Chem 1061 1st Edition Lecture 11Outline of Last Lecture I. Gases and Kinetic Molecular Energya. Identity of GasII. Gas Pressure and measurement a. Measuring Gas Pressureb. Units of PressureIII. Gas Laws and Their Experimental Foundationsa. Boyle’s Lawb. Charles’ LawOutline of Current LectureIV. TemperatureV. Avogadro’s LawVI. Gas Behavior and Standard Conditionsa. Standard Temperature and Pressureb. Standard Molar VolumeVII. Ideal Gas LawVIII. Applications of Ideal Gas LawCurrent LectureNote on TemperatureMUST use Kelvin (K) scale for gas calculations.These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.Table 1.6 and Figure 1.11 have more on the difference of temperatures.Fahrenheit (Degree F)Celsius (Degree C)Kelvin (K)We primarily use Celsius and Kelvin for Chemistry.Avogadro’s LawVolume is proportional to amount (In mol). (Pressure and Temperature are constants)Figure 5.7 and 5.19 are diagrams and information about experimental aspect of figuring out thislaw.An increase in n (mol), results in an increase in V When there is the same n, there is the same volume.At the same temperature, gases have the same kinetic energy (?)Gas Behavior and Standard ConditionsStandard Temperature and Pressure (STP)0 degree C (273.15 K) and 1 atm (760 torr)Standard Molar Volumevolume of 1 mol of ideal gas = 22.4 LIdeal Gas LawCombines the relationships.Boyle’s – V proportional to 1/PCharles’ – V proportional to TAvogadro’s – V proportional to nV is proportional to nT/P PV=nRTR is a universal constant. R=0.0821 atm*L/mol*KNOTE THE UNITS ON R.When some variables are constant and there is a change in one variable, the ideal gas law simplifies.Applications of Ideal Gas Law1) Density of a Gas2) Molar Mass of a Gas3) Partial Pressure of a Gas in a Mixturea. Collecting Gases over H2O4) StoichiometryDensity of a GasDensity = Mass/Volume = g/LIdentity of the gas matters…why? Density is proportional to molar mass!PV=nRT (PV=[mass/molar mass]RT)Rearrange the variables and you get…(molar mass)P/RT = Mass/V = DensitySo density is proportional to molar mass. The density of a heavier gas is
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