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thought it was NaCl
Well the heat of vaporization correlates with the melting points. At room temperature Cl2 is a gas and H2O and HCl are both liquids. NaCl is a solid at room temp so wouldn't it have the highest heat of vaporization
oh. I see. so we take room temperature into account?
I noticed I tried looking this up (heat of vaporization for NaCl & wikipedia lmao says it doest have a value)
i did the same thing XD
http://www.pleasanton.k12.ca.us/fhsweb/morris/APchem/ch%2010/Practice%20test%20MC.pdf idk if im allowed to post links but this one has similar compounds and states that NaCl has the highest heat of vaporization look at question 6
I'm coming up with nothing either for NaCl
@sweetburger i saw that problem don't get why though... maybe because it's a solid?
Well at room temp NaCl is a solid where all the others are liquids or gases
but it's heat of vaporization (l) --> (g) not heat of fusion.. don't know why i'm kind of confused.
I dont see how it could not be NaCl. It has a very large molecular mass compared to the other compounds in question except for which Cl2 has a higher mass but NaCl is in a strong lattice and Cl2 just has weak disperson forces holding it together. All together I dont see how NaCl would not have the highest H of Vaporization.
not sure if that logic is completely sound^ but its my attempt to reason
yes its (l)--->(g) and if some of the compounds are already liquids or gases and NaCl is a solid then it would be much harder to turn NaCl into a gas than the other compounds
*at room temperature
yeah your logic makes perfect sense man.. i just didn't understand why there was no value but both of you are right.
It's NaCl for sure.
ok I'm going to post another one
@sweetburger that last point helped me out a lot, like NaCl is a solid so it would be harder to vaporize it.
alright glad it helped :)