A 2.00 L vessel is charged with 46.0 g of N₂O₄ and then heated to 350 K. Calculate the equilibrium molar concentrations of N₂O₄ and NO₂. Use the assumption that ΔHº and ΔSº do not vary with temperature and recall that ΔGº is related with the pressure equilibrium constant.

For the reaction 2 HgO(s) → 2 Hg(l) + O₂(g), use the given thermodynamic data to calculate the equilibrium pressure of O₂ in a 1.5 L vessel that contains 10 g of HgO at 350 ºC. Use the assumption that ΔHº and ΔSº do not vary with temperature.

Given the following data

What are the ΔH°, ΔG°, K, and ΔS ° for the reaction  Sn (s) + 2 Cl₂ (g) → SnCl₄ (g) at 25 °C?

Consider the gaseous equilibrium for the dimerization of NO₂ at 350 K.

2 NO₂(g) ⇌ N₂O₄(g)

What is the value of ΔG when NO₂ = 1.23 atm and N₂O₄ = 2.45 atm? Use the following ΔG° values:

ΔG° (NO₂(g)) = 51.3 kJ/mol

ΔG° (N₂O₄(g)) = 99.8 kJ/mol

In which direction (forward or reverse) this reaction is spontaneous under the given conditions?

Molecular iodine sublimes at 184 ºC. The standard molar entropies for solid and gaseous iodine are S°_I2(s) = 116.1 J/mol K and S°_I2(g) = 260.7 J/mol K. Determine the temperature where iodine exhibits a vapor pressure of 430 mmHg.

Given the following decomposition reaction:

P₄(g) → 2 P₂(g); ΔH°_rxn = 229.1 kJ

Calculate the percentage of 0.100 atm P₄ that decomposes at 314 K if 47.00% of P₄ decomposes to P₂ when equilibrium at 298 K is reached.

Based on the given equilibrium constant at different temperatures, what are ΔS°_rxn and ΔH°_rxn for the reaction?

2 SO₂ (g) + O₂ → 2 SO₃ (g)