent dissociated. Calculate the standard free energy change at this temperature and at one atmosphere.