At 789 K, the equilibria for the following reactions are 

CuS(s) + H₂(g) → Cu(s) + H₂S(g) K_c = 78.9

CS₂(g) + H₂(g) → CS(g) + H₂S(g) K_c = 0.289

Based on the given equilibria, what will be the K_c for CuS (s) + CS (g) → Cu (s) + CS₂ (g)?

The dissociation of hydrogen selenide (H₂Se) takes place in two steps:

H₂Se ⇌ H⁺ + HSe^-        K₁ = 1.29×10^-4

HSe^- ⇌ H⁺ + Se^2-          K₂ = 1.00×10^-11

Calculate the equilibrium constant for the following reaction:

Se^2- + 2H⁺ ⇌ H₂Se

The following reaction is a vital step in the metabolism of glucose: glucose + ATP ⇌ glucose-6-phosphate + ADP

Determine the equilibrium constant for the above reaction using the related equilibrium constants:

glucose + Pi ⇌ glucose-6-phosphate, K = 3.114 × 10^–3

ATP ⇌ ADP + Pi, K = 2.716 × 10⁵

The dissociation of hydrogen selenide (H₂Se) takes place in two steps:

H₂Se ⇌ H⁺ + HSe^-        K₁ = 1.29×10^-4

HSe^- ⇌ H⁺ + Se^2-          K₂ = 1.00×10^-11

Calculate the equilibrium constant for the following reaction:

Se^2- + 2H⁺ ⇌ H₂Se