00:01
Hi, so to solve for this, we need to write our i's table for this.
00:06
I'm going to write the balance equation first.
00:08
Pcl5, this will associate to pcl3 and cl2.
00:16
So our i's table for this, initial change equilibrium concentration.
00:21
The initial concentration, we don't have it yet, but we have the number of moles and then the volume.
00:27
So that means i'm going to calculate here the initial concentration.
00:31
That's going to be 0 .3848 moles over the volume, 4 .50 liters.
00:39
So that's going to be 0 .0855 molar.
00:43
So now we have the initial concentration.
00:45
We're going to write here and the products are zero initially.
00:50
This will lose some amount.
00:52
This will gain plus x plus x.
00:54
At equilibrium, we have 0 .0855 minus x, x and x.
00:59
And how do we solve for the value of x? since that's our unknown, we will use the given kc of the reaction.
01:09
Equilibrium constant is equivalent to the concentration of the products.
01:12
So our products pcl3 and cl2.
01:15
These are concentrations at equilibrium over the initial concentration at equilibrium of the reactants.
01:21
These are equilibrium concentrations.
01:24
Plug in the information that we have.
01:26
Then we have here x squared over 0 .0855 minus x.
01:37
So rearranging this, we'll get 0 .1539 minus 1 .8x...