Dynamic Equilibrium

Reversible reaction

• The products can react with each other to produce the original reactants (it can go forwards and backwards)

The haber process is an example of a reversible reaction

• Nitrogen and hydrogen react to form ammonia: N2 + 3H2→←2NH3

• The nitrogen is obtained easily from the air

• The hydrogen can be extracted from natural gas and crude oil

• The Haber process is carried out at 450°C + pressure: 200 atmosphere + iron catalyst

Dynamic Equilibrium

• The forward and backward reactions are both happening at the same time and at the same rate (but there's no effect) + the concentrations of reactants and products have reached a balance and won’t change

• Equilibrium can only be reached if the reversible reaction takes place in a closed system → none of thr reactants or products can escape

When a reaction is at equilibrium it doesn’t mean that the amounts of reactants and products are equal

• Sometimes the equilibrium will lie to the right → this means the concentration of products is greater than the concentration of reactants

• Sometimes the equilibrium will lie to the left → this means the concentration of reactants is greater than the concentration of products

• The exact position of equilibrium depends on the conditions