Name: ________________________ Date:_____________
Chemistry: Ch. 10.4 Limiting Reactants – Problem Sheet 3
Use notes and textbook examples to complete this worksheet. Refer to textbook pages 275-280. (Use lined paper
for more work space if needed). Classwork grade. To be turned in.
1. How many grams of AlCl3 may be produced when 81.0 grams of Al reacts with 188 grams of Cl2?
a. Determine the balanced chemical equation.
b. Determine the moles of each reactant from their given quantity.
c. Convert one of the reactant moles to the moles of the other reactant (Try converting moles of Cl2
[calculated in step b] to moles of Al using mole ratio)
d. To identify the limiting reactant, compare the amount of aluminum calculated from step c with the given
amount of aluminum from step b.
If the amount calculated in step c is greater than the given amount, aluminum is the limiting reactant
If the amount calculated step c is less than the given amount, aluminum is in excess
Which is the limiting reactant, Al or Cl2?
e. Once the limiting reactant has been determined, use the given moles of the limiting reactant and convert to
grams of AlCl3 (use mole ratio).
2.
C2H4
+
O2
→
CO2 +
H2 O
a. Balance the equation.
b. If 75.6 grams of C2H4 reacts with 201.6 grams of O2, which is the limiting reactant?
c. How many grams of CO2 are formed?
3. In a single-replacement reaction, how many grams of MgCl2 may be produced when 6.00 grams of
HCl reacts with 5 grams of Mg?
a. Determine the balanced chemical equation.
b. Which is the limiting reactant?
c. How many grams of MgCl2 are produced?
4. Carbon reacts with water at high temperatures to produce hydrogen and carbon monoxide.
a. Write a balanced equation
b. If 29 g of carbon reacts with 56 g of water, identify the limiting reactant.
c. How many moles of each product are formed?
d. What is the mass of each product formed?