1. Stoichiometry
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Ideal Gas Laws
• Particles are in random motion • Volume occupied by the gas particles are negligible compared to the volume occupied by the gas • particles exert no force of attraction on other gases • no loss of energy occurs between collisions • the average kinetic energy of the particles is directly proportional to the temp (K) of the gas Exceptions - At cold temps, gas particles can stick together
Boyle’s Law
pressure exerted by a given mass of gas at constant temp is inversely proportional to the volume occupied by the gase P1V1 = P2V2
Charles’ Law
At constant mass and pressure, the volume is directly proportional to the temperature V1/T1 = V2/T2
Gay-Lussac’s Law
At constant mass and volume the pressure is directly proportional to temperature P1/T1 = P2/T2
Ideal Gas Equation
PV = nRT P = pressure in Pa ( 1atm = 101000Pa) V = volume in m3 R = Universal gas constant 8.314Jk-1mol-1 Temp in K
Dalton’s Law of Partial Pressures
The total gas pressure is equal to the partial pressures of each individual gas in the mixture Ptotal = P1 + P2 + P3…
Equation for Dilution
C1V1 = C2V2