What would have been the initial pressure reading of a sample of oxygen gas that started at 25.0 mL in volume and was compressed to 15.0 mL? The final pressure reading was 1.90 atm. (Temperature was kept constant.)
1) 2.43 atm
2) 1.14
3) 1.88
4) 3.17

Question

What would have been the initial pressure reading of a sample of oxygen gas that started at 25.0 mL in volume and was compressed to 15.0 mL? The final pressure reading was 1.90 atm. (Temperature was kept constant.)
1) 2.43 atm
2) 1.14
3) 1.88
4) 3.17

alphadxg · Answer

Well, we would need to use the ideal gas law here, right?. have you tried this yet?

chmvijay · Answer

where P1 is initial pressure and Vi intial volume of gas
P2 is final pressure and V2 is final volume of gas

chmvijay · Answer

since temperature is kept constant it wont make sense :P

alphadxg · Answer

And because temperature isn't mentioned, you can exclude it form the equation. Same goes for the rest of the variables.

chmvijay · Answer

P1V1=P2V2 yaa ur right

anonymous · Answer

Soo 1, 2, 3, 4 haa?

alphadxg · Answer

:)

chmvijay · Answer

LOL :P u find it out now :P

alphadxg · Answer

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So if you get Torr in a problem, like my teacher always did go form torr to atm you would divide by 760.

T - kelvin so if you get C just do (C+273) = K