Objectives: Determine which reactant is all
used up and which is in excess in a chem reaction.
Announcements: I would like to get notebooks this week.
Rockets will get graded (construction & pizzazz)
on Thurs. (this week, 5/5)
When magnesium combusts in the air, some little bit of the magnesium
reacts with nitrogen, rather than oxygen. Write the balanced equation
for the reaction that produces magnesium nitride. Now suppose 1.10 g
of nitrogen gas actually reacts with some of the magnesium, how many
grams of magnesium nitride is created?
Limiting reactant and percent yield:
90.0 g of FeCl3 reacts with 52.0 g of H2S. What is the
limiting reactant? What is the mass of HCl produced?
What mass of excess reactant remains after the reaction?
If only 55 grams of HCl is actually produced, what was
the percent yield for this reaction?
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