00:01
Okay, to solve this problem you have to look up the delta h reaction and delta s reaction values from a textbook in order to find them, in order to apply them to the equation.
00:15
Ultimately, the equation that we want to be using is this one, that the delta g is equal to the delta h minus t delta s for your scenario.
00:25
So i'm going to start by finding the delta h.
00:28
To find the delta h of formation, you're going to take the products enthalpies minus the reactants enthalpies.
00:34
So i've looked those up here in a table, and the carbon dioxide's enthalpy was negative 393 .5, and the water's enthalpy was 286 kilojoules per mole.
00:49
So you take the products, you put those together, then you subtract the reactants from them, and the h2co was negative 116, and the o2 is zero.
01:00
So when i put that together, the delta h that i got was negative 564 kilojoules per mole, and that's going to be what goes right here.
01:11
We'll do that same thing with our delta s's.
01:14
Again, do your products.
01:15
So i looked up carbon dioxide, and it was 219, and the water was, i'm sorry, the carbon dioxide was 214.
01:28
Excuse me...