Posted by ian on Monday, November 28, 2011 at 2:34pm.
Did you make a typo? Should the density be 0.804 g/mL?
I have assumed you made a typo and the density of propanol is 0.804 g/mL.
Volume room is 7.5 x 3 x 3 cubic meters. Convert to liters for volume.
Then use PV = nRT and solve for n. That will give you the moles of the gas at the conditions listed. (10.7 torr is what you use for pressure).
Then use density of the propanol to solve for grams, convert to moles. If moles of the liquid exceed moles of the gas, subtract to find moles liquid remaining after vaporization has ceased; i.e., reached equilibrium. If moles gas exceeds moles liquid at start, then all of the liquid will evaporate.
yeah ur right..it should be 0.0804 g/mL..sorry bout that..
dont i have to use 10.7 torr and convert it to atm,then it gives me o.01407..otherwise.my mol is a very big number..
Yes, P must be in atmospheres in PV = nRT. V must be in L. However, n still is a relatively large number, considering you had 10L (10,000 cc) propanol.
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