1. Temperature:
* Exothermic reactions: Increasing the temperature shifts the equilibrium to the left, favoring the reactants. Decreasing the temperature shifts the equilibrium to the right, favoring the products.
* Endothermic reactions: Increasing the temperature shifts the equilibrium to the right, favoring the products. Decreasing the temperature shifts the equilibrium to the left, favoring the reactants.
2. Concentration:
* Increasing the concentration of reactants: Shifts the equilibrium to the right, favoring the products.
* Increasing the concentration of products: Shifts the equilibrium to the left, favoring the reactants.
* Decreasing the concentration of reactants or products: The equilibrium will shift to compensate for the change.
It's important to note that pressure can also affect the position of equilibrium, but only for reactions involving gases.
* Increasing pressure: Shifts the equilibrium towards the side with fewer moles of gas.
* Decreasing pressure: Shifts the equilibrium towards the side with more moles of gas.
