Mr. O
Title: Single replacement reaction
Name:
Relating Moles to Coefficients of a Chemical Equation
Equipment: Balance, burner, 100mL and 250 mL beakers, 100mL graduated cylinder, ring stand, wire
gauze, stirring rod
Materials: 8 grams in 50 ml Copper sulfate and 2.24 g iron filings
Procedure:
Observation and Data:
a. Mass of empty beaker _______
b. Mass of iron filings _______
c. Mass of beaker + copper _______
d. Visual Observation
Calculations:
1. Find the mass of copper produced (c-a)
2. Find the number of moles of copper produced
3. Find the number of moles of iron reacted
4. Find the whole number ratio of moles of iron to moles of copper
Conclusion and Questions:
1. How does the mole ratio in calculation 4 compare to the ratio in the balanced equation?
2. How many moles of copper sulfate are used to produce the solution in this experiment? Why
is this amount of copper sulfate said to be “in excess”?
3. Explain why iron is the limiting factor in this experiment?
4. Why is this reaction a single replacement reaction? Give an example of another.
5. Consider the reaction: Cu + 2AgNO3  2Ag + Cu(NO3)2 if 3 moles of copper metal reacts,
how many moles of silver will be produced?