1. 2 pt 3 pt 4 pt 5pt 1 pt 2 pt 3 pt 4 pt 5 pt 1 pt 2pt 3 pt 4pt 5 pt 1pt 2pt 3 pt 4 pt 5 pt 1 pt 2 pt 3 pt 4pt 5 pt 1pt ConversionsGas Laws Molar Mass Equations Everything & Anything

2. What is the molar mass of hydrogen gas?

3. H 2 = 2.0 g/mol

4. Define molar mass.

5. The sum of atomic masses of all the atoms in a compound.

6. Find the molar mass of sodium chloride.

7. Na = 23.0 g Cl = 35.5 g 58.5 g/mol NaCl

8. Find the percent composition of calcium hydroxide.

9. Ca(OH) 2 Ca = 40.0 x 1 = 40.0 g/74.0 g = 54.05% O = 16.0 x 2 = 32.0 g/74.0 g = 43.24% H = 1.0 x 2 = 2.0 g/74.0 g = 2.70% 74.0 g /mol Ca(OH) 2

10. What is the mass of 2 moles of barium acetate?

11. Ba(CH 3 CO 2 ) 2 Ba = 137.3 x 1 = 137.3 C = 12.0 x 4 = 48.0 H = 1.0 x 6 = 6.0 O = 16.0 x 4 = 64.0 255.3 g /mol Ba(CH 3 CO 2 ) 2 X 2 mol = 510.6 g

12. Why must a chemical equation be balanced?

13. A balanced equation reflects the law of conservation of mass. The mass of the products must be equal to the mass of the reactants.

14. Balance the following equation: _____ Al + _____ FeO _____ Al 2 O 3 + _____ Fe

15. 2Al + 3FeO Al 2 O 3 + 3Fe

16. If 6 moles of nitrogen reacts with hydrogen how many moles of ammonia will be produced? N 2 + 3H 2 2NH 3

17. 12 moles of ammonia

18. Write a balanced chemical equation for the combustion of Ethane (C 2 H 6 ).

19. 2C 2 H 6 + 7O 2 4CO 2 + 6H 2 O

20. Write a balanced chemical equation for the reaction of: Potassium sulfate and hydrochloric acid

21. K 2 SO 4 + 2HCl 2KCl + H 2 SO 4

22. What is the molar volume of any gas at STP?

23. 22.4 L

24. How many atoms are in one mole of any substance?

25. 6.02 x 10 23 atoms Avogadro's Number

26. How many moles are in 326.5 grams of magnesium sulfide?

27. Molar mass = 56.4 g/mol MgS 5.8 mol MgS

28. How many molecules of hydrogen gas are in 523 L at STP?

29. 1.41 x 10 25 molecules

30. Which contains more molecules, 15.0 g CO or 22.5 g CO 2 ?

31. 15.0 g CO contains more molecules.

32. Which gas law describes the relationship between pressure and volume? What is their mathematical relationship?

33. Boyle’s Law Inversely proportional

34. Which has law describes what happens when you put too much air into a balloon?

35. Avogadro’s Law n  V

36. Use the kinetic theory to explain what happens to a gas in an enclosed container when temperature increases.

37. As temperature increases, particles begin to move faster (increase in KE) and collide more with the sides of the container, as a result pressure increases.

38. If a gas at 25.0 °C occupies 3.60 liters at a pressure of 760 mm Hg, what will be its volume at a pressure of 2.50 atm, if temperature is kept constant?

39. Boyle’s Law 1.44L

40. At a pressure of 780.0 mm Hg and 24.2 °C, a certain gas has a volume of 350.0 mL. What will be the volume of this gas under STP?

41. Combined Gas Law 329.96 mL or 0.33 L

42. How many moles of chlorine would react with 6 moles of sodium? 2Na + Cl 2 2NaCl

43. 3 moles of Chlorine

44. Describe the difference between a limiting reactant and an excess reactant.

45. The limiting reactant limits/determines the amount of product that can be formed in the reaction. It is completely used up in the reaction. The reactant that is NOT completely used up in a reaction is called the excess reagent/reactant.

46. Find the empirical formula of a compound given that the compound is found to be 47.9% zinc and 52.1% chlorine by mass.

47. ZnCl 2

48. Determine the molecular formula of a compound, given that a 212.1 gram sample of the compound contains 42.4 grams of hydrogen and 169.7 grams of carbon and the molar mass is 30.0 g/mol.

49. C2H6C2H6

50. Identify the limiting reactant when 7.81g of hydrogen chloride reacts with 5.24g of sodium hydroxide to produce sodium chloride and water.

51. Sodium hydroxide is the limiting reactant.

52. Final Jeopardy!! 100 grams of calcium carbonate reacts with 45 grams of iron (III) phosphate to produce calcium phosphate and Iron (III) carbonate. What is the percent yield if 37.28 grams of calcium phosphate is produced?