Le Chatelier's Principle?

Question

concentration, temperature, volume, and total pressure

i only get how it shifts when dealing with pressure, but for the rest (concentration, temperature, and volume) i don't get how it shifts....mind explaining?

Answer 1

In 1884, the French Chemist Henri Le Chatelier suggested that equilibrium systems tend to compensate for the effects of perturbing influences.
When a system at equilibrium is disturbed, the equilibrium position will shift in the direction which tends to minimise, or counteract, the effect of the disturbance.

If the concentration of a reactant is increased, the equilibrium position shifts to use up the added reactants by producing more products.

If the pressure on an equilibrium system is increased, then the equilibrium position shifts to reduce the pressure.

If the volume of a gaseous equilibrium system is reduced (equivalent to an increase in pressure) then the equilibrium position shifts to increase the volume (equivalent to a decrease in pressure)

If the temperature of an endothermic equilibrium system is increased, the equilibrium position shifts to use up the heat by producing more products.

Check out the link for more information,

Answer 2

Fairly simple principle, if you "add" anything, it will be "consumed". This means, in an equilibrium of:
NaCl(s) <-> Na+ Cl-

If more NaCl(s) is added, then the equilibrium will "shift" to make more Na and Cl ions (products).

For temperature, that is dependent on the reaction, whether it is EXO or ENDO -thermic. If the reaction is "- (delta) (temp)" its exothermic, and heat is a PRODUCT. So if you added heat to a exothermic reaction, the equilibrium would shift to the left in order to consume that heat. If heat is taken away, then the equilibrium would shift to the right in order to produce more heat (and consequently more products).

As for volume, well its just the opposite of pressure. Increase of pressure = reduction in volume.
Increase in volume = reduction of pressure.

Answer 3

It depends on the nature of the equilibrium.