The Equilibrium Constant, Kc - exam practice

Equal amounts of W and X are mixed and allowed to reach equilibrium.

W + X ⇌ Y + Z

The value of the equilibrium constant is 4.85. At equilibrium, the mixture will contain

Two moles of compound P were placed in a vessel. The compound P was partly decomposed by heating. A dynamic equilibrium between chemicals P, Q and R was established.

At equilibrium, x mol of R were present and the total number of moles present was (2 + x).

What is the equation for this equilibrium?

Sulfur trioxide is manufactured from sulfur dioxide and oxygen, using the Contact process.

Which condition affects the value of the equilibrium constant?

Nitrogen reacts with hydrogen to produce ammonia.

N₂(g) + 3H₂(g) 2NH₃(g)

A mixture of 2.00 mol of nitrogen, 6.00 mol of hydrogen, and 2.40 mol of ammonia is allowed to reach equilibrium in a sealed vessel of volume 1 dm³ under certain conditions. It was found that 2.32 mol of nitrogen were present in the equilibrium mixture.

What is the value of K_c under these conditions?

The value of the equilibrium constant, K_c , for the reaction to form ethyl ethanoate from ethanol and ethanoic acid is 4.0 at 60°C.

C₂H₅OH + CH₃CO₂H ⇌ CH₃CO₂C₂H₅ + H₂O

1.0 mol of ethanol and 1.0 mol of ethanoic acid are allowed to reach equilibrium at 60°C.

What is the number of moles of ethyl ethanoate formed?

The reaction between sulfur dioxide and oxygen is reversible.

2SO_2(g) + O_2(g) ⇌ 2SO_3(g) K_c = 280 mol^-1 dm³ at 1,000 K

In an equilibrium mixture at 1,000 K the sulfur trioxide concentration is 6.00 mol dm^-3.

The sulfur dioxide concentration is twice the oxygen concentration.

What is the sulfur dioxide concentration?

0.200 mol of sulfur dioxide and 0.200 mol of oxygen are placed in a 1.00 dm³ sealed container.

The gases are allowed to react until equilibrium is reached.

2SO₂ + O₂ ⇌ 2SO₃

At equilibrium there is 0.100 mol of SO₃ in the container.

What is the value of K_c?

This question is about the reversible reaction below.

2NO_2(g) ⇌ N₂O_4(g)

A chemist investigating this reaction started with 10 moles of NO₂ and allowed the system to reach equilibrium.

If 3 moles of N₂O₄ are formed, the number of moles of NO₂ at equilibrium is