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chapter 5- gases

ap chem chapter 5

QuestionAnswer
Boyles Law (pressure and volume) P1V1=P2V2
Charles' Law (volume and temperature) V1/T1=V2/T2
Avogadro's Law (volume and moles) v1/n1=v2/n2
Gay-Lussac's Law (pressure and temperature) P1/T1=P2/T2
Combined gas law p1v1/n1t1= p2v2/2t2
Ideal gas law PV=nRT
Ideal gas law with molar mass PV=m/mu times RT
Density ideal gas law D=pmu/RT
at STP, 1 mol of gas is 22.4 L
Dalton's Law of Partial Pressures Ptotal= Pa+Pb+Pc...
Mole Fraction the ratio of the number of moles of agiven compenent i a mixture to the total number of moles in the mixure. Xa=moles A/total moles
Gas collection over water Ptotal=Pgas+PvH20
Kinetic Energy of Molecules KE=3/2RT, whereR= 8.31 J/Mol times K
Units for KE J/Mol
Root mean square velocity square root of 3KT over m (in kg) where R is 8.31
Diffusion the mixing of gases
Rate of Diffusion/Effusion r1/r2=square root of mu2/mu1
effusion the passage of a gas through atiny opening into an evacuated chamber
real gases real gases do have volume and IMFS, and re not "ideal"
van der waal's equation taking into account the nonzero size of molecules and the attraction between them.
conitiodns for real gases to behave most like ideal gases low pressure and high temperature
Created by: lilee256
 

 



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