1. Chapter 13: Gases CHEMISTRY Matter and Change

2. Section 13.1The Gas LawsThe Gas Laws Section 13.2 The Ideal Gas LawThe Ideal Gas Law Section 13.3Gas StoichiometryGas Stoichiometry Exit CHAPTER 13 Table Of Contents Click a hyperlink to view the corresponding slides.

3. State the relationships among pressure, temperature, and volume of a constant amount of gas. scientific law: describes a relationship in nature that is supported by many experiments Apply the gas laws to problems involving the pressure, temperature, and volume of a constant amount of gas. SECTION 13.1 The Gas Laws

4. Boyle’s law absolute zero Charles’s law Gay-Lussac’s law combined gas law For a fixed amount of gas, a change in one variable—pressure, temperature, or volume—affects the other two. SECTION 13.1 The Gas Laws

5. Boyle's Law Boyle’s law states that the volume of a fixed amount of gas held at a constant temperature varies inversely with the pressure. P 1 V 1 = P 2 V 2 where P = pressure and V = volume SECTION 13.1 The Gas Laws

6. Charles's Law As temperature increases, so does the volume of gas when the amount of gas and pressure do not change. Kinetic-molecular theory explains this property. SECTION 13.1 The Gas Laws

7. Charles's Law (cont.) SECTION 13.1 The Gas Laws

8. Absolute zero is zero on the Kelvin scale. Charles’s law states that the volume of a given amount of gas is directly proportional to its kelvin temperature at constant pressure. SECTION 13.1 The Gas Laws Charles's Law (cont.)

9. Gay-Lussac's Law Gay-Lussac’s law states that the pressure of a fixed amount of gas varies directly with the kelvin temperature when the volume remains constant. SECTION 13.1 The Gas Laws

10. Gay-Lussac's Law (cont.) SECTION 13.1 The Gas Laws

11. The Combined Gas Law The combined gas law states the relationship among pressure, temperature, and volume of a fixed amount of gas. SECTION 13.1 The Gas Laws

12. The Combined Gas Law (cont.) SECTION 13.1 The Gas Laws

13. Boyle’s Law explains which relationship of properties in gases? A.pressure and volume B.amount and pressure C.temperature and volume D.volume and temperature SECTION 13.1 Section Check

14. Atoms are in their lowest energy state at what temperature? A.0° Celsius B.0° Fahrenheit C.–100° Celsius D.0 kelvin SECTION 13.1 Section Check

16. 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 × 10 23 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. SECTION 13.2 The Ideal Gas Law

17. 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. SECTION 13.2 The Ideal Gas Law

18. Avogadro's Principle Avogadro’s principle states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles. SECTION 13.2 The Ideal Gas Law

19. Avogadro's Principle (cont.) 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. SECTION 13.2 The Ideal Gas Law

20. 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 SECTION 13.2 The Ideal Gas Law

21. The Ideal Gas Law (cont.) 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. SECTION 13.2 The Ideal Gas Law

22. The Ideal Gas Law (cont.) SECTION 13.2 The Ideal Gas Law

23. The Ideal Gas Law—Molar Mass and Density Molar mass and the ideal gas law SECTION 13.2 The Ideal Gas Law

24. The Ideal Gas Law—Molar Mass and Density (cont.) Density and the ideal gas law SECTION 13.2 The Ideal Gas Law

25. 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. SECTION 13.2 The Ideal Gas Law

26. Real Versus Ideal Gases (cont.) 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. SECTION 13.2 The Ideal Gas Law

27. Which of the following is NOT one of the related physical properties described in the ideal gas law? A.pressure B.volume C.density D.temperature SECTION 13.2 Section Check

28. 3.00 mol of O 2 at STP occupies how much volume? A.30.0 L B.22.4 L C.25.4 L D.67.2 L SECTION 13.2 Section Check

30. Determine volume ratios for gaseous reactants and products by using coefficients from chemical equations. coefficient: the number written in front of a reactant or product in a chemical equation, which tells the smallest number of particles of the substance involved in the reaction Apply gas laws to calculate amounts of gaseous reactants and products in a chemical reaction. When gases react, the coefficients in the balanced chemical equation represent both molar amounts and relative volumes. SECTION 13.3 Gas Stoichiometry

31. Stoichiometry of Reactions Involving Gases The gas laws can be applied to calculate the stoichiometry of reactions in which gases are reactants or products. 2H 2 (g) + O 2 (g) → 2H 2 O(g) 2 mol H 2 reacts with 1 mol O 2 to produce 2 mol water vapor. SECTION 13.3 Gas Stoichiometry

32. Stoichiometry and Volume-Volume Problems Coefficients in a balanced equation represent volume ratios for gases. SECTION 13.3 Gas Stoichiometry

33. Stoichiometry and Volume-Mass Problems A balanced chemical equation allows you to find ratios for only moles and gas volumes, not for masses. All masses given must be converted to moles or volumes before being used as part of a ratio. SECTION 13.3 Gas Stoichiometry

34. How many mol of hydrogen gas are required to react with 1.50 mol oxygen gas in the following reaction? 2H 2 (g) + O 2 (g) → 2H 2 O(g) A.1.00 B.2.00 C.3.00 D.4.00 SECTION 13.3 Section Check

35. How many liters of hydrogen gas are required to react with 3.25 liters of oxygen gas in the following reaction? 2H 2 (g) + O 2 (g) → 2H 2 O(g) A.2.00 B.3.25 C.4.00 D.6.50 SECTION 13.3 Section Check

37. Chemistry Online Study Guide Chapter Assessment Standardized Test Practice Gases Resources CHAPTER 13

38. Key Concepts Boyle’s law states that the volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature. P 1 V 1 = P 2 V 2 Charles’s law states that the volume of a fixed amount of gas is directly proportional to its kelvin temperature at constant pressure. SECTION 13.1 The Gas Laws Study Guide

39. Key Concepts Gay-Lussac’s law states that the pressure of a fixed amount of gas is directly proportional to its kelvin temperature at constant volume. The combined gas law relates pressure, temperature, and volume in a single statement. SECTION 13.1 The Gas Laws Study Guide

40. Key Concepts Avogadro’s principle states that equal volumes of gases at the same pressure and temperature contain equal numbers of particles. The ideal gas law relates the amount of a gas present to its pressure, temperature, and volume. PV = nRT SECTION 13.2 The Ideal Gas Law Study Guide

41. Key Concepts The ideal gas law can be used to find molar mass if the mass of the gas is known, or the density of the gas if its molar mass is known. At very high pressures and very low temperatures, real gases behave differently than ideal gases. SECTION 13.2 The Ideal Gas Law Study Guide

42. Key Concepts The coefficients in a balanced chemical equation specify volume ratios for gaseous reactants and products. The gas laws can be used along with balanced chemical equations to calculate the amount of a gaseous reactant or product in a reaction. SECTION 13.3 Gas Stoichiometry Study Guide

43. What does the combined gas law relate? A.pressure and temperature B.volume and pressure C.pressure, temperature, and volume D.pressure, temperature, volume, and amount CHAPTER 13 Gases Chapter Assessment

44. According to Charles’s law, if pressure and amount of a gas are fixed, what will happen as temperature is increased? A.Volume will decrease. B.Volume will increase. C.Mass will increase. D.Mass will decrease. CHAPTER 13 Gases Chapter Assessment

45. Equal volumes of gases at the same temperature and pressure contain equal numbers of particles is stated by: A.Law of conservation of mass B.Boyle’s law C.Avogadro’s principle D.Ideal gas law CHAPTER 13 Gases Chapter Assessment

46. What is the volume of 1.00 mol of chlorine gas at standard temperature and pressure? A.1.00 L B.18.0 L C.22.4 L D.44.8 L CHAPTER 13 Gases Chapter Assessment

47. When do real gases behave differently than ideal gases? A.high temperature or low pressure B.high temperature or high pressure C.low temperature or low pressure D.low temperature or high pressure CHAPTER 13 Gases Chapter Assessment

48. If two variables are directly proportional, what happens to the value of one as the other decreases? A.increases B.decreases C.remains constant D.none of the above CHAPTER 13 Gases Standardized Test Practice

49. What conditions represent standard temperature and pressure? A.0.00°C and 0.00atm B.1.00°C and 1.00atm C.0.00°F and 1.00atm D.0.00°C and 1.00atm CHAPTER 13 Gases Standardized Test Practice

50. One mole of gas occupies how much volume at STP? A.1.00 L B.2.20 L C.22.4 L D.33.7 L CHAPTER 13 Gases Standardized Test Practice

51. Which of the following would deviate the most from an ideal gas? A.gas in a hot-air balloon B.water vapor from the reaction of gaseous hydrogen and oxygen C.upper atmospheric gases D.gases near absolute zero CHAPTER 13 Gases Standardized Test Practice

52. What volume will 3.50 mol of Xe gas occupy at STP? A.78.4 L B.22.4 L C.25.9 L D.54.4 L CHAPTER 13 Gases Standardized Test Practice

53. End of Custom Shows This slide is intentionally blank.