What is the equilibrium constant expression for the following equation?

2NO₂ (g) + F₂ (g) ⇌ 2NO₂F (g)

Consider the following equilibrium reaction.

2N₂O (g) + O₂ (g) ⇌ 4NO (g) ∆H = +16 kJ

Which change will move the equilibrium to the right?

Iodine and bromine gases were mixed and allowed to reach equilibrium.

What is the value of the equilibrium constant?

*Challenge Question*. Consider how much reactant has been used up and the coefficients to determine x.

Which factor does not affect the position of equilibrium in this reaction?

2NO₂(g) ⇌ N₂O₄(g) ΔH = −58 kJ mol⁻¹

Consider the reaction:

2N₂O (g) ⇌ 2N₂ (g) + O₂ (g)

The values of Kc at different temperatures are given in the table.

Which statement is correct at higher temperature?

The equilibrium constant for

N₂(g) + 3H₂(g) ⇌ 2NH₃(g) is K.

What is the equilibrium constant for this equation?

2N₂(g) + 6H₂(g) ⇌ 4NH₃(g)

Consider the equilibrium between N₂O₄(g) and NO₂(g).

N₂O₄(g) ⇌ 2NO₂(g) ΔH = +58 kJ mol⁻¹

Which changes shift the position of equilibrium to the right?

Select all that apply.

Which change will favor the reverse reaction in the equilibrium?

2 CrO₂^2- (aq) + 2H⁺ (aq) ⇌ Cr₂O₇^2- (aq) + H₂O (l) ∆H= -42 kJ

Which combination of temperature and pressure will give the greatest yield of sulfur trioxide?

2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) ∆H = -196 kJ