Practice
Questions
XI-AKUEB
Topics:
(Stiochiometry
Q.1
1 When 142 g of calcium fluoride are reacted with an
excess of sodium
bromide,
calculate the mass of calcium bromide formed.
2.
How many grams of sodium
aluminate can be obtained from 7.71 g of
aluminum
chloride according to the reaction:
AlCl3(aq) +
4NaOH(aq) = ¼ NaAlO2(aq) +
3NaCl(aq) + 2H2O(l)
3). How many
grams of carbon dioxide are
obtained when 2.96 g of
cerium(III)
oxalate are formed according to the reaction:
2Ce(IO3)4(aq)
+ 24H2C2O4(aq)= ¼ Ce2(C2O4)3(aq)
+ 4I2(aq) + 42CO2(g) + 24H2O(l)
4). Calculate the mass of sodium permanganate
that can be prepared from
1.27
g of sodium bismuthate according to the reaction:
2Mn(NO3)2
+ 5NaBiO3 + 14HNO3 = ¼ 2NaMnO4 + 5Bi(NO3)3
+ 3 NaNO3 + 7H2O
5). If excess sulfuric acid is reacted with
sodium hydroxide, 15.0 g of water
is
formed. What mass of sodium hydroxide was
used?
6).
50.0 g of calcium carbonate was added to excess phosphoric acid. What
mass
of calcium phosphate was formed?
7). Calculate the
mass of barium nitrate that must decompose in order to
produce
112 g of oxygen.
8).
Calculate the mass of potassium chloride
that is produced when 17.0 g of
potassium
carbonate reacts with hydrochloric acid.
9). When “x” grams of calcium chloride was reacted with an excess of
bromine,
14.0 kg of a gas was formed. Calculate
“x”.
10).
How many grams of zinc oxide are formed when 10.0 g of zinc reacts with
oxygen?
11.
Sodium nitrate decomposes to give 3.00 g of oxygen. Calculate the mass
of
sodium nitrate used.
12.
Potassium metal reacts with 70.0 g of chlorine. Calculate the mass of
product.
13.
Calculate the mass
of magnesium oxide that must be decomposed in
order
to produce 48.0 g of oxygen.
14). Sodium chloride was reacted with an excess
of sulfuric acid to give
hydrochloric
acid and 142 g of a second product. What
is the product,
and
how much sodium chloride was reacted?
15.
What mass of copper(I) sulfide can be produced from 9.90 g of copper(I)
chloride
reacting with an excess of hydrogen sulfide gas?
16.
How many grams of calcium hydroxide will be needed to react completely
with
10.0 g of phosphoric acid?
17.
How many grams of hydrogen can be produced from the reaction of 72.0
g
of sodium with an excess of water?
18.
An excess of nitrogen reacts with 6.57 g of hydrogen. How many grams
of
ammonia are produced?
19.
How many grams of oxygen are required to burn completely 84.9 g of
carbon? C(s)
+ O2(g) = ¼ CO2(g)
20.
In the decomposition of potassium chlorate, 82.6 g of oxygen are formed.
How
many grams of potassium chloride are produced?
21.
The action of carbon monoxide can be expressed by the equation,
Fe2O3(cr) +
3CO(g) = ¼ 2Fe(s) + 3CO2(g)
What
would be the minimum amount of carbon monoxide used if 80.3 g of
iron
were produced?
22.
How many grams of hydrochloric acid are required to react
completely
with
44.7 g of calcium hydroxide?
23.
How many grams of hydrogen are produced when 4.77 g of aluminum react
with
excess hydrochloric acid?
24.
Calculate the mass of lithium carbonate that must decompose to produce
78.0
g of carbon dioxide.
25.
How many grams of oxygen gas are formed when 100.0 g of magnesium
chlorate
are decomposed?
26.
Hydrochloric acid was reacted with zinc
to produce 137 g of hydrogen
gas. What mass of zinc did you begin with?
Q.2
Stoichiometry
- Limiting Reactants
1. Hydrogen gas can be produced in the
laboratory by the reaction of magnesium metal
with
hydrochloric acid.
a) How many grams of hydrogen can be produced
when 4.00 g of hydrochloric acid
are
added to 3.00 g of magnesium?
b) What is the volume of this hydrogen at
standard conditions?
2. Potassium
nitrate is widely used as a
fertilizer because it provides two essential
elements,
potassium and nitrogen. It is made by
mixing potassium chloride and nitric
acid
in the presence of oxygen according to the equation:
4KCl + 4HNO3 + O2 =
4KNO3 + 2Cl2 + 2H2O
How
many kilograms of potassium nitrate will be produced from 50.0 kg of potassium
chloride and 50.0 kg of nitric acid? An important by-product is chlorine. How many
kilograms
of chlorine will be produced?
3. Phosphorus forms a compound similar to
ammonia. The compound has the formula PH3
and
is called phosphine. It can be prepared
by the reaction:
P4 +
3NaOH + 3H2O = ¼
PH3 + 3NaH2PO2
If
20.0 g of phosphorus and 50.0 g of sodium hydroxide are reacted with excess
water,
how
many grams of phosphine will be obtained?
4.
Bromine can be prepared by adding
chlorine to an
aqueous solution of
sodium bromide.
How
many grams of bromine are formed
if 25.0 g of sodium bromide and 25.0 g of
chlorine
are reacted?
5. Silver
tarnishes in the presence of
hydrogen sulfide, a gas that originate from the
decay
of food, because of the reaction:
4Ag + 2H2S + O2
= ¼
2Ag2S + 2H2O
The
black product, silver sulfide, is the
"tarnish". If 25.00 g of silver, 5.00 g of
hydrogen
sulfide, and 4.00 g of oxygen are present in a reaction mixture, which one is
the
limiting reactant, and what mass of silver sulfide is produced?
6. Sulfur dioxide can be produced from the reaction of hydrogen sulfide and oxygen as
shown
by the following reaction: 2H2S + 3O2
= ¼
2SO2 + 2H2O
a) How many grams of sulfur dioxide can be
produced from 70.0 g of hydrogen
sulfide
and 125 g of oxygen.
b) How many grams of excess reactant are left
over after the reaction is complete?
7. What mass of carbon disulfide is produced
when 17.5 g of carbon are reacted with 39.5
g
of sulfur dioxide according to the equation:
5C(s) + 2SO2(g)
= ¼
CS2(s) + 4CO(g)
8. What mass of P4 is
produced when 41.5
g of Ca3(PO4)2,
26.5 g of SiO2 and 7.80 g of C
are
reacted according to the equation:
2Ca3(PO4)2
+ 6SiO2 + 10C= ¼ P4 + 6CaSiO3 + 10CO
9.
What volume of
carbon dioxide, measured
at STP, can
be produced when
15.65 g of
pentane
is reacted with 40.0 L of oxygen, measured at STP, according to the equation:
C5H12(l)
+ 8O2(g) = ¼ 5CO2(g) + 6H2O(l)
10. What mass of hydrogen chloride gas is
produced when 4.50 g of hydrogen and 140.0 g
of
chlorine are reacted. Which reactant is
in excess and how much remains unreacted?
11. The roasting of siderite ore, FeCO3,
produces ferric oxide:
4FeCO3(s)
+ O2(g) ¼ 2Fe2O3(s) + 4CO2(g)
What
mass of ferric oxide is produced when 55.0 g of siderite is reacted with 40.0 L
of
oxygen
gas? Which reactant is in excess and how
much remains unreacted?
12. A manufacturer of bicycles has 5050 wheels,
3013 frames, and 2455 handlebars.
a) How many bicycles can be manufactured using
these parts?
b) How many parts of each kind are left over?
c) Which part is like a limiting reactant in
that it limits the production of bicycles?
13. The fizz produced when an Alka-Seltzer
tablet is dissolved in water is due to the
reaction
between sodium bicarbonate and citric acid:
3NaHCO3(aq)
+ H3C6H5O7(aq) ¼ 3CO2(g)
+ 3H2O(l) + Na3C6H5O7(aq)
In a
certain experiment 1.00 g of
sodium bicarbonate and 1.00 g of citric
acid are
allowed
to react.
a) What volume of carbon dioxide is formed?
b) Which reactant is the limiting reactant?
c) How much of the excess reactant remains after
the limiting reactant is
completely
consumed?
14. One of the steps in the commercial process
for converting ammonia to nitric acid
involves
the conversion of ammonia to nitrogen monoxide:
2NH3(g)
+ 5O2(g) = ¼ 4NO(g) + 6H2O(g)
In
a certain experiment 2.50 g of ammonia reacts with 2.85 g of oxygen.
a) What mass of nitrogen monoxide is formed?
b) Which reactant is the limiting reactant?
c) How much of the excess reactant remains after
the limiting reactant is
completely
consumed?
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