An equilibrium is a state in a physical or chemical system in which the forward and reverse reactions occur at the same rate, resulting in a constant concentrat...
An equilibrium is a state in a physical or chemical system in which the forward and reverse reactions occur at the same rate, resulting in a constant concentration of reactants and products. Equilibrium is established when the forward and reverse reactions occur simultaneously at the same rate, resulting in a constant overall reaction rate.
An equilibrium can be achieved through various mechanisms, including changes in temperature, pressure, concentration, and surface area. For instance, when the temperature of a gas is increased, the equilibrium will shift towards the endothermic reaction (the reverse reaction), resulting in a decrease in the concentration of the product. Conversely, when the temperature is decreased, the equilibrium will shift towards the exothermic reaction (the forward reaction), resulting in an increase in the concentration of the product.
Another mechanism for achieving equilibrium is through changes in pressure. When the pressure is increased, the equilibrium will shift towards the side with fewer moles of gas, resulting in a decrease in the concentration of the gas molecules. Conversely, when the pressure is decreased, the equilibrium will shift towards the side with more moles of gas, resulting in an increase in the concentration of the gas molecules.
Lastly, equilibrium can also be achieved through changes in the surface area of the system. When the surface area of the system is increased, the equilibrium will shift towards the side with more molecules on the surface, resulting in an increase in the concentration of the product. Conversely, when the surface area is decreased, the equilibrium will shift towards the side with fewer molecules on the surface, resulting in a decrease in the concentration of the product