Chemical Forums
Chemistry Forums for Students => Physical Chemistry Forum => Topic started by: Collegekid on November 30, 2005, 08:58:52 PM
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Two moles of water are allowed to vaporize at 100°C and 1 atm pressure. The heat of vaporization of water at this pressure and temperature is 540 cal/g. Calculate ?U, ?A, ?G, w, q, ?H, and ?S for this process in units of calories. (This is just an example problem that I didn't know how to do.)
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What have you done so far?
Did you search this site? This might help a little:
http://www.chemicalforums.com/index.php?board=6;action=display;threadid=5471
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consider boiling water as an open system,
dH = Q + W = Q + VdP
Constant Pressure (dP=0): dH = Q
H = U + PV
Constant Pressure: dH = dU + PdV
Since at 100C, 1atm, water is at equilibrium, then
?S = Q/T
Mike's link will give you a clue on the value of dG.
To find ?A, try differentiating the expression for A