Consider this system at equilibrium.
a(aq) < ==> b(aq)
delta h= -550 kl/mol
what can be said about q and k immediately after an increase in temperature?

a) q > k because q increased
b) q > k because k decreased
c) q < k because q decreased
d) q < k because k increased
e) q=k because neither changed

how will the system respond to a temperature increase?

1, shift left
2, shift right
3, no change

Q is the "reaction quotient" and is used to determine which way a given system will move to establish equilibrium. If the initial conditions give a Q which is larger than K, then the equilibrium will move to the left to establish equilibrium. If the value of Q is less than the value of K, then the system will move to the right to establish equilibrium. If Q happens to equal K, then the system is at equilibrium. 
When equilibrium is re-established the value of K will be greater. Temperature changes are the only changes that actually change the value of K.

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