given that the ∆H vapor is 40.79 kJ/ mol
and that the ∆H fusion is 6.01 kJ/mol?
I was told to apply Hess' law to this, but I don't understand how it applies...
Thank you for your time!
"...the enthalpy of sublimation is the sum of the enthalpies of vaporization and fusion." See link.
∆H sub = ∆H fus + ∆H vap
Using Hess's Law:
H2O(s) --> H2O(l) ∆H fus = 6.01 kJ/mol
H2O(l) --> H2O(g) ∆H vap = 40.79 kJ/ mol
------------------------------------------------------------ When you add these algebraically you get your answer.
H2O(s) --> H2O(g) ∆H sub = ?
I'll bet you can figure it out from here. Best to you.
none of the above kid. the answer is pi
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"...the enthalpy of sublimation is the sum of the enthalpies of vaporization and fusion." See link.
∆H sub = ∆H fus + ∆H vap
Using Hess's Law:
H2O(s) --> H2O(l) ∆H fus = 6.01 kJ/mol
H2O(l) --> H2O(g) ∆H vap = 40.79 kJ/ mol
------------------------------------------------------------ When you add these algebraically you get your answer.
H2O(s) --> H2O(g) ∆H sub = ?
I'll bet you can figure it out from here. Best to you.
none of the above kid. the answer is pi