Name: _______________________________________ Date: _______________ Mods: __________
Stoichiometry Review Worksheet
1)
Using the following balanced equation:
2 NaOH (aq) + H2SO4 (aq)  2 H2O (l) + Na2SO4 (aq)
How many grams of sodium sulfate will be formed if you start with 200 grams of sodium
hydroxide and you have an excess of sulfuric acid?
2)
Using the following balance equation:
Pb(NO3)4 (aq) + 2 Li2SO4 (aq)  Pb(SO4)2 (s) + 4 LiNO3 (aq)
How many moles of lead (IV) nitrate will be needed to produce 175 grams of lithium nitrate,
assuming that you have more than enough of lithium sulfate to complete the reaction?
3)
Use the following UNBALANCED equation:
____ C6H10 (l) + ____ O2 (g)  ____ CO2 (g) + ____ H2O (l)
How many moles of oxygen are needed to produce 1.5 moles of carbon dioxide?
4)
Use the following UNBALANCED equation:
____ N2 + ____ F2  ____ NF3
How many grams of nitrogen would be required to react with 3.67 moles of fluorine?
Limiting Reactants, Excess Reactant, & Percent Yield
5)
When copper metal is heated with an excess of sulfur, copper (I) sulfide is formed.
2 Cu (s) + S (s)  Cu2S (s)
a) Suppose that 233 grams of copper react with 188 grams of sulfur. Which reactant would
be the limiting reactant? Which reactant would be the excess reactant? What is the
theoretical yield, in grams, of copper (I) sulfide that would be produced?
Limiting Reactant = _____________
Excess Reactant = _____________
Theoretical Yiled = _______________________________________
b) In the laboratory you actually produced a mass of 274.8 grams of copper (I) sulfide. What
is the percent yield of this experiment?
c) Using the theoretical yield from part a, determine the actual yield of copper (I) sulfide if the
percent yield in a different trial of the experiment was only 55.7%?