Chemistry
Name:________________________
Stoichiometry Test A
Date:__________________
Solve the following problems (*don’t forget to balance the equations!)
1.
Barium chloride and potassium hydroxide participate in a double replacement reaction.
a.
How much Ba(OH)2 is formed from 10.0 g of BaCl2?
b. What is the percent yield if only 7.25 g of Ba(OH)2 is formed in lab?
BaCl2 +
KOH →
Ba(OH)2 +
KCl
2. Ammonium nitrate decomposes to nitrogen, oxygen and water.
a.
How many grams of O2 can be formed from 34.9 g of ammonium nitrate?
b. What is the percent yield if only 6.00 g of O2 is formed experimentally?
(BONUS) c. Calculate the volume (L) of O2 gas that would be formed from 34.9 g of
ammonium nitrate.
NH4NO3 →
N2 +
O2 +
H 2O
3. Nitrogen combines with oxygen in the atmosphere during lightning flashes to produce
nitrogen monoxide. Nitrogen monoxide then reacts with O 2 to form nitrogen dioxide (shown
below).
a.
What mass of nitrogen dioxide is formed when 600. g of nitrogen monoxide reacts with
568 g oxygen?
b. What is the limiting reactant?
c.
What is the reactant in excess?
(BONUS) d. How much of the excess reactant is leftover after the above reaction has
taken place?
(BONUS) e. Find the volume (L) of NO2 produced when 160. L of NO gas combines with
excess O2.
NO +
O2 →
NO2
4. In a soda acid fire extinguisher, concentrated sulfuric acid reacts with sodium bicarbonate
to produce carbon dioxide, sodium sulfate and water.
a.
How many grams of sodium sulfate is produced from 14.5 g of sodium bicarbonate
reacting with 15.0 g of sulfuric acid (H2SO4)?
b. What is the limiting reactant?
c.
What is the reactant in excess?
(BONUS) d. How much of the excess reactant is leftover after the above reaction has
taken place?
NaHCO3 +
H2SO4 →
Na2SO4 +
CO2
+
H 2O
5. Zinc reacts with copper (II) chloride to form copper metal and zinc chloride.
a.
Write and balance the above reaction.
b. What type of reaction is this?
c.
How much copper can be obtained from a reaction between 16.0 g of zinc and 50.0 g of
copper (II) chloride?
d. What is the limiting reactant?
e.
What is the reactant in excess?
(BONUS) f. How much of the excess reactant is leftover after the above reaction has
taken place?