Question

What's the unit for enthalpy?

Answer 1

MY textbook is being mean, so I can't remember what the unit for enthalpy is (for a reaction at equilibrium, if that clarifies anything). I'm thinking between kJ/mol, kJ*mol and J/mol. The data I'm given is T, in degrees Celsius, and Keq (uM), from a chart.

Answer 2

The unit for enthalpy is joules or J.
Enthalpy is the transfer of heat.

Answer 3

I should have specified, this is true when it is deltaH too?

Answer 4

It can be written as H or delta H
Delta H would mean enthalpy change as H would be enthalpy.
\[\Delta H= H _{2}-H _{1}\]
\[\Delta H= 32.76J\]

Answer 5

Ah, so units are the same regardless? In what situations would I consider using kJ/mol, or J/mol? I've seen that in some instances in the practice problems in the later chapters, but I don't understand why its like that.

Answer 6

It can be written as \[32.76 J/mol\] in a chemical reaction.

Answer 7

I was about to state that.

Writing it as J/mol would mean solving for the amount of heat the product transferred or released during the chemical reaction.

Answer 8

Or you want to know the mass per 1 joule of enthalpy change.

Answer 9

It is quite simple really.
You do not need to understand the concept deeply.

Answer 10

For example: http://openstudy.com/study#/updates/55f89467e4b0a91f39321a0f

Answer 11

I'm just working through making a graph for the van't Hoff equation.

Answer 12

So for -deltah/(RT), I was suppose to give the units of both delta H, and -deltah/(RT)

Answer 13

Yes.

Answer 14

sorry, afk. washroom

Answer 15

Do you know the units for that?

Answer 16

I got to go so,

R is (Joules) (Kelvin)^-1 (mol-)^1
-Delta H is J/mol
T is temperature in Kelvins (K)
So the units are obtained by canceling

\[\frac{ Joules }{ mol \times mol ^{-1}\times K ^{-1} \times Joules \times K }\]
\

Answer 17

=\[\frac{ Joules \times mol \times K }{ Joules \times mol \times K }=1\]
So no units at all.

Answer 18

Just thought I'd add a little more, when you do an experiment at constant pressure and there's heat released or absorbed, the amount of heat is dependent on how much stuff you have. Enthalpy is an extensive property, which means it depends on how much stuff you have. Extensive properties aren't generally very useful to think about. It's like if I weigh some gold, it depends on how much of it I have, I would never write down "5 pounds of gold" in a text book for students to learn because it depends on the gold chunk I felt like picking up that day.

However the density of gold is what's called an intensive property. We've said that now the mass per amount you have is what doesn't change, which is actually useful. I can weigh my gold to find out how much volume it has or find out how much volume it displaces to figure out how much mass it has, which might actually be important to do something.

Wait what does this have to do with enthalpy? Well like I was saying, on its own Enthalpy changes aren't that interesting since the heat depends on how much stuff you have. So if you divide out the number of particles you used, you'll get a kind of "density" like property, an intensive property called the molar enthalpy. These are the kinds of values you can look up in a book too.

Answer 19

Thanks Woodward