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.
4. BaI2 / 5. AgC2H3O2Convert.
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.
11. Mn2O7 / 12. AuNO3Stoichiometry
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.
Mass of empty container / 22.347 gInitial mass of sample and container / 25.825 g
Mass of sample and container after first heating / 23.982 g
Mass of sample and container after second heating / 23.976 g
Mass of sample and container after third heating / 23.977 g
66. Determine the moles of water lost when the sample was heated.
67. Determine the formula of the hydrated compound.