CHEM 210 1nd Edition Lecture 19 Outline of Last Lecture I. Ideal Gas LawII. Density of a GasOutline of Current Lecture III. Mixtures of GasesIV. Dalton’s Law of Partial PressuresV. Kinetic Molecular Theory of GasesCurrent LectureGaseous mixtures are always homogeneous. They are uniformly mixed throughout. A gas in a mixture behaves as if it were the only gas present. Dalton’s Law of Partial Pressures states that the total pressure equals the sum of all of the pressures. The total moles is equal to the sum of all the moles as well. The mole fraction is equal to the number of moles of the gas, divided by the total number of moles. Ptotal = p1 + p2 + p3…..Ntotal = n1 + n2 + n3…..X1 = n1/ ntotal (x stands for mole fraction)Pressure is due to the collisions of the gas particles hitting the walls of the container.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.Kinetic Molecular Theory of GasesThe kinetic molecular theory of gases includes Boyles, Charles and Avogadro’s laws. If the temperature of a gas is increased, the pressure increases as well. This is because increased pressure means increased number of collisions, which means more kinetic energy. This follows Charles Law that states that pressure is directly proportional to temperature. If the number of moles of the gas is increased, there are more particles floating around which means more collisions, more kinetic energy and eventually more pressure. This follows Avogadro’s Law which states that volume is directly proportional to the number of moles. When the volume decreases, the pressure increases because the gasses have less space to move around, which results in more collisions. This refers to Boyle’s Law which states that volume is inversely proportional to the
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