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WorksheetsStoichiometry
Total questions: 16
Worksheet time: 1hrs 4mins
Name
Class
Date
1.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 6 moles H2?
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 6 moles H2?
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
2.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)
12.00 moles of NaClO3 will produce how many grams of O2?
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
3.
What is the limiting reactant if 10 moles of NH3 react with 30.0 moles of NO?
4NH3+6NO --> 5N2 + 6H2O
4NH3+6NO --> 5N2 + 6H2O
a)
NH3
b)
NO
c)
N2
d)
water
4.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
5.
Fe (s) + S (l) --> FeS (s)
In the experiment above, 7.62 g of Fe are allowed to react with 8.67 g of S.
How much FeS is formed?
In the experiment above, 7.62 g of Fe are allowed to react with 8.67 g of S.
How much FeS is formed?
a)
14.8 g
b)
12.2 g
c)
13.7 g
d)
19.9 g
6.
Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.
Mg + 2HCl --> MgCl2 + H2
Mg + 2HCl --> MgCl2 + H2
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
7.
When two substances react to form products, the reactant which is used up is called the_____.
a)
excess reactant
b)
limiting reactant
c)
catalytic reactant
d)
determining reactant
8.
What can be determined from a balanced chemical equation?
a)
Mole ratio of any two substances in the reaction
b)
Energy released in the reaction.
c)
Electron configuration of all elements in the reaction.
d)
Mechanism involved in the reaction.
9.
Lead nitrate can be decomposed by heating. What is the % yield of the decomposition reaction if 7.4g Pb(NO3)2 are heated to give 4.1 g PbO?
2Pb(NO3)2 (s)→2PbO(s)+4NO2(g)+O2(g)
2Pb(NO3)2 (s)→2PbO(s)+4NO2(g)+O2(g)
a)
82%
b)
44%
c)
56%
d)
67%
10.
What is the empirical formula for a compound containing: 92.30% carbon and 7.70% hydrogen
a)
CH
b)
CH4
c)
C2H4
d)
C2H4
11.
What is the empirical formula if you have 36.84% nitrogen and 63.16% oxygen?
a)
NO
b)
N2O3
c)
N2O4
d)
N2O5
12.
Given the following: 42.07% Na, 18.89% P, and 39.04% O, determine the empirical formula.
a)
NaPO2
b)
Na2PO3
c)
Na3PO4
d)
NaPO4
13.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.
a)
SO
b)
SO2
c)
SO3
d)
SO4
14.
How many grams of H2O will be formed when 16.0 g H2 is allowed to react with 16.0 g O2 according to
2H2 + O2 → 2H2O?
a)
18.0 g
b)
144 g
c)
9.00 g
d)
32.0 g
15.
Calculate the mass of hydrogen formed when 25 g of aluminum reacts with excess hydrochloric acid.
2Al + 6HCl → 2 AlCl3 + 3H2
a)
0.41 g
b)
0.92 g
c)
1.2 g
d)
2.8 g
16.
The reaction of 25.0 g benzene, C6H6, with excess HNO3 resulted in 21.4 g C6H5NO2. What is the percentage yield?
C6H6 + HNO3 → C6H5NO2 + H2O
a)
100%
b)
27.4%
c)
54.3%
d)
85.6%
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