Properties-of-Gases-1.pptx the most abundant and sexiest kimi na rot ganun

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1. Unit 4. MODULE 1 Lesson 1 Properties of Gases

2. Learning Objectives: At the end of the lesson, the learners should be able to; K - identify the different properties of gases; S - demonstrate the Kinetic Molecular Theory of Gases; A – apply gas concepts to real world situations, such as air conditioning

3. FACT OR BLUFF Directions: The learners will raise the green flag if the answer is FACT and red flag if the answer is BLUFF. 1. Gases have low densities. 2. Water vapor is a mixture of gas 3. Ozone is a gas at room temperature 4. Gases expand when more pressure is applied

4. FACT OR BLUFF 5. Gases assume the volume and shape of their container. 6. Gases are the most studied and easily understood states of matter 7. The higher the temperature of a gas, the lower its particles are moving. 8. Under the normal atmosphere conditons , there are only eight that are gases.

5. FACT OR BLUFF 9. At STP, the standard temperature and pressure are 273 k and 1 atm. Respectively. 10. Gases are so compressible because they consist mostly of empty space between particles.

6. Questions: What are the main properties of gases? How do gases differ from solids and liquids? What is the relationship between gas pressure and volume?

7. Describing Gases There are threee states of matter, namely solid, liquid, and gases. All states of matter differ in their properties based on the arrangement of their particles. Solid particles are tightly packed, usually in a regular pattern, liquid particles are close together with no regular arrangement, while gas particle are well separated with no regular arrangement.

8. Characteristics of Gases Gases expand to fill any container. random motion, no attraction Gases are fluids (like liquids). no attraction Gases have very low densities. no volume = lots of empty space

9. Characteristics of Gases Gases can be compressed. no volume = lots of empty space

10. Volume Is one of the measureable properties of gas, is denoted by the symbol V. It is the amount of space occupied by as gas sample. 1 L = 1 dm³ = 1000 mL = 1000 cm³

11. Pressure Pressure is denoted by the symbol of P. Pressure of the gas is the forcd exerted by the gas per unit area. Pressure (P) = force (F) / area (A) The SI unit used for pressure is pascal (Pa). Named after Blaise Pascal 1 Pa = 1 N / m² 1atm = 760 mmHg = 760 torr = 1.01325 bar = 101. 325 kPa = 101.325 × 103 Nm³

12. Standard Temperature & Pressure 0°C 273 K 1 atm 101.325 kPa -OR- STP

13. Temperature The temperature is denoted by the letter T. The temperature of a gas depends on its kinetic energy. Gases expand when the temperature is increased. The temperature of gas is expressed in Fahrenheit (°F), Centigrade or Celsius (°C) and Kelvin (K) To convert Celsius to Kelvin, we use the equation K = °C + 273

14. Amount or number of Moles The amount of gas (or mass) is another measureable property of gas. The mass of gas is related to its number of moles and is generally expressed in kilogram (kg) or gram (g) Number of moles = mass of the gas or molar mass of the gas. In symbols, n = m/M

15. Kinetic Molecular Theory of Gases The properties of gases can be explained in terms of their molecular motion. The ideas about molecular motion were developed into the kinetic molecular theory by Rudolf Clasius , James Maxwell, and Ludwig Boltzman . The kinetic molecular theory of gases is a model that could help us understand the behavior of gases. Its postulates are the following:

16. Kinetic Molecular Theory of Gases A gas consist of very small particles. The particles are in constant , random, and straight-line following . The particles of a gas are separated by distances much larger than their size. The attractive forces between particles are negligible, and the particles act indepently of one another.

17. ACTIVITY: HOW DOES GAS BEHAVE Materials : Ordinary party balloon, empty 2 liter plastic soda bottle. Procedure : Push an ordinary party balloon into an empty 2 liter plastic soda bottle Stretch the balloon’s mouthpiece over the opening of the bottle. Blow into the balloon. Blow up an identical balloon outside the soda bottle to serve as a comparison

18. Questions: How big does the balloon in the soda bottle get? How big does the balloon outside the soda bottle get? Explain the difference?

19. 3, 2, 1 EXIT What are the 3 Properties of Gas? How do properties of gases relate to the behavior of real world systems, such as engines and refrigerators? How do properties of gases change at extreme temperature or pressure?

20. QUIZ TIME!

21. Assignment Directions: Write TRUE if the statement is accurate and FALSE If the statement is flawed. Write your answer in separate sheet of paper. KINETIC MOLECULAR THEORY

22. The particles are is contant , random, and straight-line motion. The attractive forces among the particles are negligible. The average kinetic of the gas particles is equal to the absolute temperature. The collision of the particles with each other and with the walls of the container changes the kinetic energy of the particle.

23. 5. The particle of a gas are separated by distances much larger than their size 6. The gas particle occupies a negligible volume. 7. Collisions among molecules are perfectly inelastic. 8. After each collision, the total energy of a system is the same

24. 9. The regulative forces among particles are negligible. 10. At higher temperature, the collision of the gas particle with the walls of the container becomes more often and with more force, thus producing a lesser pressure.

25. Lesson 2: Conversion of Unit

26. K - define and explain the concept of unit conversion S - identify and explain the different types of unit conversion A - convert between different units of measurement using appropriate conversion factors Learning Objectives :

27. Objectives: To guess what the other player is thinking of, without directly communicating, by questioning or identify the chosen concepts or answer ACTIVITY: TELEPATHY GAME

28. Directions: The learners will choose a partner to answer the questions Procedure: Ask questions that involve our topic and both players try to guess what the other person is thinking of simultaneously

29. 1. Give at least one properties of gases? 2. Give at least one states of matter? 3. What object mostly used as example of Gas? Questions:

30. Direction: The learners will arrange the jumbled letters to get its correct word Materials: Marker and Paper Procedure: The teacher will assign the learners to create five groups to play a game. ACTIVITY: ARRANGE ME

31. 1. What is the different between volume, pressure, and temperature? 2. SI unit for volume, pressure, and temperature? Questions:

32. The process of changing a measurement from one unit to another, typically by multiplying or dividing by a conversion factor Conversion of Unit

33. Commonly used units and their equivalents for volume, pressure, and temperature

34. Variable SI Unit Metric Unit English Unit Units and their equivalents Volume Cubic meter (m3) Cubic decimeter (dm3) Centimeter (cm3) Liter (L) Milliliter (mL) Quart (qt) Gallon (gal) 1mL = 1cm3 1 L = 1dm3 1cm3 = 1000 L Pressure Pascal (Pa) Atmosphere (atm) millimeters of mercury (mmHg) Centimeters of mercury (cm Hg) Torr 1b/in2 (psi) 1 ATM= 760 mm Hg = 76 cm Hg= 760 torr = 101,325 Pa = 14, 6956 psi Temperature Kelvin (K) Celcius (C) Fahrenheit (F) 0 C = 273.15 K 0 C = 32 F

35. QUIZ TIME!

36. Directions: Choose the letter of the correct answer and write it on the separate sheet of paper. Multiple Choice

37. 1. What are the different types of unit conversion? A. Volume, pressure, and temperature B. Volume and pressure C. Temperature and pressure D. None of the above

38. 2. The SI unit of volume is. A. Cubic meter, decimeter, and centimeter B. Liter, and milliliter C. Torr D. Quart

39. 3. It is expressed in fahrenheit,centigrade or Celsius, and Kelvin. A. Volume B. Temperature C. Pressure D. All of the above

40. 4. The metric unit of pressure. A. Atmosphere B. Celsius C. Meter D. Centimeter

41. 5. The SI unit used for pressure is Pascal (P), named after? A. Robert Boyle B. Blaise Pascal C. Jacques Charles D. Joseph Louis Gay Lussac

42. Directions: Answer the following problem. Write your answer on a separate sheet of paper. Assignment

43. 1. The inflated balloon that slipped from the hand of Renn has a volume of 0.50 L at sea level (1.0 atm) and it reached a heightof approximately 8 km where the atmospheric pressure is approximately 0.33 atm. Assuming the temperature is constant, compute for the final volume of the balloon.

44. Lesson 3: Boyle's Law

45. Learning Objectives: K – state Boyle’s law S – solve problems involving changes in the condition of the gas using the equations for Boyle’s law A – cite an application of Boyle’s law in daily occurences

46. Volume and Pressure A clear inverse relationship between pressure and volume is observed, meaning as pressure increases, volume decreases, and vice versa, which is best visualized by a curved line on a graph where pressure is plotted againts volume, demonstrating a hyperbolic curve.

47. Robert Boyle He was analyzed the relationship between the volume of a gas and it pressure. He found that the volume of the gas decreases as the pressure exerted on it increases. This phenomenon is known as Boyle’s Law.

48. Boyle’s Conclusion The molecules of a gas exert pressure on the walls of its container. When pressure is applied on the gas the molecules move closer to one another which result in the decrease in the volume. This increases the chances of collisions among the molecules and the walls of the container; thus pressure is increased.

49. Boyle’s Law Equation P1V1=P2V2 Where: P1 = initial pressure P2 = final pressure V1 = initial volume V2 = final volume

50. Sample Problem 1: Two hundred cubic centimeter of gas (200 cm³) is contained in a vessel under a pressure of 850 mmHg. What would be the new volume of the gas if the pressure is changed to 1000 mmHg? Assume that the constant temperature remains constant .

51. Given: P1 = 850 mmHg V1 = 200 cm³ P2 = 1000 mmHg Find: V2? Formula: P1V1 = P2V2 Solution: V2 = 850 mmHg × 200 cm³ 1000 mmHg V2 = 170 cm³

52. Sample Problem 2: A 200 ml sample of hydrogen gas is collected when the pressure is 800 mmHg. What volume will the gas occupy at 760 mmHg?

53. Given: P1 = 800 mmHg V1 = 200 ml P2 = 760 mmHg Find: V2? Formula: P1V1=P2V2 Solution: V2 = 800 mmHg × 200 ml 760 mmHg V2 = 210.53 ml

54. GROUP ACTIVITY: SOLVE ME

55. GROUP 1 A gas has an initial pressure of 5.85 atm and an initial volume of 3.65 L. What is the new volume of the gas if the pressure drops to 3.00 atm. Assume temperature and the number of moles are kept constant.

56. GROUP 2 A scuba tank has a pressure of 200 atm and a volume of 10 L, the pressure is decreased in 150, what is the new volume?

57. GROUP 3 A sample nitrogen gas (N²) has volume of 12.0 L, and a pressure of 760.0 mmHg. When the gas is released, it gives 32.0 L of nitrogen. If the temperature is the same, what is the new pressure of nitrogen?

58. QUIZ TIME!

59. Multiple Choice : Directions : Choose the letter of the correct answer and write it on the separate sheet of paper.

60. 1. He was analyzed the relationship between the volume of a gas and it pressure. A. Robert Boyle B. Robert Boles C. Robert Blaise D. Robert Boisle

61. 2. What is the formula for Boyle’s Law? A. P1V1=P2V2 B. P2V2=P1V1 C. T1V1= T2V2 D. All of the above

62. 3. A balloon has a pressure of 1.5 atm and a volume of 20 L. If the pressure is increased to 2.5 atm , what is the new volume? A. 11 L B. 12 L C. 13 L D. 14 L

63. 4. A diver descends to a depth where the pressure is 4 atm. If the diver’s air tank has a volume of 15 L, at the surface 1 atm , what is the volume of the tank depth? A. 3.76 L B. 3.75 L C. 3.74 L D. 3.77 L

64. 5. What happens to pressure of a gas when its volume is decreased, according to Boyle’s law? A. Pressure increases B. Pressure decreases C. Pressure remains the same D. Pressure becomes zero

65. Assignment Directions: Analyze and solve the following problem on your separate sheet of paper.

66. 1. A cylinder with a movable piston contains 250 cm³ air at 10°C, if the pressure is kept constant, at what temperature would you expect the volume to be 150 cm³? Take note that the temperature must be Kelvin.

67. Lesson 4: Charles Law

68. Learning Objectives: K – state Charles’ Law S – solve problems involving changes in the condition of the gas using the equations for Charles’ Law A – cite an application of Charles’ Law in daily occurences .

69. ACTIVITY HOT AND COLD BALLOON

70. Directions: The learners will demonstrates how air expands when heated and contracts when cooled, causing a balloon to inflate when placed over a bottle of hot water and deflate when moved to cold water. Materials: Balloon, empty plastic bottle, bowl of hot and cold water.

71. Procedure: 1.Stretch the balloon over the opening of the bottle. 2. Place the bottle in the bowl of hot water. 3. Observe the balloon inflate as the air inside the bottle heats up. 4. Transfer the bottle to the bowl of cold water. 5. Watch the balloon deflate as the air cools down.

72. Question 1. What happen to balloon when it place to hot water? 2. What happen to balloon when move to cold water? 3. What is the difference?

73. Jacques Charles He studied the relationship between the volume and temperature of a gas using a balloon. He concluded that when the pressure of a gas is kept constant, its volume is directly proportional to its temperature. This means that the volume of a gas increases as the temperature rises and the volume decreases as the temperature drops.

74. Charles’ Law Equation Charles’ law can be expressed mathematically as; V a T at constant pressure To remove the proportionality sign, we introduce the constant K V = k T

75. Charles’ Law Equation If the same gas is brought to two different temperatures, it will give two different volumes. The equation will become V1T1=V2T2 Where: T1 = initial temperature of the gas V1 = initial volume of the gas T2 = final temperature of the gas V2 = final volume of the gas

76. Charles’ Law He states that the volume of a gas is directly proportional to its absolute temperature ( in Kelvin ) when pressure is held constant, meaning as temperature increases.

77. Sample Problem 1: A cylinder with a movable piston contains 250 cm³ air at 10°C. If the pressure is kept constant, at what temperature would you expect the volume to be 150 cm³? Take note that the temperature must be in Kelvin.

78. Given: T1 = 10°C V1 = 250 cm³ V2 = 150 cm³ Find: T2? Formula: V1T1=V2T2 Solution: (T1) K = 10°C + 273 = 283 K T2 = (150 cm³)(283 K) 250cm³ T2 = 169.8 K or 170 K

79. Sample Problem 2: A balloon has a volume of 2.5 L at a temperature of 20°C. What is the volume of the balloon when the temperature is increased to 80°C?

80. Given: V1 = 2.5 L T1 = 20°C + 273 = 293 K T2 = 80°C + 273 = 353 K Find: V2? Formula: V1T1 = V2T2 Solution: V2 = (2.5 L) (353 K) 293 K V2 = 3.01 L

81. GROUP ACTIVITY: PICK ME UP: SLAWGAN

82. Concepts of Charles’ Law 1. Heat it up, watch it expand. 2. Temperature rising, volume soaring. 3. Hot air balloons take flight. 4. Cool it down, shrink it up. 5. Gases on the move.

83. CRITERIA Excellent (5) Very Good (4) Good (3) Needs improvement (2) SCORE Creativity and Originality All the visuals used on the slogan reflect an exceptional degree of student in creativity in their output. Most of the visuals used on the poster slogan reflect student creativity in their output The visuals were made by the student but copied from design of others The visuals were not made by the students Accuracy and Relevance of the content All visuals in the slogan are accurate and related to the topic Most of the visuals in the poster slogan are accurate and related to the topic Some of the visuals are accurate and related to the topic The graphics in the visuals are not accurate nor related Presentation The slogan clearly communicates the main idea and strongly promotes awareness The slogan communicates some of the important ideas and slightly promotes awareness The slogan indirectly communicates the idea and hardy promotes awareness The slogan does not sufficiently communicate any idea that can promote awareness

84. Question: 1. What is the significance of Charles’ law in real life applications? 2. How does Charles’ law apply to the operation of a hot air balloon? 3. What is the main reasons why balloons expand when they are heated?

85. QUIZ TIME!

86. Multiple Choice: Directions: Choose the letter of the correct answer and write it on separate sheet of paper.

87. 1. Which of the following statements is a correct expression of Charles’ Law? A. P1V1=P2V2 B. V1T1=V2T2 C. P1T1=P2T2 D. V1P1=V2P2

88. 2. What happens to the volume of a gas when its temperature is doubled, according to Charles’ law? A. The volume is halved B. The volume remains the same C. The volume is doubled D. The volume is quarupled

89. 3. Which of the following is a consequence of Charles’ Law? A. Increasing the pressure of a gas increases its volume. B. Increasing the temperature of a gas increases its volume C. Decreasing the temperature of a gas increases its volume D. Decreasing the pressure of a gas decreases its temperature

90. 4. According to Charles’ law, what is the effect of decreasing the temperature of a gas on its volume? A. The volume increases B. The volume remains the same C. The volume decreases D. The volume becomes zero

91. 5. A balloon has a volume of 2.5 L at a temperature of 20°C. If the temperature is increased to 40°C, what is the new volume of the balloon? A. 2.1 L B. 2.5 L C. 2.9 L D. 3.3 L

92. Assignment Directions: Read the following questions below and answer it briefly.

93. 1. Explain Charles’ Law and its significance in understanding the behavior of gases. Provide examples of how Charles’ Law in real-life.

94. 2. Describe the relationship between temperature and volume of a gas, as described by Charles’ Law. How does this relationship affect the behavior of gases in different temperature conditions? Provide examples to illustrate your answer.

95. THANK YOUUUU AND GOD BLESSED^^