00:01
In this problem, we are going to define what is meant by a reaction quotient and specifically how it differs from an equilibrium constant.
00:11
If we have a reversible reaction of reactant a reversibly producing product b, then we know that we can form equilibrium expression for kc based on those equilibrium concentrations of b and a.
00:30
And again, when we are defining this equilibrium constant, both of these concentrations of each one of these species have to be at their equilibrium concentrations.
00:46
Because that defines equilibrium at a given temperature.
00:51
A reaction quotient q is found using that same ratio.
00:58
And again, for this specific reaction, that would be the concentration of product b divided by the concentration of reactant a.
01:07
And the difference between k and q is that either one or both of these concentrations are no longer at their equilibrium concentration values.
01:21
So if we had the system at a certain temperature, and we said that kc is equal to one, and that would mean that the concentration that equilibrium for product b would be one, for example...