Describe the differences between the effect of changes in concentration, pressure and temperature on the equilibrium constant.

Changes in concentration, pressure and temperature affect the equilibrium constant differently.

Changes in concentration affect the equilibrium constant by shifting the position of the equilibrium. If the concentration of a reactant is increased, the equilibrium will shift towards the products to counteract the change, resulting in an increase in the equilibrium constant. Conversely, if the concentration of a product is increased, the equilibrium will shift towards the reactants, resulting in a decrease in the equilibrium constant.

Changes in pressure affect the equilibrium constant only for reactions involving gases. An increase in pressure will cause the equilibrium to shift towards the side with fewer moles of gas to counteract the change, resulting in a decrease in the equilibrium constant. Conversely, a decrease in pressure will cause the equilibrium to shift towards the side with more moles of gas, resulting in an increase in the equilibrium constant.

Changes in temperature affect the equilibrium constant by changing the value of the equilibrium constant itself. An increase in temperature will cause the equilibrium constant to increase for endothermic reactions and decrease for exothermic reactions. Conversely, a decrease in temperature will cause the equilibrium constant to decrease for endothermic reactions and increase for exothermic reactions.

In summary, changes in concentration and pressure affect the position of the equilibrium, while changes in temperature affect the value of the equilibrium constant.