What are the conditions for equilibrium in a closed system?

For a closed system to be in equilibrium, the rates of the forward and reverse reactions must be equal.

In a closed system, equilibrium is achieved when the rates of the forward and reverse reactions are the same. This doesn't mean that the reactions have stopped, but rather that they are happening at the same speed. This is known as dynamic equilibrium. The concentrations of the reactants and products remain constant, but they are not necessarily equal.

The conditions for equilibrium are governed by Le Chatelier's Principle. This principle states that if a change in conditions is applied to a system at equilibrium, the system will adjust itself to counteract that change. For example, if the concentration of a reactant is increased, the system will respond by increasing the rate of the forward reaction to use up the added reactant and restore equilibrium.

Temperature also affects equilibrium. If the temperature is increased, the system will respond by favouring the endothermic reaction (the reaction that absorbs heat) to try and decrease the temperature. Conversely, if the temperature is decreased, the system will favour the exothermic reaction (the reaction that releases heat) to try and increase the temperature.

Pressure changes can also affect equilibrium in reactions involving gases. If the pressure is increased, the system will shift to favour the side of the reaction with fewer gas molecules to try and decrease the pressure. If the pressure is decreased, the system will favour the side with more gas molecules to try and increase the pressure.

In summary, a closed system is in equilibrium when the rates of the forward and reverse reactions are equal, and this equilibrium can be shifted by changes in concentration, temperature, and pressure.