Quarter: 4 Week: 1 MELC(s): Investigate the relationship between volume and pressure at constant temperature of a gas and explain these relationships using the kinetic molecular theory. ($10MT-IVa-b-21) > Title of Textbook/LM to Study: Science 10 Learner's Manual Chapter: _4 _Pages: 362-371 Topic: Boyle's Law > Objectives: 1. Describe the relationship between volume and pressure at constant temperature of a gas using kinetic molecular theory. 2. Solve problems involving volume and pressure at constant temperature of gas. 3. Apply concept of Boyle's Law in real life scenario. Let Us Discover This learning activity sheet offers interesting discussion about gases, its behaviour and properties. Like solids and liquids, gases are governed by laws of nature. One of the fundamental laws that governs gas is the Boyle's Law. This law is explained by the kinetic molecular theory, in which the pressure of a gas depends on the number of times per second that the molecules strike the surface of the container or collide with each other, as the volume of gas decreases, the pressure increases forcing the gas particles to move closer to one another. Boyle's law states that the relationship between the volume and pressure of gases at constant temperature is inversely proportional, meaning when one value decreases, the other value increases. This was first stated by Robert Boyle during the 16th century while he performed an experiment wherein he trapped a fixed amount of air in the J-tube, he changed the pressure and controlled the temperature and then, he observed its effect to the volume of the air inside the J-tube. He found out that as the pressure is increased, the volume decreases. He finally concluded that the volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature. Gas particles have a very weak intermolecular force of attraction, hence they move as far as possible from each other. They have the tendency to occupy all the spaces they are contained in. If the pressure is increased, the volume will be decreased. This phenomenon can be expressed in the Boyle's Law equation: V at constant T and n P GSC-CID-LRMS-ESSLM, v.r. 02.00, Effective April 21, 2021Where: V = volume, p = pressure, T = temperature and n = amount of :5 , Let us apply the equation you learned about Boyle's Law. Since volume ' of the gas can be varied, let P1 and V1 be the initial pressure and volume respe l and V2 be the final preSSure and volume respectively. According to Boyle's Law, PV=K therefore: , . V1P1=K i V2P2=K Then: V1P1=V2P2 / M Let Us Try Since you are now equipped with the fundamental knowledge about Boyle's Law, W to answer these questions by examining the picture below. 'yle's Law illustration as the set of weights is added on top of it? tringe when the set of weights is added? and pressure of gases at constant temperature? Let Us Do To further investigate the relationship between the pressure and volume of gas at constant temperature, try to solve these problems in a separate sheet of paper using this Boyle's Law formula: VIP 1 = V 2P 2 Sample Problem: 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 height of approximately 8 km where the atmospheric pressure is approximately 0.33 atm. Assuming that the temperature is constant, compute for the final volume of the balloon. Initial Conditions Final Conditions V = 0.50 L V = ? P = 1.0 atm P = 0.33 atm VIP 1 = V 2P 2 P 2 = V1 P 1 /V 2 = (0.50 L)(1.0 atm) / ( 0.33L) = 1.5 L Problems: 1. Oxygen gas inside a 1.5 L gas tank has a pressure of 0.95 atm. Provided that the temperature remains constant, how much pressure is needed to reduce its volume by 1/2? 2. A scuba diver needs a diving tank in order to provide breathing gas while he is underwater. How much pressure is needed for 6.00 liters of gas at1.01 atmospheric pressure to be compressed in a 3.00 liter cylinder? Let Us Apply Now you already have the concepts about Boyle's law, let's apply these concepts in a real life situation. Scenario: One sunny afternoon, you decided to buy a can of soda from the convenient store nearby, right after buying a can of soda, you hurriedly ran to your home. Upon reaching home, you excitedly opened the can of Figure 2: Liquid fizz soda and surprisingly, liquid fizz right up out of the bottle, creating a right up out of the huge mess. What do you think is the reason why liquids fizz out from the can of soda? bottle 3 GSC-CID-LRMS-ESSLM, v.r. 02.00, Effective April 21, 2021Answer: Rubrics 5 3 2 All concepts are Most concepts Some of the Few of the Little to none of complete, are complete concepts are concepts are the concepts are clearly stated and clearly present discussed discussed with sufficient stated understanding of the topic: Boyle's law References Acosta, H. D., Alvarez, L. A., Angeles, D. G., Arre, R. D., Carmona, M. P., Garcia, A. S., ... Salazar, N. G. (2013). Grade 10 Learner's Manual. Pasig City: REX Book Store Inc. Page 362- 371 Acosta, H. D., Alvarez, L. A., Angeles, D. G., Arre, R. D., Carmona, M. P., Garcia, A. S.,... Salazar, N. G. (2013). Grade 10 Teacher's Manual. Pasig City: REX Book Store Inc. Page 265-267 SSLM Development Team Writer: Ely Bobbylord C. Alamin Evaluator: Rosalie P. Gillesania