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A certain liquid has a vapor pressure of 92.0 Torr at 23.0 °C and 313.0 Torr at 45.0 °C. Calculate the value of ΔH°vap for this liquid. Calculate the normal boiling point of this liquid. How would I do this? Please help

Chemistry
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Should you use Clausius-Clapeyron equation?
do I just solve for T2 and use the same values?

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Other answers:

Well, let the normal boiling point be T2
wouldn't that just give me the T that is given in the question ?
Nope. Sorry :/ I suck at explaining chemistry
i just get a very small number
What did you get for ΔH°vap?
im not good at chemistry but let's try
43.55 kj/mol
I used \[\log\frac{ P2 }{ P1 }=\frac{ ΔH }{2.303R }*(\frac{ 1? }{ T1 }-\frac{ 1 }{ T2 })\]
Erase the ?
what is v?
I got 49.78kj
Lol. I don't know if i'm right. Ignore me :))
volume i dont know if that's right , it's been i while i dont see chemistry
lol
sing those number? i dont have V so i dont think i can use that
You saw my equation?
yea
Have you tried it?
yea...and i got 43.55...its ok..i will do the question tmr...im just really tired now
Okies. Just close this question ^_^

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