The ozone layer in the Earth's stratosphere has an average total pressure of 10 mm Hg 11.3 * 10-2 atm2. The partial pressure of ozone in the layer is about 1.2 * 10-6 mm Hg 11.6 * 10-9 atm2. What is the concentration of ozone in parts per million, assuming that the average molar mass of air is 29 g/mol?

Partial pressure refers to the pressure exerted by a single component of a gas mixture. In the context of the ozone layer, it helps determine the contribution of ozone to the total atmospheric pressure. Understanding partial pressure is crucial for calculating the concentration of gases in a mixture, as it allows us to isolate the behavior of individual gases.

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). For air, the average molar mass is approximately 29 g/mol, which is essential for converting between mass and moles in gas calculations. This concept is vital when determining the concentration of a gas in a mixture, as it relates the mass of the gas to its volume and number of moles.

Parts per million (PPM) is a unit of measurement used to describe the concentration of a substance in a solution or mixture. It indicates how many parts of a substance are present in one million parts of the total mixture. In the context of the ozone concentration, converting the partial pressure of ozone to PPM allows for a standardized way to express its abundance in the atmosphere, facilitating comparisons and assessments of air quality.