1. The ideal gas law relates the number of particles to pressure, temperature, and volume. Section 2: The Ideal Gas Law K What I Know W What I Want to Find Out L What I Learned

2. 9(A) Describe and calculate the relations between volume, pressure, number of moles, and temperature for an ideal gas as described by Boyle's law, Charles' law, Avogadro's law, Dalton's law of partial pressure, and the ideal gas law. 9(C) Describe the postulates of kinetic molecular theory. 2(I) Communicate valid conclusions supported by the data through methods such as lab reports, labeled drawings, graphs, journals, summaries, oral reports, and technology–based reports. 3(A)In all fields of science, analyze, evaluate, and critique scientific explanations by using empirical evidence, logical reasoning, and experimental and observational testing, including examining all sides of scientific evidence of those scientific explanations, so as to encourage critical thinking by the student. The Ideal Gas Law Copyright © McGraw-Hill Education

3. Essential Questions How does Avogadro’s principle relate the number of particles of gas to the gas’s volume? How is the amount of gas present related to its pressure, temperature, and volume by the ideal gas law? What are the properties of real gases and of ideal gases? The Ideal Gas Law Copyright © McGraw-Hill Education

4. Review mole New Avogadro’s principle molar volume standard temperature and pressure (STP) ideal gas constant (R) ideal gas law The Ideal Gas Law Copyright © McGraw-Hill Education Vocabulary

5. The Ideal Gas Law Copyright © McGraw-Hill Education Avogadro's Principle Avogadro’s principle states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles.

6. The Ideal Gas Law Copyright © McGraw-Hill Education 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. 0.00°C and 1.00 atm are called standard temperature and pressure (STP). At STP, 1 mol of gas occupies 22.4 L.

7. The Ideal Gas Law Copyright © McGraw-Hill Education MOLAR VOLUME Use with Example Problem 5. Problem The main component of natural gas used for home heating and cooking is methane (CH 4 ). Calculate the volume that 2.00 kg of methane gas will occupy at STP. Response ANALYZE THE PROBLEM The number of moles can be calculated by dividing the mass of the sample, m, by its molar mass, M. The gas is at STP (0.00°C and 1.00 atm pressure), so you can use the molar volume to convert from the number of moles to the volume. KNOWNUNKNOWN m = 2.00 kgV = ? L T = 0.00ºC P = 1.00 atm

8. The Ideal Gas Law Copyright © McGraw-Hill Education MOLAR VOLUME EVALUATE THE ANSWER The amount of methane present is much more than 1 mol, so you should expect a large volume, which is in agreement with the answer. The unit is liters, a volume unit, and there are three significant figures.

9. The Ideal Gas Law Copyright © McGraw-Hill Education 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

10. The Ideal Gas Law Copyright © McGraw-Hill Education The Ideal Gas Law The ideal gas constant is represented by R and is 0.0821 Latm/molK when pressure is in atmospheres. The ideal gas law describes the physical behavior of an ideal gas in terms of pressure, volume, temperature, and amount.

11. The Ideal Gas Law Copyright © McGraw-Hill Education The Ideal Gas Law

12. Copyright © McGraw-Hill Education THE IDEAL GAS LAW Use with Example Problem 6. Problem Calculate the number of moles of ammonia gas (NH 3 ) contained in a 3.0-L vessel at 3.00 × 10 2 K with a pressure of 1.50 atm. Response ANALYZE THE PROBLEM You are given the volume, temperature, and pressure of a gas sample. Use the ideal gas law, and select the value of R that contains the pressure units given in the problem. Because the pressure and temperature are close to STP, but the volume is much smaller than 22.4 L, it would make sense if the calculated answer were much smaller than 1 mol. KNOWNUNKNOWN V = 3.0 Ln = ? mol T = 3.00 × 10 2 K P = 1.50 atm

13. The Ideal Gas Law Copyright © McGraw-Hill Education THE IDEAL GAS LAW EVALUATE THE ANSWER The answer agrees with the prediction that the number of moles present will be significantly less than 1 mol. The unit of the answer is the mole, and there are two significant figures.

14. The Ideal Gas Law Copyright © McGraw-Hill Education The Ideal Gas Law—Molar Mass and Density Molar mass and the ideal gas law:

15. The Ideal Gas Law Copyright © McGraw-Hill Education The Ideal Gas Law—Molar Mass and Density Density and the ideal gas law:

16. Gasses Video FPO Add link to video from page 456 here. The Ideal Gas Law Copyright © McGraw-Hill Education

17. The Ideal Gas Law Copyright © McGraw-Hill Education Real Versus Ideal Gases Ideal gases follow the assumptions of the kinetic-molecular theory. Characteristics of ideal gases: 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.

18. The Ideal Gas Law Copyright © McGraw-Hill Education Real Versus Ideal Gases Real gases deviate most from ideal gases at high pressures and low temperatures. Polar molecules have larger attractive forces between particles. Polar gases do not behave as ideal gases. Large nonpolar gas particles occupy more space and deviate more from ideal gases.

19. Gasses, Pressure and Scuba Diving Video FPO Add link to video from page 458 here. The Ideal Gas Law Copyright © McGraw-Hill Education

20. The Ideal Gas Law Copyright © McGraw-Hill Education Review Essential Questions How does Avogadro’s principle relate the number of particles of gas to the gas’s volume? How is the amount of gas present related to its pressure, temperature, and volume by the ideal gas law? What are the properties of real gases and of ideal gases? Vocabulary Avogadro’s principle molar volume standard temperature and pressure (STP) ideal gas constant (R) ideal gas law