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Chemical Equilibrium

Equilibrium

Concetration:

The concept of chemical equlibrium refers to the state in which the products and reactants of the reaction have reached an amount of concentration that will not proceed to change with time.

• Increase in reactant concentration(Product Favoured Reaction Shift) : The equlibirum shifts to the products, to reduce the concetration of the reactants.

• Increase in product concentration (Reactant Favoured Reaction Shift) :

The equilibrium shifts to the reactants, to reduce the concetration of the products.

Factors Considered in Equilibrium: - Temperature - Concetration - Pressure - Volume

C + D

A + B

Le Chatelier's Principle

Temperature:

• Increase in temperature: Equilibrium shifts in order to reduce temperature.

• Decrease in Temperature: Equilibrium shifts in order to increase the temeprature of reaction

Le Chatelier's Principle states that when a change is made to the system at equlibrium, the system's resposne will be to make a counteractive change, to re=establish equlibrium.

Endothermic Reaction: A + 2B C + D There is more A and B than C and D, and the endothermic reaction will shift the reaction leading to a decrease in temperature

Exothermic Reaction: A + 2B C + D In this case, there will be more C and D than A and B, and will cause an exothermic reaction, leading to an increase in temperature.

Pressure:

• Pressure Increase: Reaction shifts towards the side with fewer gas particles.

• Pressure Decrease : Reaction shifts towards the side with greater number of gas molecules.

Example:

A common example in which Le Chatelier's principle is applied is the Haber Bosch process that is used for the synthesis of ammonia. In this case, a balance between temperature and pressure is what is being determined.