FINAL DEMO BOYLE'S LAW in education.pptx

boyles law demo teaching

1. THE GAS LAW Subtopic: BOYLE’S LAW Rachel Ann C. Ramilo Teacher

2. REVIEW GAME!

3. GUESS THE WORD

4. USE THE PICTURES TO GUESS THE WORD. READY ?

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9. For Playing Thank You

10. MARSHMALLOW AND SYRINGE

11. Procedure 1. Remove the needle of the syringe if there is any. Put a marshmallow inside the syringe. 2. Place your thumb over the end of the syringe where the needle is usually located. Holding your thumb in place, push in the plunger. Observe what happens to the marshmallow as you do so. 3. With your thumb still in place, pull the plunger out and observe what happens.

12. What happen to the marshmallows when you push plunger of the syringe?

13. What happened when the plunger was pulled out?

14. BOYLE’S LAW VOLUME-PRESSURE RELATIONSHIP

15. FOUR MAIN GAS LAWS Boyle’s Law Charles’ Law Gay-Lussacs Law Avogadro’s Law

16. Who do you think is the proponent of Boyle’s law? Question

17. Robert Boyle Boyle’s Law was named after chemist and physicist Robert Boyle , who published the original law in 1662.

18. Boyle’s law states that the volume of a gas is inversely proportional to its pressure (P) at constant temperature (T). In symbol; P∞ 1/V

19. Volume (V) Pressure (P) VxP 2.0 10.00 4.0 5.00 8.0 2.50 16.0 1.25 The table below shows volume and pressure data for a set amount of gas at the constant temperature.

20. Volume (V) Pressure (P) VxP 2.0 10.00 4.0 5.00 8.0 2.50 16.0 1.25 The table below shows volume and pressure data for a set amount of gas at the constant temperature. 20 20 20 20

21. Boyle’s Law PV=k Therefore: P1V1= k P2V2= k then , P1V1=P2V2

22. Based on the relationship of pressure and volume, what do you think will happen to the volume if pressure of a gas doubles? Based also on the relationship of pressure and volume, in what particular situation where you can relate the concept of pressure volume relationship?

23. A sample of nitrogen gas (N2) has a volume of 12L and pressure of 760mmHg. When the gas is released, it gives 32L of nitrogen. If the temperature is the same, what is the new pressure of hydrogen? sample problem 1

24. Solution; GIVEN: P1= 760mmHg V1= 12L V2 = 32L P2 = ? Derived the equation for P2 using Boyle’s Law: P1V1=P2V2 FORMULA: P2= P1V1 V2 SOLUTION: P2= 760mmHg(12 L ) 32 L P2 = 1 9,120 mmHg 32 P2 = 285 mmHg The final pressure is 285 mmHgt

25. A gas tank holds 20L of oxygen (O2) at a pressure of 15atm. How many liters will the gas occupy if the pressure is changed to 0.800atm at constant temperature? sample problem 2

26. Solution; GIVEN: Given P1= 15atm V1= 20.0L P2 = 0.800atm V2 = ? Derived the equation for V2 using Boyle’s Law: P1V1=P2V2 FORMULA: V2= P1V1 P2 SOLUTION: The final volume is 375L V2= 15 atm (20L ) 0.800 atm V2 = 300L 0.800 V2 = 375L

27. CHECK FOR UNDERSTANDING

28. 1. A 4.2L balloon holds air at 580torr. If the balloon expands to 5.6L, what will the pressure of the air inside become? 2. The volume of air in the marshmallows blaster is 450ml. The pressure is 1.00 atm. If I decrease the volume to 50ml, what will the new pressure be? ANSWER THESE PROBLEM

29. 3. A tank of nitrogen has a volume of 14.0 L and a pressure of 760.0 mm Hg. Find the volume of the nitrogen when its pressure is changed to 400.0 mm Hg while the temperature is held constant. 4. A gas has a volume of 100 ml, when the pressure is 735 mmHg. How many milliliters will the gas occupy at 700 mm Hg?

30. 1. A 4.2L balloon holds air at 580torr. If the balloon expands to 5.6L, what will the pressure of the air inside become? Given P1= 580 torr V1= 4.2L P2= ? V2=5.6L Solution: P2= 580torr (4.2 L) 5.6L P2= 2,436torr 5.6 P2= 435 torr Formula: P1V1=P2V2 P2= P1V1 V2 The final pressure is 435 torr.

31. 2. The volume of air in the marshmallows blaster is 450ml. The pressure is 1.00 atm. If I decrease the volume to 50ml, what will the new pressure be? Given P1= 1.00atm V1= 450ml V2=50ml P2= ? Formula: P1V1=P2V2 P2= P1V1 P2 Solution: P2= 1.00atm (450ml) 50ml P2= 450 50 P2= 9.00 atm The final pressure is 9.00atm

32. 3. A tank of nitrogen has a volume of 14.0 L and a pressure of 760.0 mm Hg. Find the volume of the nitrogen when its pressure is changed to 400.0 mm Hg while the temperature is held constant. Given; P1=760.0 mmHg V1= 14.0 L. P2= 400.0 mmHg V2=? Formula: P1V1=P2V2 V2= P1V1 P2 solution: V2= 760.0 mmHg (14.0 L.) 400.0 mmHg V2= 10640 L. 400.0 V2= 26.6 L. The final volume is 26.6 L.

33. 4. A gas has a volume of 100 ml, when the pressure is 735 mmHg. How many milliliters will the gas occupy at 700 mm Hg? Given; P1=735 mmHg V1= 100 ml P2= 700 mmHg V2=? Formula: P1V1=P2V2 V2= P1V1 P2 Solution: V2= 735 mmHg (100ml) 700mmHg V2= 73500 ml. 700 V2= 105 ml. The final volume is 105 ml.

34. Question What does Boyle’s Law states? What will happen if the pressure increases? What about if the volume increases?

35. - If the pressure increases the volume decreases. - If the volume increases, the pressure decreases. - Boyle’s law states that the volume of a gas is inversely proportional to its pressure (P) at constant temperature (T).

36. Cite a real life situation wherein the concept of Boyles is being applied.

37. You can observe a real-life application of Boyle's Law when you fill your bike tires with air. When you pump air into a tire, the gas molecules inside the tire get compressed and packed closer together. This increases the pressure of the gas, and it starts to push against the walls of the tire.

38. ANY QUESTIONS?

39. A. Multiple Choice: Choose the letter of the correct answer. ___1. What law describes the relationship of the volume of the gas to its pressure when mass and temperature are held constant? a. Boil’s Law c. Boyle’s Law b. Boles’ Law d. Broil’s Law ___2. Who conceptualized the relationship between the volume and pressure of the gas that varies inversely proportional to each other at constant temperature and mass? a. Robby Boyle c. Rob Boyle b. Robert Boil d. Robert Boyle

40. ___3. In Boyle’s Law when the mass and temperature are held constant, what happens to the volume if the pressure increases? a. Increase c. Decrease b. Unchanged d. Became zero ___4. In contrast to no. 3 what happens to the volume if the pressure decreases? a. Increase c. Decrease b. Unchanged d. Became zero ______5. Which of the following best describe the concept of Boyle’s Law? a. Hot air balloon c. Pressure Cooker b. Syringes d. all of the above

41. B. Direction: Solve the following. (Show your solution) 1. A gas occupies 25.3 mL at a pressure of 790.5 mm Hg. Determine the volume if the pressure is reduced to 0.804 atm. 2. Convert 77.0 L at 18.0 mm of Hg to its new volume at standard pressure. 3. 500.0 mL of a gas is collected at 745.0 mm Hg. What will the volume be at standard pressure?

42. A. Give two (2) good and bad effects of using Boyle’s Law in our daily living. B. Answer the following question; 1. What is Charles law? 2. What are the variables involve in Charles law?