Download All Gas Laws in a Cheat Sheet and more Cheat Sheet Chemistry in PDF only on Docsity! Gas Laws Cheat Sheet STP is 1 atm and 0°C K = 273 + °C (Change ALL temperatures to Kelvin!!!!) 1 atm = 760 mmHg or 760 torr 1000 mL=1 L 1 atm = 101.3 kPa Molar Volume of a Gas at STP 22.4 L/mol V1 = initial volume Boyle’s Law V1P1 = V2P2 V2 = final volume P1 = initial pressure P2 = final pressure Charles’s Law V1 = V2 T1 = initial temperature (in Kelvin) T1 T2 T2 = final temperature (in Kelvin) n1= initial moles Gay-Lussac’s Law P1 = P2 n2 = final moles T1 T2 Moles and Volume Law V1 = V2 n1 n2 Combined Gas Law V1P1 = V2P2 n1T1 n2T2 Ideal Gas Law PV = nRT P = pressure in atm, kPa, or mmHg (Make sure you pick correct R!) V = volume in liters n = number of moles T = temperature in Kelvin Ideal Gas Constant = R = 0.0821 L • atm = 8.31 L • kPa = 62.4 L • mmHg mol • K mol • K mol • K (Pressure)(volume) = (moles)(ideal gas constant)(temperature) Daltons Law PT = P1 + P2 + P3 + ……. PT = total pressure P# = the partial pressures of the individual gases Total Pressure of a Gas = (Sum of the partial pressures of the component gases) Daltons Law applied to Gases Collected by Water Displacement Patm or PT = Pgas + PH2O Patm or PT = barometric pressure or total pressure Pgas = pressure of the gas collected PH2O = vapor pressure of water at specific temperature (table below also on page 899 in textbook) Water – Vapor Pressure Temperature (ºC) Pressure (mmHg) Temperature (ºC) Pressure (mmHg) Temperature (ºC) Pressure (mmHg) Temperature (ºC) Pressure (mmHg) 0.0 4.6 21.0 18.6 27.0 26.7 50.0 92.5 5.0 6.5 22.0 19.8 28.0 28.3 60.0 149.4 10.0 9.2 23.0 21.1 29.0 30.0 70.0 233.7 15.0 12.8 24.0 22.4 30.0 31.8 80.0 355.1 18.0 15.5 25.0 23.8 35.0 42.2 90.0 525.8 20.0 17.5 26.0 25.2 40.0 55.3 100.0 760.0 Graham’s Law Rate of diffusion/effusion of A = √(MB / MA) M = molar mass of that compound Rate of diffusion/effusion of B Gas A is the lighter, faster gas Rate of diffusion/effusion is the same as the velocity (or speed) of the gas. After the rates of diffusion/effusion for two gases are determined, the gas with the lower molar mass will be the one diffusing/effusing faster.
