Le chatelier principle

LE CHATELIER'S PRINCIPLE

• WHEN A SYSTEM IN CHEMICAL EQUILIBRIUM IS DISTURBED BY A CHANGE OF TEMPERATUR, PRESSURE OR A CONCENTRATION, THE SYSTEM SHIFTS IN EQUILIBRIUM COMPOSITION IN A WAY THAT TENDS TO COUNTERACT THIS CHANGE VARIABLE
• CHANGING THE REACTION CONDITION:
• CONCENTRATIONS
• PRESSURE
• TEMPERATURE
• CATALYST

CONCENTRATIONS

• REACTANTS >>>>>> PRODUCTS
• When more reactant is added, an equilibrium mixture, net reaction occurs left to right( forward direction) , more products are produce
• When more products is added / some reactants is removed from, an equilibrium, net reaction occurs from right to left, more reactants are produced.

pReSSurE

• Number of moles is independent on the volume
• IF PRESSURE INCREASE, VOLUME DECREASE, FEWER MOLES
• if the pressure increase by decreasing the volume of reaction mixture, the reaction shifts in the direction of fewer moles of gas

TEMPERATURE

• ENdothermic
• REACTANTS + HEAT >>>>>>>>> PRODUCTS
• for this reaction , the amount of products are increased at equilibrium by an increase in temperature.
• EXOthERMic
• REACTANTS >>>>>> PRODUCT + HEAT
• the amounts of products are increased at equilibrium by an decrease in temperature