Chapter 13

Chapter Menu Gases Section 13.1 The Gas Laws Section 13.2 The Ideal Gas Law Section 13.3 Gas Stoichiometry Exit Click a hyperlink or folder tab to view the corresponding slides.

Section 13-1 Section 13.1 The Gas Laws ,[object Object],scientific law: describes a relationship in nature that is supported by many experiments ,[object Object]

Section 13-1 Section 13.1 The Gas Laws (cont.) 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 Boyle's Law ,[object Object],P 1 V 1 = P 2 V 2 where P = pressure and V = volume

Section 13-1 Charles's Law ,[object Object],[object Object]

Section 13-1 Charles's Law (cont.)

Section 13-1 Charles's Law (cont.) ,[object Object],[object Object]

Section 13-1 Gay-Lussac's Law ,[object Object]

Section 13-1 Gay-Lussac's Law (cont.)

Section 13-1 The Combined Gas Law ,[object Object]

Section 13-1 The Combined Gas Law (cont.)

[object Object],[object Object],[object Object],[object Object],Section 13-1 Section 13.1 Assessment 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

[object Object],[object Object],[object Object],[object Object],Section 13-1 Section 13.1 Assessment Atoms are in their lowest energy state at what temperature? A. 0° Celsius B. 0° Fahrenheit C. –100° Celsius D. 0 kelvin

Section 13-2 Section 13.2 The Ideal Gas Law ,[object Object],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 ,[object Object],[object Object]

Section 13-2 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.

Section 13-2 Avogadro's Principle ,[object Object]

Section 13-2 Avogadro's Principle (cont.) ,[object Object],[object Object],[object Object]

Section 13-2 The Ideal Gas Law ,[object Object],[object Object]

Section 13-2 The Ideal Gas Law (cont.) ,[object Object],[object Object]

Section 13-2 The Ideal Gas Law (cont.)

Section 13-2 The Ideal Gas Law—Molar Mass and Density ,[object Object]

Section 13-2 The Ideal Gas Law—Molar Mass and Density (cont.) ,[object Object]

Section 13-2 Real Versus Ideal Gases ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

Section 13-2 Real Versus Ideal Gases (cont.) ,[object Object],[object Object],[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Section 13-2 Section 13.2 Assessment 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

[object Object],[object Object],[object Object],[object Object],Section 13-2 Section 13.2 Assessment 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 13-3 Section 13.3 Gas Stoichiometry ,[object Object],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 ,[object Object],When gases react, the coefficients in the balanced chemical equation represent both molar amounts and relative volumes.

Section 13-3 Stoichiometry of Reactions Involving Gases ,[object Object],[object Object],[object Object]

Section 13-3 Stoichiometry and Volume-Volume Problems ,[object Object]

Section 13-3 Stoichiometry and Volume-Mass Problems ,[object Object],[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Section 13-3 Section 13.3 Assessment 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

[object Object],[object Object],[object Object],[object Object],Section 13-3 Section 13.3 Assessment 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

Resources Menu Chemistry Online Study Guide Chapter Assessment Standardized Test Practice Image Bank Concepts in Motion

Study Guide 1 Section 13.1 The Gas Laws Key Concepts ,[object Object],[object Object],[object Object]

Study Guide 1 Section 13.1 The Gas Laws (cont.) Key Concepts ,[object Object],[object Object]

Study Guide 2 Section 13.2 The Ideal Gas Law Key Concepts ,[object Object],[object Object]

Study Guide 2 Section 13.2 The Ideal Gas Law (cont.) Key Concepts ,[object Object],[object Object]

Study Guide 3 Section 13.3 Gas Stoichiometry Key Concepts ,[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 1 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

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 2 According to Charles’s law, if pressure and amount of a gas are fixed, what will happen as volume is increased? A. Temperature will decrease. B. Temperature will increase. C. Mass will increase. D. Mass will decrease.

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 3 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

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 4 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

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 5 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

[object Object],[object Object],[object Object],[object Object],STP 1 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

[object Object],[object Object],[object Object],[object Object],STP 2 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

[object Object],[object Object],[object Object],[object Object],STP 3 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

[object Object],[object Object],[object Object],[object Object],STP 4 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

[object Object],[object Object],[object Object],[object Object],STP 5 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

IB Menu Click on an image to enlarge.

CIM Figure 13.3 The Gas Laws Table 13.1 The Gas Laws

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Chapter 13

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Chapter 13