00:01
Okay, we are given this reaction right here, and we're asked to calculate delta g, the free energy, under specific conditions.
00:11
So let's find the delta g for the reaction, our standard.
00:20
And this will equal, and i'm going to switch colors here, i'm given my delta g of formation in units of kilojoules per mole as follows.
00:33
Ch4 is ch4.
00:50
Where are my values here? let me go to a thermodynamic data table.
01:01
Okay, ch4.
01:03
I've got to get up to carbon.
01:13
Methane is negative 50 .72.
01:23
And this is zero.
01:26
This is zero.
01:27
And co2 is negative 394 .36.
01:38
Okay, so to get my delta g for my reaction under standard conditions, we will be doing one mole times negative 394 .36 kilojoules per mole plus two times zero.
02:08
And then i will have, make sure this is balanced, minus one mole times, this one should have, no, that was right, 394 is correct, minus one mole times, just happened here, where's my, can't even find my, oh, there it is.
02:53
There we go.
02:55
One mole times negative five zero point seven two kilojoules per mole plus.
03:08
And then i'm good down here.
03:09
One times zero.
03:12
Let me put this into my calculator.
03:14
So i have negative three ninety four point thirty six minus negative five zero point seventy two...