4b - More Gas Problems

4b - More Gas Problems - More Gas Problems Tro Problem 5.48...

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    More Gas Problems
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    Tro Problem 5.48 A 1.0 L container of liquid nitrogen is kept in a  closet measuring 1.0 m by 1.0 m by 2.0 m.   Assuming that the container is completely full,  that the temperature is 25.0 C, and that the  atmospheric pressure is 1.0 atm, calculate the  percent (by volume) of air that would be  displaced if all of the liquid nitrogen evaporated.   [Liquid nitrogen has a density of 0.807 g/mL]
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    Volume displaced If you release a second gas into a room, there are  two options: either the pressure increases (more  moles!) or some of the air in the room escapes.    Unless the room is airtight and sealed, some of the  air will escape because the pressure in the room  wants to be the same as the pressure outside.
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    Volume of air The air fills the closet. V closet  = l x w x h = 1.0 m x 1.0 m x 2.0 m          = 2.0 m 3 Is this a good unit? It’s the BEST UNIT!!!  It’s the SI unit!! (But we’d  probably rather have L   )
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    Volume of air The air fills the closet. V closet  = 2.0 m * (100 cm)   3*  1 mL  * 1 L                           (1m) 3         1 cm 3   1000 mL V closet  = 2000 L
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    How much Nitrogen? I’m sure many of you are tempted to say 1.0 L. 1.0 L is the volume of LIQUID nitrogen.  (Which  means there’s really only 1999 L of air in the  room!) We need to know how much GASEOUS nitrogen  is formed when the liquid evaporates.
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    1.0 L of liquid is ??? Gas? ???? PV = nRT What do we know? We know the R, T, P for sure. We want to know V So we need to know n.
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    Finding n We know the volume of the liquid and its density,  so we know… …the mass of the liquid which is the same as… …the mass of the gas, which can be used to find… …the moles of gas, by using… …the molar mass!
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4b - More Gas Problems - More Gas Problems Tro Problem 5.48...

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