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Gas Law problem

Kandi
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60 L of a gas were collected over water when the barometer read 670mmHg, and the temp. was 20C. The pressure of H2O vapor at 20C is 17.5 mmHg. What volume would the dry gas occupy at standard conditions? I used the rearranged equation: V2=T2xP1xV1/t1xP2 and got 2329.5 L. Is that correct??Any help would be appreciated.

 

Also, what gas equation is to be used to answer this problem: N2 occupies a volume of 600mL at 60C and 650mmHg of pressure. What will the volume be at STP??

60 L of a gas were collected over water when the barometer read 670mmHg' date=' and the temp. was 20C. The pressure of H2O vapor at 20C is 17.5 mmHg. What volume would the dry gas occupy at standard conditions? I used the rearranged equation: V2=T2xP1xV1/t1xP2 and got 2329.5 L. Is that correct??Any help would be appreciated.

 

Also, what gas equation is to be used to answer this problem: N2 occupies a volume of 600mL at 60C and 650mmHg of pressure. What will the volume be at STP??[/quote']

 

Does it seem reasonable that the gas would occupy almost 40 times the volume at STP? Are the given conditions that different?

 

PV=nRT should work for the second problem.

 

Show some detail of your work and people can give you detailed feedback.

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Thanks, but what equation should I use for the 1st problem?? And if I'm using the Ideal Gas equation for the 2nd one, what am I solving for?

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