A cylinder of compressed gas rolls off a boat and falls to the bottom of a lake. Eventually it rusts and the gas bubbles to the surface. A chemist collects a sample of the gas with the idea of trying to identify the gas. The wet gas collected occupies a volume of 291 mL at a pressure of 802 torr and temperature of 28.0oC. The vapor pressure of water at 28.0oC is 0.0372 atm.
1. Calculate the volume (L) that the gas occupies after it is dried (the water vapor removed) and stored at STP.
I tried P1v1=p2v2 so (802 torr/760 torr)*(291ml/1000 ml)=((802/760 torr)-.0372)v2 and solve for v2. this was wrong....help please?
1. Calculate the volume (L) that the gas occupies after it is dried (the water vapor removed) and stored at STP.
I tried P1v1=p2v2 so (802 torr/760 torr)*(291ml/1000 ml)=((802/760 torr)-.0372)v2 and solve for v2. this was wrong....help please?
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0.0372 atm = 28.27 torr
(291 mL) x (273.15 / (28.0 + 273.15)) x ((802 - 28.27)/ 760) = 269 mL = 0.269 L
(291 mL) x (273.15 / (28.0 + 273.15)) x ((802 - 28.27)/ 760) = 269 mL = 0.269 L