equilibria
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what is dynamic equilibrium?
dynamic equilibrium exists in a closed system where the rate of the forwards reaction is equal to the rate of the reverse reaction, and the concentrations of reactants and products remain constant
why does adding a catalyst not affect the position of equilibrium?
the rate of the forwards and reverse reaction is increased equally so the position does not change
Le Chatelier’s Principle
when a system in equilibrium is subject to an external change, the system readjusts itself to minimise the effect of that change
Effect of concentration changes on equilibrium
increase in conc. of products = p.o.e shifts to reactant side so more reactants formed increase in conc. of reactants = p.o.e shifts to product side so more products formed
effect of temperature changes on equilibrium
temp increases = p.o.e shifts to endothermic side (so temp decreases) temp decreases = p.o.e shifts to exothermic side (so temp increases)
effect of pressure on equilibrium
increase pressure = shift towards side with fewer gas moles decrease pressure = shift towards side with more gas moles
Kc equation
2A + 3B <—> C + 4D [products]/[reactants] [C][D]^4 / [A]^2[B]^3
predictions from magnitude of Kc
Kc value of 1 = p.o.e halfway between reactants and products Kc < 1 = p.o.e towards reactants Kc > 1 = p.o.e towards products