00:01
Okay, so in this problem we are given a reversible reaction and we are told that we introduce two moles of no and one mole of co2 into a one liter flask.
00:12
And then we're asked what will be the concentrations at equilibrium.
00:16
So for that we can do an ice table for this reaction.
00:21
And the ice table stands for initial concentrations, the change in those concentrations, and the final equilibrium concentrations.
00:32
For those species.
00:35
So if we look at the problem we are told that we place two moles of no and one mole of co2 in a one liter flask.
00:45
Now two moles in one liters, so if we look at the initial concentration of co2, is going to be two moles in one liter.
00:56
And that is a two, i'm sorry for this was for one mole for chloride, for co2.
01:03
One mole in one liter and that equals to a one molar concentration in molarity.
01:10
One molar concentration.
01:13
For no we are given two moles in one liter and that equals a two molar concentration.
01:21
And we are not told anything about nocl so we can assume that the initial concentration of nocl in this problem is zero.
01:29
So those are going to be my initial concentrations for the three species.
01:33
Zero, two molar for no and one molar for co2.
01:39
Now the change, since we're starting with no and cl and we have no nocl, we are going to know that the reactions are actually going to occur towards the left.
01:52
So we're going to produce nocl and therefore we're going to lose some no.
01:57
So we can say that the change for no is going to be minus 2x because we have two moles in the reaction for the balanced reaction and two mole coefficient.
02:08
For cl2 is going to be minus x because we have a one coefficient in the reaction...