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chem200 gases cheat sheet to use when studying
Gas LawsBoyle's Law | PinitialVinitial=PfinalVfinal | Charles's Law | Vi÷Ti = Vf÷Tf | Combined Gas Law | PiVi÷Ti = PfVf÷Tf | Avogadro's Law | Vi÷ni=Vf÷nf | Ideal Gas Law | PV=nRT | Dalton's Law of Partial Pressure | Ptotal=P1+P2+P3... |
Dalton's Law of Partial PressurePartial Pressure | Pgas(atm)=(total pressure x molesgas)÷total moles | PP when volumes are different | Ptotal=P1(atmxV1÷Vtotal)+P2(atmxV2÷Vtotal)... | Mole fraction | moles of gas ÷ total moles | Wet Gas | Pwet gas=Ptotal-PH2O | | | then use PV=nRT to solve for variables |
Real GasesVan der waal's equation | P=[(nRT)÷(V-nb)] - [(a*n2)÷(V2)] | When comparing real gases | a gas with a larger "a" value will require the largest correction to account for intermolecular forces | | | a gas with a smaller "b" value will behave most ideally at high pressures | | | If Vdw's pressure is lower than the ideal pressure, attractive forces dominate | | | If Vdw's pressure is higher than ideal pressure, repulsive forces dominate | Real Gas Behavior | attractive forces between molecules cause a decrease in pressure | | | As molecules increase in size deviations from ideal behavior become apparent at relatively HIGH temps | | | In general, most gases behave most ideally at HIGH temps and LOW pressures |
| | Pressure Units and Conversions1 atm= | 1 atm (R= .08206) | | | 760 mmHg (R= 62.364) | | | 760 torr | | | 1.013x105 Pa | | | 101.3 kPa | | | 29.92 inches Hg | | | 14.69 psi | | | 1.01325 bar |
Stoichiometry and GasesMole ratio = Volume ratio | 2A+3B=AB | | | 2A:3B | | | 2mL A:3mL B |
Kinetic Molecular TheoryTemperature | If temperature is increased, Pressure and KE increase by a factor of Tf÷Ti and rms increases by a factor of √Tf÷Ti | Volume | 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)) | Moles | If moles are increased, pressure increases by a factor of nf÷ni, while KE and rms increase by a factor of 1 (no change) |
| | Using Ideal Gas Law to Calculate Gas PropertiesIdeal Gas Law | PV=nRT | STP | 0 degrees celcius, 273 degrees Kelvin, 1 atm, 22.4 L/mol | Density | d=MP÷RT where M is molar mass | Volume | When not given volume, but told to assume ideal gas behavior, use V=1L |
Diffusion and EffusionG1=gas 1 | G2=gas 2 | Average Kinetic Energy | KEG1 = KEG2 when TG1=TG2 | Molecular Speed | √u2 = √3RT÷M where M is the molar mass | | | √u2G1 ÷ √u2G2 = √MG2 ÷ √MG1 | Rate | d/dx G1 ÷ d/dx G2 = √MG2 ÷ √MG1 | Time | tG2 ÷ tG1 = √MG2 ÷ √MG1 |
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