Chemistry Final Review Problem Set

Chemistry Name ______

Block ___ Date ___/___/___

SLO Final Review

Problem Set

Balance these equations:

1. _____Ca(OH)2(s) + _____HCl(aq) ---> ____CaCl2(aq) + _____H2O(l)

2. _____Ag2O(s) ---> _____Ag(s) + _____O2(g)

3. _____C4H10(g) + _____O2(g) ---> _____CO2(g) + _____H2O(g)

Find the molecular weight of each compound.

Convert.

6. 0.4 moles of Sn to atoms

7. 32 g of K2O to molecules

8. 800 g of CaCl2 to moles

9. 0.75 moles of H2O to grams

10. 9.0 g of Cl2 to atoms

Find the percent composition for each element in the compound.

Stoichiometry

13. Na + I2 ---> NaI

a.  If 2.8 grams of sodium were used for the reaction, and an excess of iodine was present, how many moles of sodium iodide would be produced?

14. Pb(NO3)2 + K2CrO4 --> PbCrO4 + 2 KNO3

b.  If you started with 0.97 g of K2CrO4 and excess Pb(NO3)2, how many grams of KNO3 could be produced?

Reactions. Complete and balance.

15. K2CO3 + BaCl2 --->

16. NaCl + O2 --->

17. Zn(CO3) --->

18. RaCl2 --->

19. C6H6 + O2 --->

20. Ra + Cl2 --->

Name the following compounds (some could be acids).

21. H3PO3

22. HCl

23. H2Se

24. HNO2

25. H2CO3

26. CuF

27. CdI2

28. HI

29. NO

30. NF3

31. N2Cl2

32. CF4

33. KCl

34. NaNO3

35. Ca(NO2)2

36. Mg3(PO4)2

Write the formula for each of the following compounds:

37. Sulfur difluoride

38. Sulfur hexafluoride

39. Phosphoric acid

40. Lithium nitride

41. Chromium (III) carbonate

42. Tin (II) fluoride

43. Ammonium acetate

44. Perchloric acid

45. Cobalt (III) nitrate

46. Copper (II) chloride

47. Potassium sulfite

48. Sodium hydroxide

Molarity

49. What is the molarity of 5.00 g of NaOH in 750.0 mL of solution?

50. How many moles of Na2CO3 are there in 10.0 L of 2.0 M soluton?

Percent mass/Percent volume

51. What is the percent by mass of 5.0 g of iron (II) sulfate dissolved in 75.0 g of water?

52. An experiment requires a solution that is 80% methyl alcohol by volume. What volume of methyl alcohol should be

added to 200 mL of water to make this solution?

53. A solution is made by adding 25 mL of benzene to 80 mL of toluene. What is the percent by volume of benzene?

54.. A solution is formed by adding 35 g of ammonium nitrate to 250 g of water. What is the percent by mass of

ammonium nitrate?

Stoichiometry: Limiting reactants and Percent Yield

55. Disulfur dichloride, S2Cl2, is used to vulcanize rubber. It can be made by treating molten sulfur with gaseous

chlorine:

56. S8(l) + 4 Cl2(g) ® 4 S2Cl2(l)

57. Starting with a mixture of 32.0 g of sulfur and 71.0 g of Cl2, which is the limiting reactant?

58. What mass of S2Cl2 (in grams) can be produced?

59. What mass of the excess reactant remains when the limiting reactant is consumed?

60. Methyl alcohol (wood alcohol), CH3OH, is produced via the reaction: CO(g) + 2 H2(g)  CH3OH (l)

61. A mixture of 1.20 g H2(g) and 7.45 g CO(g) are allowed to react.

(a)  Which reagent is the limiting reagent?

(b)  What is the yield of CH3OH? [Assume theoretical yield in g is what is

wanted here.]

(c)  How much of the reagent present in excess is left over?

(d)  Suppose the actual yield is 7.52 g of CH3OH. What is the % yield?

62. A compound contains 36.48% Na, 25.41% S, and 38.11% O. What is the empirical formula?

63. A carbon, oxygen and hydrogen containing compound is 58.8%C. 9.8% H, and 31.4% O. Its molar mass is 102

g/mol. What is its molecular formula?

HYDRATE LAB

64. A student is assigned the task of determining the number of moles of water in one mole of MgCl2 · n H2O.

65. The student collects the data shown in the following table.

66. Determine the moles of water lost when the sample was heated.

67. Determine the formula of the hydrated compound.