00:01
Okay, so let's go ahead and start setting this information up.
00:03
It appears we have to do quite a bit of conversions here.
00:06
So we have one gram of hydrogen gas.
00:09
We need to change that to moles and then change that to molarity.
00:14
So we'll take one divided by two and then divided by the 0 .5, which takes us back to one molar.
00:22
So i'm going to just change this to one molar.
00:26
And then for our h2s that's 1 .06 grams divided by 34 sorry and then i'm going to take that divided by 0 .5 because that's how many liters we have and so our molarity of this is 0 .0624 molar okay we have none of the s2 so that means that our change this is going to be plus 2x and this this is going to be plus x and this is going to be minus 2x.
01:00
Okay, we are told that at equilibrium we have this 8 times 10 to the negative 6 moles of the s2 that is produced.
01:10
So we'll take 8 ee negative 6 divided by 0 .5 and that's our molarity which is, i'm going to erase all of this.
01:23
And so our equilibrium concentration is 1 .6 times 10 to the negative fifth.
01:29
Okay, so we now know that is x.
01:32
So that got kind of out of place there.
01:36
So when i take that times 2 and add it, then take 0 .0624 minus 2 times that value, you, i get 0 .062368.
02:00
I'm just going to put them all in there because it's not changing very much.
02:05
This is such a small amount.
02:06
And then 1 .6 times 10 to the negative fifth times two plus one equals equals 1 .000432.
02:23
Okay, i know that's really obnoxious.
02:25
We wouldn't know it out to that many sig figs.
02:28
But from this, we can find our kc value...