The vapor pressure of any liquid and the pressure exerted by its vapor are equal when the two are in equilibrium. Determine the value of K_p at the normal boiling point of a liquid in equilibrium with its vapor.

The equilibrium constant for the following decomposition reaction at 212 °C is 1.20. 

Ca(OCl)₂(s) → Ca(s) + Cl₂(g) + O₂(g) 

What are the equilibrium concentrations of Cl₂ and O₂ if a sample of Ca(OCl)₂(s) is put inside a closed container at 212 °C and allowed to reach equilibrium?

For the reaction A + X ⇌ B, where X = C (blue), D (orange), or E (grey), refer to the three images below showing the reaction at equilibrium at the same temperature. Arrange K_eq for the three reactions from smallest to largest.

A dry ice container with a capacity of 20.0 US liquid quarts was used to hold cylindrical dry ice pellets. Assuming that each pure cylindrical dry ice pellet has a density of 1.6 g/cm³, a diameter of 1.6 cm, and a length of 6.0 cm, find the number of pellets required to saturate the container with gaseous carbon dioxide. The equilibrium constant K_c for the sublimation of carbon dioxide is 1889.2.

CO₂ (s) ⇌ CO₂ (g)

The equilibrium constant (K_c) of the reaction MgC₂O₄(s) ⇌ Mg²⁺(aq) + C₂O₄^2–(aq) at 25.0°C is 8.6×10^–5. In a saturated solution of MgC₂O₄, calculate the equilibrium concentrations of Mg²⁺ and C₂O₄^2–.

Sulfur dioxide (SO₂) gas reacts with oxygen (O₂) to produce sulfur trioxide (SO₃): 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g). A 5.5 L reaction vessel is charged with a mixture of SO₂ and O₂ at 300 °C. When the equilibrium was established, the mixture had the three gases at these partial pressures: P_SO2 = 1.15 atm, P_O2 = 2.35 atm, and P_SO3 = 0.855 atm. Determine K_p.

In an equilibrium mixture, [SO₂] = 3.50 M and [SO₃] = 9.20 M. Calculate [O₂] at equilibrium for the mixture.

2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g), K_eq = 560