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