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The pressure exerted on a 240.0 mL sample of hydrogen gas at constant temperature is...

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hennyyyx3 | Student, Grade 10 | eNoter

Posted June 11, 2013 at 5:01 PM via web

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The pressure exerted on a 240.0 mL sample of hydrogen gas at constant temperature is increased from 0.428 atm to 0.724 atm. What will the final volume of the sample be?

I'm not sure which law to use for this, and I don't know whether to use V1, V2, T1, T2, P1, or P2 for this question. Pleaseee help if you can! 

 

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jeew-m | College Teacher | (Level 1) Educator Emeritus

Posted June 11, 2013 at 6:00 PM (Answer #1)

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Since the temperature is constant we can use Boyle's law here. It says that when temperature is constant an ideal gas would have its pressure(P) inversely proportional to volume(V). In other words;

PV = constant

 

So applying Boyle's law to the two situations will give you;

`P1V1 = K`

`P2V2 = K`

 

`P1V1 = P2V2`

`240xx428 = 724xxV2`

`V2 = 141.88`

 

So the final volume of gas is 141.88ml.

 

Assumption

`H_2` act as a ideal gas.

Sources:

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hennyyyx3 | Student , Grade 10 | eNoter

Posted June 11, 2013 at 6:03 PM (Reply #1)

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I got it! Thanks so much (: 

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