Could someone help me with this chemistry problem dealing with partial pressure of gases?
I've tried this problem numerous times, and i can't seem to get the right answer. I may be missing a step or something. I'd really appreciate an explanation.
Two gases are contained in gas bulbs connected by a valve. Gas A is present in a 1 liter bulb at a pressure of 967 torr. Gas B exerts a pressure of 276 torr in a 1 liter bulb. The valve is opened and the two gases equilibrate. What is the partial pressure of gas A expressed after equilibration. Answer in units of torr. I need some help with the process involved with this problem. Thanks
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In boyle's law he states that if the temperature remains constant absolute pressure of a given mass of gas is inversely proportional to the volume.
PV = k
For the two occasions if we assume that the temperature remains constant from Boyle's law to gas A;
P1V1 = P2V2
At initial state pressure and volume is given. At the second state since the valve is open the volume will become 2L.
967*1 = P2*2
P2 = 483.5torr
So the partial pressure of the gas will be 483.5 torr
- The temperature remains constant in the whole process
- Gasses show ideal gas behavior
- There is no reaction between gasses when they mix
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