Sooooooooo, did you ever think we were done with the mole?
DON'TTHINK THAT WAY because I'm about to prove you wrong.
Enthalpy calculations=the usage of MOLES -insert dramatic scream-
And the return of the mole also means the return of sig figs, btdubs. -insert double dramatic scream-
That my friends was a double double, double double combo. (:
Let's get started:
ΔH--> change in energy of a reaction; expressed in kJ/mol
Here is an example:
1 mol C10H8
12 mol O2
10 mol CO2
4 mol H2O
Once you've identified these, it will be easy to do conversions.
eg. Calculate how many grams of O2 would be needed to produce 1500kJ of energy.
-1500kJ x 12 mol O2 x 32g = 1321.1 kJ
-436kJ 1 mol
**SIG FIGS!!** So, the answer is 1300 kJ.
Watch this video if you're still confused!!
GOOD LUCK WITH THIS CONFUSING SECTION!! :D
Written by Jialynn.