Common Misconceptions
This section outlines some of the common misconceptions in equilibrium. It is important that the student is cleared of theses misconceptions for this unit.
This section outlines some of the common misconceptions in equilibrium. It is important that the student is cleared of theses misconceptions for this unit.
Chemical equilibrium is a static condition
Equilibrium constants are constant under all condition
If you add more solid, the equilibrium concentrations of the aqueous species will go up
The rate of the forward reaction increases with time from the mixing of the reactants until equilibrium is established.
A simple arithmetic relationship exists between the concentrations of reactants and products at equilibrium
When a system is at equilibrium and a change is made in the conditions, the rate of the favoured reaction increases but the rate of the other reaction decreases
- The net equation would be static due to the rate of the forward reaction and the rate of the reverse reaction being equal, but both reactions are simultaneously occurring.
Equilibrium constants are constant under all condition
- They change according to the change in outer conditions such as temperature and pressure
If you add more solid, the equilibrium concentrations of the aqueous species will go up
- It could be true, but it depends on the situation; if it’s a saturated solution, the concentration of the aqueous species will not change
The rate of the forward reaction increases with time from the mixing of the reactants until equilibrium is established.
- The rates increasing depends on how far you are in the establishment of the equilibrium. This misconception can be cleared with the aid of the equilibrium quotient.
A simple arithmetic relationship exists between the concentrations of reactants and products at equilibrium
- The relationship between the two values contain more complex mathematic relationships, including exponents and roots of equations.
When a system is at equilibrium and a change is made in the conditions, the rate of the favoured reaction increases but the rate of the other reaction decreases
- This depends on what change was applied; in certain conditions, the rate of the less favoured reaction could increase (Haber-Bosch Process)