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  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

  Convert.

  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

  Stoichiometry

  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?