CHM 111 Lecture Notes - Lecture 4: Ideal Gas Law, Gas Thermometer, Ideal Gas

• School: University of Miami
• Department: Chemistry
• Course: CHM 111
• Professor: Lewis Nita

Document Summary

Since one mole of an ideal gas occupies 22. 4 l under standard conditions, the density of an ideal gas can be easily calculated under standard conditions. Since density is simply mass/volume, and since the mass of one mole of a gas is simply its molar mass, the density of a gas under standard conditions is given by the following relationship: Notice that the density of a gas is directly proportional to its molar mass. The greater the molar mass of a gas, the more dense the gas. For this reason, a gas with a molar mass lower than that of air tends to rise in air. In any case, we can calculate the density of a gas more generally by using the ideal gas law. For example, we arrange the ideal gas law as follows: Since the left-handed side of this equations has units of moles per liter, it represents the molar density.