00:01
To calculate the equilibrium constant from delta g, we need to know the relationship between delta g and the equilibrium constant.
00:09
This is expressed as delta g is equal to negative rt natural log k.
00:15
Or if you rearrange this, the k, the equilibrium constant, will be equal to e to the negative delta g over rt.
00:24
So for the first chemical reaction, 2n02 goes to 1 and 204.
00:30
With a delta g value of 99 .8 kilojoules per mole.
00:38
I'm sorry, a delta h value of 99 .8 kilojoules per mole.
00:42
We can calculate delta g by taking delta h minus, sorry, let me back up.
00:53
We'll calculate delta g not using the delta h minus t delta s, but by simply using standard delta gs of formation from the back of the book.
01:02
So we'll take the delta g of formation of n204, minus 2 times the delta g of formation of no2, and we'll get delta g of the reaction of negative 2 .8 kilojoules, or negative 2 ,800 joules.
01:17
When using this equation, our delta g value needs to have units of joules rather than kilojoules...