00:01
Alright, so we have some statements about internal energy and how it relates to heat and work under different pressure and volume conditions.
00:10
So, the internal energy is equal to the sum of the heat and the work and the work is the negative pressure times the change in volume.
00:17
So, if we have constant volume, which means the change in the volume, delta v, is equal to zero, then w, which is pressure times the change in volume, is equal to zero.
00:32
So, then plugging in for that, the internal energy is equal to the heat, q.
00:39
We also know that the enthalpy change, delta h, is going to be equal to q at constant pressure.
00:56
And if we have a non -constant pressure, which we're considering here, then delta h is equal to delta u plus the volume times the change in pressure.
01:10
So, delta h here would be equal to, delta u is equal to q.
01:15
So, q plus volume times the change in pressure, or delta u plus something.
01:33
So, delta h is greater than delta u.
01:39
It's a value of delta u plus some positive term.
01:48
Okay, so if the reaction occurs at constant volume, delta u greater than delta h, that's false...