MORE STOICHIOMETRY WITH LIMITING AND EXCESS REAGENTS
1)
15.50 g of lead (II) nitrate is reacted with 3.81 g of sodium chloride.
a) Which reactant is in excess?
b) Calculate the mass of excess.
c) Calculate the mass of lead chloride produced.
2)
8.99 L of SO2 (g) reacts with 10.2 L of CO2 (g) to form SO3 (g) and CO (g).
a) Calculate the volume of each gas produced at RTP.
b) Why was it not necessary to convert the litres of reactants into moles at RTP?
3)
Why would an excess of one reagent be used in a chemical reaction?
4)
7.98 g of iron (III) oxide reacts with 3.92 L of carbon monoxide to form solid iron
and carbon dioxide gas. If the reaction occurs at RTP, find the mass of iron and
the volume of carbon dioxide produced.
(this is an important industrial reaction in which the iron (III) oxide from ores of iron is
converted to iron in blast furnaces)
5)
AlCl3 +
1.41 moles
K
--->
KCl
+
Al
5.34 moles
If 313 g of KCl is produced, the minimum grams of each reactant should be:
a) 187 g AlCl3 and 55.0 g K
b) 188 g AlCl3 and 165 g K
c) 133 g AlCl3 and 117 g K
d) 237 g AlCl3 and 208 g K
6)
How many grams of barium hydroxide will be used up in the reaction with
hydrochloric acid to produce 45.00 g of barium chloride plus some water?
7)
Calculate the number of moles of NaOH required to remove the sulphur dioxide
from 10.0 metric tons (10.0 x 106 g) of atmosphere if the sulphur dioxide is 0.10%
by mass? (note: sodium sulphite and water are the products).
8)
How much sulphur dioxide is produced by the reaction of 1.00 g Sulphur and all
the oxygen in the atmosphere on earth?
9)
SO2 (g)
9.0L
10)
N2O4 (g)
11.8 L
+ CO2 (g) -->
10.2 L
-->
SO3 (g) +
_______
N2 (g) +
O2 (g)
_____
21.5 L
______
CO (g)