Equilibrium
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Forward reaction
Initially reactants are used up but then slow as their concentration drops
Dynamic equilibrium
Rate of forwards reaction = backwards Conc of each substance remains constant - only in a closed system Backward reaction - initially reactants are reformed slowly but then speed up as conc of products increases
Le chateliers principle
If a reaction at equilibrium is subjected to a change in pressure, temperature or concentration, the position of equilibrium will move to counteract the change
Change in condition resulting in shift to left
Make more reactants
big value for Kc
higher conc of B so, position of equilibrium is to the right (forward reaction favoured)
increasing reactant concentration
equilibrium shifts to the right to use it up and reduce concentration more products produced
increasing pressure
equilibrium shifts to side with fewest number of gas particles to reduce pressure
increasing temp
makes equilibrium shift to endothermic direction to reduce temp more reactants produced
catalysts
have no effect on position of equilibrium will speed up rate of forward and backward reaction equally