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Stoichiometry: Review Questions for AP Chemistry

By — McGraw-Hill Professional
Updated on Feb 1, 2011

Review the following concepts if necessary:

Problems

Answer the following questions. You have 25 minutes, and you may not use a calculator. You may use the periodic table in the back of the book. For each question, circle the letter of your choice.

  1. How many milliliters of 0.100 M H2SO4 are required to neutralize 50.0 mL of 0.200 M KOH?
    1. 25.0 mL
    2. 30.0 mL
    3. 20.0 mL
    4. 50.0 mL
    5. 60.0 mL
  2. A sample of oxalic acid, H2C2O4, is titrated with standard sodium hydroxide, NaOH, solution. A total of 45.20 mL of 0.1200 M NaOH is required to completely neutralize 20.00 mL of the acid. What is the concentration of the acid?
    1. 0.2712 M
    2. 0.1200 M
    3. 0.1356 M
    4. 0.2400 M
    5. 0.5424 M
  3. A solution is prepared by mixing 50.0 mL of 0.20 M arsenic acid, H3AsO4, and 50.0 mL of 0.20 M sodium hydroxide, NaOH. Which anion is present in the highest concentration?
    1. HAsO42–
    2. OH
    3. H2AsO4
    4. Na+
    5. AsO33–
  4. 14 H+ + 6 Fe2+ + Cr2O7 2– → 2 Cr3+ + 6 Fe3+ + 7 H2O
  5. This reaction is used in the titration of an iron solution. What is the concentration of the iron solution if it takes 45.20 mL of 0.1000 M Cr2O7 2– solution to titrate 50.00 mL of an acidified iron solution?

    1. 0.5424 M
    2. 0.1000 M
    3. 1.085 M
    4. 0.4520 M
    5. 0.2712 M
  6. Tungsten metal may be prepared by reducing WO3 with H2 gas. How many grams of tungsten may be prepared from 0.0500 mol of WO3 with excess hydrogen?
    1. 5.58 g
    2. 0.500 g
    3. 9.19 g
    4. 184 g
    5. 18.4 g
  7. Manganese, Mn, forms a number of oxides. A particular oxide is 63.2% Mn. What is the simplest formula for this oxide?
    1. MnO
    2. Mn2O3
    3. Mn3O4
    4. MnO2
    5. Mn2O7
  8. Vanadium forms a number of oxides. In which of the following oxides is the vanadium-to-oxygen mass ratio 2.39:1.00?
    1. VO
    2. V2O3
    3. V3O4
    4. VO2
    5. V2O5
  9. How many grams of nitrogen are in 25.0 g of (NH4)2SO4?
    1. 5.30 g
    2. 1.30 g
    3. 0.190 g
    4. 2.65 g
    5. 14.0 g
  10. Nitrogen forms a number of oxides. Which of the following oxides is 64% nitrogen?
    1. N2O5
    2. N2O4
    3. N2O3
    4. N2O2
    5. N2O
  11. Sodium sulfate forms a number of hydrates. A sample of a hydrate is heated until all the water is removed. What is the formula of the original hydrate if it loses 43% of its mass when heated?
    1. Na2SO4·H2O
    2. Na2SO4·2H2O
    3. Na2SO4·6H2O
    4. Na2SO4·8H2O
    5. Na2SO4·10H2O
  12. 3Cu(s) + 8HNO3(aq) → 3Cu(NO3)2(aq) + 2 NO(g) + 4 H2O(l)
  13. Copper metal reacts with nitric acid according to the above equation. A 0.30-mol sample of copper metal and 10.0 mL of 12 M nitric acid are mixed in a flask. How many moles of NO gas will form?

    1. 0.060 mol
    2. 0.030 mol
    3. 0.010 mol
    4. 0.20 mol
    5. 0.10 mol
  14. Gold(III) oxide, Au2O3, can be decomposed to gold metal, Au, plus oxygen gas, O2. How many moles of oxygen gas will form when 221 g of solid gold(III) oxide is decomposed? The formula mass of gold(III) oxide is 442.
    1. 0.250 mol
    2. 0.500 mol
    3. 1.50 mol
    4. 1.00 mol
    5. 0.750 mol
  15. __C4H11N(1) + __O2(g) →__CO2(g) + __H2O(l) + __N2 (g)
  16. When the above equation is balanced, the lowest whole number coefficient for O2 is:

    1. 4
    2. 16
    3. 22
    4. 27
    5. 2
  17. 2 KMnO4 + 5 H2C2O4 + 3 H2SO4 → K2SO4 + 2 MnSO4 + 10 CO2 + 8 H2O
  18. How many moles of MnSO4 are produced when 1.0 mol of KMnO4, 5.0 mol of H2C2O4, and 3.0 mol of H2SO4 are mixed?

    1. 4.0 mol
    2. 5.0 mol
    3. 2.0 mol
    4. 2.5 mol
    5. 1.0 mol
  19. __KClO3 → __KCl + __O2
  20. After the above equation is balanced, how many moles of O2 can be produced from 4.0 mol of KClO3?

    1. 2.0 mol
    2. 4.0 mol
    3. 5.0 mol
    4. 6.0 mol
    5. 3.0 mol
  21. When the following equation is balanced, it is found that 1.00 mol of C8H18 reacts with how many moles of O2?
  22. __C8H18 + __ O2 → __ CO2 + __ H2O

    1. 1.00 mol
    2. 10.0 mol
    3. 25.0 mol
    4. 37.5 mol
    5. 12.5 mol
  23. Ca + 2 H2O → Ca(OH)2 + H2
  24. Calcium reacts with water according to the above reaction. What volume of hydrogen gas, at standard temperature and pressure, is produced from 0.200 mol of calcium?

    1. 5.60 L
    2. 2.24 L
    3. 3.36 L
    4. 1.12 L
    5. 4.48 L
  25. 2CrO42– + 3SnO22– + H2O → 2 CrO2 + 3 SnO32– + 2 OH
  26. How many moles of OH form when 50.0 mL of 0.100 M CrO42– is added to a flask containing 50.0 mL of 0.100 M SnO22–?

    1. 0.100 mol
    2. 6.66 × 10–3 mol
    3. 3.33 × 10–3 mol
    4. 5.00 × 10–3 mol
    5. 7.50 × 10–3 mol
  27. A solution containing 0.20 mol of KBr and 0.20 mol of MgBr2 in 2.0 liters of water is provided. How many moles of Pb(NO3)2 must be added to precipitate all the bromide as insoluble PbBr2?
    1. 0.10 mol
    2. 0.50 mol
    3. 0.60 mol
    4. 0.30 mol
    5. 0.40 mol
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