Discuss about le chatliers principle. (5 marks)
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Le Châtelier's principle, chemical principle that states that if a system in equilibrium is disturbed by changes in determining factors, such as temperature, pressure, and concentration of components, the system will tend to shift its equilibrium position so as to counteract the effect of the disturbance (see chemical equilibrium ). For example, at a given temperature a covered beaker partly filled with water constitutes a system in which the liquid water is in equilibrium with the water vapor that forms above the surface of the liquid. While some molecules of liquid are absorbing heat and evaporating to become vapor, an equal number of vapor molecules are giving up heat and condensing to become liquid. If stress is put on the system by raising the temperature, then according to Le Châtelier's principle the rate of evaporation will exceed the rate of condensation until a new equilibrium is established. At the new equilibrium point a greater proportion of molecules will exist in the vapor phase. Le Châtelier's principle is evident in chemical systems, as in the common-ion effect and in buffer solutions (see also separate article on p H). Le Châtelier's principle can be used to encourage formation of a desired product in chemical reactions.
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Le Châtelier's principle, chemical principle that states that if a system in equilibrium is disturbed by changes in determining factors, such as temperature, pressure, and concentration of components, the system will tend to shift its equilibrium position so as to counteract the effect of the disturbance (see chemical equilibrium ). For example, at a given temperature a covered beaker partly filled with water constitutes a system in which the liquid water is in equilibrium with the water vapor that forms above the surface of the liquid. While some molecules of liquid are absorbing heat and evaporating to become vapor, an equal number of vapor molecules are giving up heat and condensing to become liquid. If stress is put on the system by raising the temperature, then according to Le Châtelier's principle the rate of evaporation will exceed the rate of condensation until a new equilibrium is established. At the new equilibrium point a greater proportion of molecules will exist in the vapor phase. Le Châtelier's principle is evident in chemical systems, as in the common-ion effect and in buffer solutions (see also separate article on p H). Le Châtelier's principle can be used to encourage formation of a desired product in chemical reactions.
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❤. Le-Chatlierś principle ❤
⭐.If a chemical rection at equilibrium is subjected to a change in temperature , pressure , or concentration , the equilibrium position shifts in the direction , in which this change is reduced or nullified.
➡FACTORS EFFECTING THE EQUILIBRIUM POSITION :
❤. EFFECT OF CONCENTRATION ❤
- Increase in the concentration of reactants in the reaction mixtures at equilibrium favours forward reaction.
- Decrease in the concentration of reactants in the reaction mixture at equilibrium favours backward reaction.
- Increase in the concentration of products in the reaction mixtures at equlibrium favours backward reaction.
- Decrease in the concentration of products in the reaction mixtures at equilibrium favours forward reaction.
❤. EFFECT OF PRESSURE ❤
- Increase in the pressure of the system at equilibrium , shifts the equilibrium position in that direction in which the volume or the number of moles gets decreased.
- Decrease in the pressure of the system at equilibrium , shifts the equilibrium position in that direction in which the volume or the number of moles gets increased.
❤. EFFECT OF TEMPERATURE ❤
- Increase in the temperature of the system at equilibrium , shifts the equilibirium position in that direction in which temperature is decreased or heat is absorbed.The endothermic reaction is favoured.
- Decrease in the temperature of the system at equilibrium , shifts the equlibrium position in that direction in which temperature is increased or heat is released .The exothermic reaction is favoured.
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