00:01
I think they're assuming standard states here.
00:04
They want to know the difference in the molar enthalpy and the change in internal energy for the synthesis of ammonia.
00:12
Well if we're going to synthesize one mole of ammonia, nh3, we'll do so as a gas with one half a mole of n2 and three halves of a mole of h2.
00:30
So the delta h for the synthesis of ammonia will simply be equal to its delta h of formation.
00:41
So if we go to a table of thermodynamic values, we can look at the delta h of formation of ammonia.
00:50
And in the table i have, the delta h of formation of ammonia is in the gaseous state negative 46 .19 kilojoules per mole.
01:09
Then the change in internal energy is going to be equal to q plus work.
01:18
Well if this process is occurring at constant pressure, which they didn't tell us, but i'll assume that, then delta h is equal to q.
01:30
So to get the change in internal energy, we simply take the change in heat, negative 46 .19 kilojoules, and we add to that the work.
01:44
Well the work that needs to be done will be associated with the change in moles of gas.
01:50
We're going to one mole of gas from two moles of gas...