Relate number of particles and volume using Avogadro’s principle. mole: an SI base unit used to measure the amount of a substance; the amount of a pure substance that contains 6.02 × representative particles Relate the amount of gas present to its pressure, temperature, and volume using the ideal gas law. Compare the properties of real and ideal gases. Distinguish between molar mass and Avogadro’s number.

Section 13.2 The Ideal Gas Law (cont.) Avogadro’s principle molar volume ideal gas constant (R) ideal gas law The ideal gas law relates the number of particles to pressure, temperature, and volume. STP means standard temperature & pressure) Standard Temperature = 0 o C Standard Pressure = 1 atm

Avogadro's Principle Avogadro’s principle states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles.Avogadro’s principle

The molar volume of a gas is the volume 1 mol occupies at 0.00°C and 1.00 atm of pressure.molar volume 0.00°C and 1.00 atm are called standard temperature and pressure (STP). Write a conversion factor to convert between moles & liters. When can you use this conversion factor? At STP, 1 mol of gas occupies 22.4 L. Avogadro's Principle

The Ideal Gas Law Ideal gas particles occupy a negligible volume and are far enough apart to exert minimal attractive or repulsive forces on each other. Combined gas law to ideal gas law What is a constant?

The Ideal Gas Law (cont.) The ideal gas constant is represented by R and is Latm/molK when pressure is in atmospheres.ideal gas constant The ideal gas law describes the physical behavior of an ideal gas in terms of pressure, volume, temperature, and amount.ideal gas law PV= nRT This is the form that I will always use in class

The Ideal Gas Law (cont.) Calculate the ideal gas constant using bars as the unit of pressure.

The Ideal Gas Law—Molar Mass and Density Molar mass and the ideal gas law

The Ideal Gas Law—Molar Mass and Density (cont.) Density and the ideal gas law How are molar mass and density related concepts?

Real Versus Ideal Gases Ideal gases follow the assumptions of the kinetic-molecular theory. Ideal gases experience: – There are no intermolecular attractive or repulsive forces between particles or with their containers. – The particles are in constant random motion. – Collisions are perfectly elastic. – No gas is truly ideal, but most behave as ideal gases at a wide range of temperatures and pressures. Give examples of gases behaving as real gases.