1. Warm-up R=0.08206 L atm/mol k  If a gas is compressed…  What happens to the volume?  What happens to the pressure?  What happens to Temperature?  Kinetic-Molecular Theory applies to what type of particles?  According to the kinetic-molecular theory, what is the cause of pressure?  Pressure is the measure of force per unit of?

2. Objective SWBAT calculate and articulate relationships between the components of ideal gases in a Whiteboard practice activity.

3. HW Review

4. Whiteboard Practice

5. Practice Convert 350.0 mL at 740.0 mm of Hg to its new volume at standard pressure.

6. Practice 600.0 mL of a gas is at a pressure of 8.00 atm. What is the volume of the gas at 2.00 atm?

7. Practice At 27.00 °C a gas has a volume of 6.00 L. What will the volume be at 327.0 °C?

8. Practice When the temperature of a gas decreases, does the volume increase or decrease?

9. Practice If the Kelvin temperature of a gas is doubled, the volume of the gas will increase by ____.

10. Practice If a gas is cooled from 300.0 K to 150.00 K and the volume is kept constant what final pressure would result if the original pressure was 800.0 mmHg?

11. Practice A container holds three gases: oxygen, carbon dioxide, and helium. The partial pressures of the three gases are 3.20 atm, 3.00 atm, and 1.00 atm, respectively. What is the total pressure inside the container?

12. Practice What is the volume of gas at 2.00 atm and 200.0 K if its original volume was 300.0 L at 1.00 atm and 400.0 K.

13. Temperature is the measure of the average _______________ of the particles in a sample of gas?

14. Practice Why does decreasing the volumes of gas cause a nonideal behavior?

15. Practice Given the following unbalanced equation: Given 2.00 grams of water at STP, what volume of Hydrogen will be produced? H 2 0 (l) -> H 2(g) + O 2(g)

16. More Problems

17. Write the formula for Boyle’s Law

18. What are the constant for Boyle’s Law

19. If Pressure decreases, what happens to volume?

20. White formula for Charles’s Law

21. What are Charles’s Constants?

22. If volume increases, what happens to temperature?

23. Write the equation for Avogadro’s Law.

24. What were Avogadro’s Constants?

25. If the number of moles increase, what happens to volume?

26. What is the temperature of absolute zero?

27. All ____________ stops at absolute zero.

28. What pressure is required to compress 1.00 L of gas at 600.0 mm Hg pressure to a volume of 500.0 mL.

29. If 1.00 L of an ideal gas is heated from -272C to -173C, what will the volume of the gas become?

30. O=16.00g/mol R=.08206 If 64.00 grams of Oxygen gas has a volume of 4.00L, what volume would 1.00 mol of oxygen gas occupy under the same conditions.

31. N=14.00g/molR=.08206 What volume does 14.00g of nitrogen gas occupy at 2.04 atm and 60C?

32. Who is responsible for the Law of Partial Pressures?

33. The following gases: 5.00 mol Neon, 2.50 mol Oxygen gas, 2.50 mol Hydrogen gas have a total pressure of 20.0 atm. What is the partial pressure of Hydrogen Gas?

34. Leave final answer for next problem Write the equation and balance: Water decomposes to make Hydrogen gas and Oxygen gas.

35. O=16.00, H=1.00, R=.08206 If 36.00 g of water decomposes to make Hydrogen gas and Oxygen gas, what volume of Oxygen is produced at STP? Leave work for next problem

36. O=16.00, H=1.00,R=.08206 If 36.00 g of water decomposes to make Hydrogen gas and Oxygen gas, what volume of Oxygen is produced at 2.00 atm and 27.0C?