Calc Volume and Temp of gas with changing conditions

AI Thread Summary
To calculate the volume of 18.75 mol of helium gas at 10.0°C and a gauge pressure of 0.035 atm, the ideal gas law (PV=nRT) was applied, but the initial pressure was incorrectly converted to pascals. The correct absolute pressure is 1.035 atm, which should be converted to pascals for accurate calculations. The calculated volume was found to be 3.27 * 10^4 m³, but the book answer is 0.323 m³, indicating a significant error in the pressure conversion. The user has not yet attempted part b, as they need to resolve the volume calculation first. Accurate pressure conversion is crucial for solving gas law problems.
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Homework Statement



If 18.75 mol of helium gas is at 10.0C and a gauge pressure of 0.035atm, calculate a) the volume of the helium gas under these conditions. b) calculate the temp if the gas is compressed to half the voume at a gauge pressure of 1.00atm.


Homework Equations



PV=nRT
P1V1/T1 = P2V2/T2
Tk = Tc + 273
absolute press = gauge press +1atm


The Attempt at a Solution



V=nRT/P = (18.75mol * 8.315 J/mol K * 283K) / 1.35 atm = 3.27 *10^4 m3

Book answer = 0.323 m3

Haven't yet attempted part b, because haven't yet calculated V correctly. Anybody see where I went wrong? Thanks!
 
Physics news on Phys.org
Pressure is in pascals not atm. 1 atm = 101325 Pa.
 

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