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 Study Guide:  Chapter 12, Stoichiometry

  Students should be able to...

  • Explain mole ratio
  • Convert moles, grams, atoms/molecules
  • Calculate theoretical yields when given the limiting reactant (Convert: moles A to moles B, grams A to moles B, moles A to grams B, grams A to grams B)
  • Explain limiting reactant and excess.
  • Calculate theoretical yields by finding the limiting reactant
  • Calculate percent yield.
  • Calculate percent composition.
  • Calculate theoretical yield, limiting reactant, excess, and percent yield for a double replacement reaction (laboratory)

    Practice Problems

    Find the molar mass of each compound.

    1. BaI2
    2. AgC2H3O2


    3. 0.4 moles of Sn to atoms
    4. 32 g of K2O to molecules
    5. 3.7 g of H2 to moles
    6. 800 g of CaCl2 to moles
    7. 0.75 moles of H2O to grams
    8. 9.0 g of Cl2 to atoms
    9. 0.5 moles of KNO3 to grams

    Find the percent composition for each element in the compound.

    10. Mn2O7
    11. AuNO3


    12. MgO + H2O -----> Mg(OH)2

    If you started with 3.7 moles of magnesium oxide, how many moles of magnesium hydroxide would be produced?

    13. Na + I2 ---> NaI

    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. N2 + 3 H2 ------> 2 NH3

    How many grams of ammonia were produced if you started with 10 moles of nitrogen and excess hydrogen gas?

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

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

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

    If you started with 0.97 g of K2CrO4 and 0.97g Pb(NO3)2, how many grams of KNO3 could be produced? How many grams of PbCrO4 could be produced? How much of the left over reactant will be present at the end of the reaction?


Last updated on April 3, 2006 11:06 AM