Unit 7: Equilibrium

For the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g), which change shifts equilibrium to the right?

For A ⇌ 2B, Kc = 4.0. If [A] = 0.50 M at equilibrium, what is [B] in M?

For the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g), the equilibrium expression Kc is

For the reaction 2SO₂(g) + O₂(g) ⇌ 2SO₃(g), Kc = 280 at a certain temperature. If the initial concentrations are [SO₂] = 0.10 M, [O₂] = 0.20 M, and [SO₃] = 0, the reaction will

According to Le Chatelier's principle, if the volume of a container holding the equilibrium N₂(g) + 3H₂(g) ⇌ 2NH₃(g) is decreased, the equilibrium will

For the equilibrium PCl₅(g) ⇌ PCl₃(g) + Cl₂(g), Kp = 1.05 at 250°C. If the partial pressures of PCl₅, PCl₃, and Cl₂ are 0.80, 0.60, and 0.60 atm respectively, which statement is correct?

Adding a catalyst to a reaction at equilibrium will

The solubility product constant (Ksp) for AgCl is 1.8 × 10⁻¹⁰. The molar solubility of AgCl in pure water is

According to Le Chatelier's principle, adding more reactant to a system at equilibrium will:

A large equilibrium constant ([math]) indicates:

The equilibrium constant expression for solubility, [math]:

If [math] for a reaction, the system will:

Increasing the temperature of an exothermic reaction at equilibrium will:

Adding a catalyst to a system at equilibrium:

The common ion effect states that:

Pure solids and liquids are excluded from equilibrium expressions because:

What is the value of Kc for this reaction at equilibrium?

Based on the data, is the forward reaction exothermic or endothermic? Explain the shift.

What is the equilibrium concentration of I₂?

What will happen when these concentrations are mixed?