00:01
If our reaction is 2 s .o2 plus o2 gas goes to 2 -3, then the k expression will be equal to the concentration of s -o -3 squared, divided by the concentration of o2 and the concentration of s -o2 squared.
00:31
So if the volume of the equilibrium system was suddenly increased, if we increase the volume, that means all the concentrations are going to decrease.
00:44
But because we've got more concentrations in the denominator, then the decrease here will be more dramatic, resulting in an increase in this ratio.
00:59
So qc, which is going to be the ratio under non -equilibrium conditions, is going to increase.
01:13
If it increases, then after the volume of the system has increased, then qc is going to be greater than kc.
01:23
If qc is greater than kc, then the reaction needs to shift to the left.
01:31
As it shifts to the left, or we would say in the reverse direction, we are going to make more reactant...