Honors Chemistry
Stoichiometry Practice
Name __________________________
4-9-15
COMPLETE THE FOLLOWING ON YOUR OWN PAPER! SHOW ALL YOUR WORK FOR CREDIT. You can
use the Formula Weight Calculator at http://bit.ly/1xf4yqg as needed as well as the
computer’s calculator to solve problems.
Ways to lose points:



Failure to balance the equation if needed.
Failure to label/cancel units in the dimensional analysis.
Get the wrong answer without showing how you got it!
Problem #1 Mass-Mass
When Calcium Carbonate (CaCO3) is reacted with Hydrobromic Acid (HBr), Calcium Bromide (CaBr2),
Water (H2O) and Carbon Dioxide (CO2). How many grams of Calcium Bromide can be formed if 175.4
grams of Calcium Carbonate react with an unlimited supply of Hydrobromic Acid?
The equation for the reaction is:
CaCO3 +
HBr

CaBr2 +
H2O
+
CO2
Problem #2 Mass-Mass with a Limiting Reagent
*Remember in a limiting reagent problem you will have to work at least TWO problems: choose the substance that gives the least product as
your limiting reagent and the other as the excess.
If 25.5 grams of Magnesium (Mg) are reacted with a solution containing 45.9 grams of Copper (II)
Nitrate, Cu(NO3)2, how many grams of Magnesium Nitrate, Mg(NO3)2, can be formed? The equation for
the reaction is:
Mg + Cu(NO3)2  Mg(NO3)2 + Cu
Problem #2 Mass-Volume
Sulfur Dioxide, SO2 [which has the odor of rotten eggs] is produced as a byproduct when a naturally
occurring ore of iron, Iron (II) Sulfide, FeS, is heated in the presence of Oxygen, O2, to form Iron (III)
Oxide, Fe2O3. The balance equation for the reaction is:
4 FeS
+ 7O2
→
2 Fe2O3
+
4 SO2
How many liters of Sulfur Dioxide are formed when 585.0 grams of Iron (II) Sulfide are “roasted”?
[“roasted” is the term used to describe processes such as this].