Le-Chatelier's principle
Le-Chatelier and Braun (in the year 1884), French chemists, made some generalizations to explain effect of the changes in concentration, temperature or the pressure on the state of system in the equilibrium. When the system is subjected to a change in one of the factors stated above, the equilibrium gets disturbed and system readjusts itself until it returns back to equilibrium. The generalization is termed as Le-Chatelier's principle. It can be stated as follows:
The change in any of the factors which determine the equilibrium conditions of the system will shift the equilibrium in such a manner to reduce or to counteract the effect of change.
The principle is quite helpful in predicting the qualitatively effect of change in concentration, pressure or the temperature on a system in equilibrium.
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Change imposed on the system in equilibrium
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Equilibrium position moves
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Equilibrium constant
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Any other points
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Conc. of A and/or B increased
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To right
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No change
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No change
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Conc. of C and /or D increased
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To left
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No change
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No change
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Pressure increased
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To right if (c+d)<(a+b), i.e. Δn = -ve
To left if (c+d)>(a+b), i.e. Δn = +ve
No change if (c+d)=(a+b), i.e. Δn = 0
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No change
No change
No change
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Very little effect, if any, on reactions in liquid solution.
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Temperature increased
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To left if ΔH = -ve (exothermic)
To right if ΔH = +ve (endothermic)
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Value decreased
Value increased
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Equilibrium achieved faster
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Addition of catalyst
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No change
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No change
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Equilibrium achieved faster
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Table : The effect of varying conditions on the equilibrium a A + b B ? c C + d D, Δn = (c + d) - (a + b)
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