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Pressure Force per unit area on a surface Newton SI unit for force; the force that will increase the speed of a one-kilogram mass by one meter per second each second that the force is applied Barometer A device used to measure atmospheric pressure; invented by Torricelli in 1643 Millimeters of mercury Common unit of pressure; symbolized mm Hg; pressure of 1 mm Hg is also called 1 torr in honor of Torricelli Atmosphere of pressure Symbolized atm; exactly equivalent to 760 mm Hg Pascal Converted to kPa; 1 Pa is the pressure exerted by a force of one newton acting on an area of one square meter; standard atmosphere (1 atm) = 1.01325 x 10^5 Pa or 101.325 kPa Partial pressure Pressure of each gas in a mixture Dalton's law of partial pressures The total pressure of a gas mixture is the sum of the partial pressures of the component gases; PT=P1 + P2 + P3... Boyle's law The volume of a fixed mass of gas varies inversely with the pressure at constant temperature; PV=k Absolute zero -273.15 degrees Celcius is given a value of zero in the Kelvin scale; rounded to 273 for calculations Charles's law The volume of a fixed mass of gas at constant pressure varies directly with the Kelvin temperature; V=kT or V/T=k where T=Kelvin temperature and k=constant; V1/T1=V2/T2 Gay-Lussac's law The pressure of a fixed mass of gas at constant volume varies directly with the Kelvin temperature; P=kT or P/T=k or P1/T1=P2/T2 Combined gas law Expresses the relationship between pressure, volume, and temperature of a fixed amount of gas; PV/T=k or P1V1/T1=P2V2/T2 Gay-Lussac's law of combining volumes of gases At a constant temperature and pressure, the volumes of gaseous reactants and products can be expressed as ratios of small whole numbers Avogadro's law Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules; gas volume is directly proportional to the amount of gas at a given temperature and pressure; V=kn where n=amount of gas in moles Standard molar volume of a gas The volume occupied by one mole of a gas at STP is known as the standard molar volume of a gas; 22.41410 L but use 22.4 L Ideal gas law Mathematical relationship among pressure, volume, temperature, and number of moles in gas; PV=nRT where R=constant Ideal gas constant The constant of R; R=PV/nT; see chart on p. 384 Graham's law of effusion The rates of effusion of gases at the same temperature and pressure are inversely proportional to the square roots of their molar masses