Partial Pressures and Equilibrium Calculations Quiz

Study Notes

Chemical Equilibrium

Chemical equilibrium is a state where the rates of forward and reverse reactions are equal, and the concentrations of reactants and products remain constant.
The position of equilibrium is a measure of the percentage of reactants converted to products.
If the equilibrium lies to the left, less than half of the reactants are converted to products, resulting in a low yield of products.
If the equilibrium lies to the right, more than half of the reactants are converted to products, resulting in a high yield of products.

Le Chatelier's Principle

Le Chatelier's Principle states that a system at equilibrium will try to resist any changes to the equilibrium conditions.
If the temperature is increased, the system will try to cool down.
If the pressure is increased, the system will try to reduce the pressure.
If the concentration of a reactant is increased, the system will try to remove the excess reactant.

Effect of Concentration on Equilibrium

If the concentration of a reactant is increased, the system will try to remove the excess reactant by promoting the forward reaction, causing the equilibrium to shift to the right.
If the concentration of a product is increased, the system will try to remove the excess product by promoting the reverse reaction, causing the equilibrium to shift to the left.
If the concentration of a reactant is decreased, the system will try to make more reactant by promoting the reverse reaction, causing the equilibrium to shift to the left.

Effect of Pressure on Equilibrium

If the pressure is increased, the system will try to reduce the pressure by promoting the reaction that produces fewer moles of gas, causing the equilibrium to shift to the right.
If the pressure is decreased, the system will try to increase the pressure by promoting the reaction that produces more moles of gas, causing the equilibrium to shift to the left.

Acid-Base Equilibrium

For a weak acid HA, the acid dissociation constant (Ka) represents the extent of dissociation in water.
A higher Ka value indicates a stronger acid, which dissociates more in water.
The pH of a solution can be calculated using the Ka value and the concentration of the acid.

Self-Ionisation of Water

Water self-ionises to form H3O+ and OH- ions, with an equilibrium constant Kw = 1.00 x 10-14 mol2 dm-6 at 298 K.
The pH of pure water is 7.00 at 298 K.
The self-ionisation of water is an endothermic process, meaning that the concentration of H3O+ increases with increasing temperature.

Description

Test your knowledge on calculating partial pressures of gases and equilibrium concentrations in chemical reactions. Questions involve determining the partial pressures of different gases in a mixture and calculating equilibrium concentrations. Get ready to practice these important concepts!