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Boyle's Law
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PinitialVinitial=PfinalVfinal
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Charles's Law
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Vi÷Ti = Vf÷Tf
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Combined Gas Law
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PiVi÷Ti = PfVf÷Tf
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Avogadro's Law
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Vi÷ni=Vf÷nf
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Ideal Gas Law
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PV=nRT
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Dalton's Law of Partial Pressure
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Ptotal=P1+P2+P3...
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Partial Pressure
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Pgas(atm)=(total pressure x molesgas)÷total moles
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PP when volumes are different
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Ptotal=P1(atmxV1÷Vtotal)+P2(atmxV2÷Vtotal)...
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Mole fraction
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moles of gas ÷ total moles
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Wet Gas
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Pwet gas=Ptotal-PH2O
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then use PV=nRT to solve for variables
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Van der waal's equation
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P=[(nRT)÷(V-nb)] - [(a*n2)÷(V2)]
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When comparing real gases
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a gas with a larger "a" value will require the largest correction to account for intermolecular forces
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a gas with a smaller "b" value will behave most ideally at high pressures
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If Vdw's pressure is lower than the ideal pressure, attractive forces dominate
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If Vdw's pressure is higher than ideal pressure, repulsive forces dominate
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Real Gas Behavior
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attractive forces between molecules cause a decrease in pressure
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As molecules increase in size deviations from ideal behavior become apparent at relatively HIGH temps
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In general, most gases behave most ideally at HIGH temps and LOW pressures
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1 atm=
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1 atm (R= .08206)
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760 mmHg (R= 62.364)
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760 torr
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1.013x105 Pa
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101.3 kPa
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29.92 inches Hg
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14.69 psi
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1.01325 bar
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Mole ratio = Volume ratio
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2A+3B=AB
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2A:3B
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2mL A:3mL B
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Temperature
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If temperature is increased, Pressure and KE increase by a factor of Tf÷Ti and rms increases by a factor of √Tf÷Ti
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Volume
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If volume is increased, Pressure increases by a factor of Vi÷Vf while KE and rms increase by a factor of 1 (because they are not affected))
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Moles
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If moles are increased, pressure increases by a factor of nf÷ni, while KE and rms increase by a factor of 1 (no change)
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Ideal Gas Law
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PV=nRT
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STP
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0 degrees celcius, 273 degrees Kelvin, 1 atm, 22.4 L/mol
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Density
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d=MP÷RT where M is molar mass
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Volume
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When not given volume, but told to assume ideal gas behavior, use V=1L
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G1=gas 1
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G2=gas 2
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Average Kinetic Energy
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KEG1 = KEG2 when TG1=TG2
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Molecular Speed
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√u2 = √3RT÷M where M is the molar mass
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√u2G1 ÷ √u2G2 = √MG2 ÷ √MG1
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Rate
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d/dx G1 ÷ d/dx G2 = √MG2 ÷ √MG1
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Time
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tG2 ÷ tG1 = √MG2 ÷ √MG1
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