Chemical Equilibrium Practice Problems
Problem 1: Classify the following equilibrium reactions as homogeneous or heterogeneous.
- 2Hg(l) + O2(g) ⇌ 2HgO(s)
- H2(g) + I2(g) ⇌ 2HI(g)
- CH3COOH(aq) ⇌ CH3COO– (aq) + H+(aq)
- C(s) +O2(g) ⇌ CO2(g)
- CaCO3(s) ⇌ CaO(s) + CO2(g)
Problem 2: Consider the equilibrium equation: H2(g) + I2(g) ⇌ 2HI(g)
If 2 moles of H2 and 1 mole of I2 are placed in a 1-liter vessel. How many moles of each substance is present at equilibrium at 458℃, if Kc at 458℃= 49.7?
Problem 3: Consider the reaction: 2Hg(l) + O2(g) ⇌ 2HgO(s)
If 10 moles of Hg, and 5.6 moles of O2 attain equilibrium at 350℃. If 20 moles of HgO are obtained, find the equilibrium constant.
Problem 4: The equilibrium constant at 500℃ for the reaction A(g) +B2(g) ⇌ AB2(g) is 0.04. A catalyst is added the rate of equilibrium is increased by five times. Find the change in equilibrium constant.
Chemical Equilibrium
Chemical Equilibrium is a condition of a reversible chemical reaction, where the rate of forward and backward reactions are equal. In Chemical equilibrium, the concentrations of the products and reactants remain constant i.e. it does not change with time. This is a state after which there are no observable changes in the properties and the system becomes constant. In this state, the forward reaction proceeds at the same rate as the reverse reaction.
In this article, we will learn more about chemical equilibrium, its types, its examples, and more, so Let’s get started.
Table of Content
- What is Chemical Equilibrium?
- Types of Chemical Equilibrium
- Conditions for Chemical Equilibrium
- Factors Affecting Chemical Equilibrium
- Equilibrium constant
- Importance of Chemical Equilibrium