Reversible Reactions

Reversible Reactions

1. A reaction that can work in both directions i.e. reactants can form products and those products can then react to form the reactants again

2. EXAMPLE 1 - THERMAL DECOMPOSITION OF AMMONIUM CHLORIDE

3. The concentrations of the reactants and products in a reversible reaction remain constant if the system is closed. Thowever, the reactions are contiuining continuously in both directions.

4. The point of equilibrium=Proportion of components in the equilibrium mixture.

   • Factors that affect it
     • Temperature
     • Pressure
       • only applies to gases
       • <pressure = shifted equilibrium position to direction producing fewer moles of gas
   • There are two main characteristics of a reaction that has reached dynamic equilibrium:
     • 1. The forward and reverse reactions occur at the same rate.
     • 2.. The concentrations of reactants and products remain constant.
     • A reversible reaction will reach dynamic equilibrium in a sealed container (a closed system)

5. EXAMPLE 2 - HYDRATION OF COPPER (ll) SULFATE

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