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WorksheetsUnit 5.2 Stoichiometry
Total questions: 62
Worksheet time: 3hrs 21mins
Name
Class
Date
1.
What is the molar mass of NaCl?
a)
1.5 g/mol
b)
22.99 g/mol
c)
58 g/mol
d)
0.22 mol/g
2.
Balance the following reaction :
CaC₂(s) + H₂O(l) --> C₂H₂(g) + Ca(OH)₂(aq)
CaC₂(s) + H₂O(l) --> C₂H₂(g) + Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
3.
What is the molar mass of C3H8?
a)
44 g/mol
b)
0.44 mol
c)
4.4 g/mol
d)
4.4 g
4.
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)
2 moles Fe
b)
1 moles Fe
c)
9 moles Fe
d)
4 moles Fe
5.
N2 + 3H2 → 2NH3
How many moles of hydrogen gas are needed to react with 2 moles of nitrogen gas?
How many moles of hydrogen gas are needed to react with 2 moles of nitrogen gas?
a)
2 mol
b)
6 mol
c)
3 mol
d)
4 mol
6.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the mole ratio of MgO to Fe?
a)
1 mol Mg / 2 mol Fe
b)
2 mol Mg / 3 mol Fe
c)
1 mol Fe / 2 mol Mg
d)
3 mol MgO / 2 mol Fe
7.
2H2 + O2 → 2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2 mol
b)
4 mol
c)
6 mol
d)
8 mol
8.
How many grams of oxygen gas is produced from 202g of potassium nitrate?
2KNO3 --> 2KNO2 + O2
2KNO3 --> 2KNO2 + O2
a)
16
b)
64
c)
100
d)
32
9.
What is the first thing you must do to solve a stoichiometry problem?
a)
Write a Balanced Equation
b)
Solve for the Unknown
c)
Write the mole ratio
d)
Solve for mass of A (known)
10.
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
11.
How many grams are in one mole of Oxygen gas (O2)
a)
16 g/mol
b)
32 g/mol
c)
2 g/mol
d)
1/16 g/mol
12.
In the reaction 2 H2 + O2 → 2 H2O what is the mole ratio of oxygen to water
a)
1:2
b)
2:1
c)
3:4
d)
4:3
13.
What is the molar mass of CH4
a)
16.05
b)
4.04
c)
12.01
d)
32.32
14.
Calculate the molar mass of Mg(OH)2.
a)
33.2 g/mol
b)
41.3 g/mol
c)
86.9 g/mol
d)
58.3 g/mol
15.
2NaClO3 (s) → 2NaCl (s) + 3O2 (g)
53 grams of NaClO3 will produce how many grams of NaCl?
(Molar Mass: NaClO3 = 106g, NaCl = 58g and O2 = 32g)
a)
29.0 g of NaCl
b)
19.3 g of NaCl
c)
43.5 g of NaCl
16.
2H2 + O2 → 2H2O
How many grams of water can be produced if 4.0 moles H2 are used?
(Molar Mass = H2 = 2g, O2 = 32g and H2O = 18g)
a)
0.89g
b)
72.0 g
c)
8.0 g
d)
13.33g
17.
The limiting reactant
a)
speeds up the chemical reaction
b)
is the first reactant to run out
c)
is the reactant that is left over
18.
When does a chemical reaction stop?
a)
When the temperature of the reaction drops
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
19.
Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3. If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.
a)
AlCl3
b)
Cl2
c)
Al
20.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
21.
P4 + 3O2 --> P4O6
What is the limiting reactant is 12 moles of P4 react with 15 moles of O2?
What is the limiting reactant is 12 moles of P4 react with 15 moles of O2?
a)
P4
b)
O2
c)
P4O6
d)
none of the above
22.
What is the theoretical yield?
a)
the maximum amount of product from a reaction
b)
the amount of product recovered from a lab experiment
c)
amount of product that causes the reaction to stop
d)
the amount of product needed to reverse the reaction
23.
When reacting Na with Cl2, we calculated that the theoretical yield should be 12.5 grams. Our actual yield was 13.0 grams. What is the percent yield?
a)
100%
b)
104%
c)
96%
d)
1.04
24.
What is the molar mass of C6H12O6?
a)
180.18
b)
180.21
c)
180.42
d)
181.00
25.
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
26.
Balance the following reaction :
CaC₂(s) + H₂O(l) --> C₂H₂(g) + Ca(OH)₂(aq)
CaC₂(s) + H₂O(l) --> C₂H₂(g) + Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
27.
In the equation 6 CO2 + 6 H2O → C6H12O6 + 6 O2, the mole ratio of water to oxygen is:
a)
6:6
b)
1:6
c)
6:1
28.
How many grams are in 7.8 moles of NaCl?
a)
476grams
b)
460 grams
c)
453 grams
d)
462 grams
29.
How many grams are in 3.3 mol of Potassium Sulfide (K2S)?
a)
363 g
b)
454 g
c)
238 g
d)
132 g
30.
How many atoms of iodine are in a mole of iodine?
a)
53
b)
63.55g
c)
126.9
d)
6.02 x 1023
31.
The number 6.02 x 1023 is called...
a)
Obama's number
b)
Bohr's number
c)
Trump's number
d)
Avogadro's number
32.
How many particles would be in 8.4 moles of Octane (C8H18)?
a)
5.77 x 1023
b)
5.04 x 1024
c)
5.77 x 1026
d)
5.04 x 1023
33.
How many molecules are in 32.4 grams of phosphorous pentoxide?
a)
1.76 x 1023 molecules
b)
0.29 moles
c)
1.76 x 1022 molecules
d)
0.29 molecules
34.
Which has more molecules?
a)
1 mole H2O
b)
1 mole Al(OH)3
c)
1 mole NaCl
d)
There are all the same
35.
How many molecules are present in 25 g of NaBr?
a)
102.96 molecules
b)
0.24 molecules
c)
1.45x1023 molecules
d)
2.34 x 1020molecules
36.
What is the mass of 54.3x1045molecules of BeO?
a)
3.27x1070 g
b)
9.01 x1022g
c)
2.25 x1024 g
d)
1.31 x1069g
37.
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.
38.
What is the molecular formula if the empirical formula is C2H5 and the molecular molar mass is 58.14 g/mol?
a)
C2H5
b)
C4H10
c)
C1H2.5
d)
C4H8
39.
Find the percent composition of N2S2.
a)
N: 69.6% S: 30.4%
b)
N:36% S: 75.6%
c)
N: 96.6% S: 3.4%
d)
N: 30.4% S: 69.6%
40.
Find the percent composition of Mg in Mg3(PO4)2.
a)
27.75% Mg
b)
23.57% Mg
c)
48.68% Mg
d)
13.45% Mg
41.
What is the Law of Conservation of mass?
a)
Mass is created in a chemical reaction
b)
Mass is created in a physical change
c)
New chemicals formed from a chemical reaction have a larger overall mass than the original reactants
d)
Mass is never created or destroyed
42.
In this image, what are the information in red or orange is called the_______.
a)
Product
b)
Reactant
c)
Chemical Subscript
43.
In this image, what are the information to the right of the arrow (in black) is called the_______.
a)
Product
b)
Reactant
c)
Chemical Subscript
44.
Whats the empirical formula of a molecule containing 18.7% of Lithium, 16.3% of Carbon and 65.0% of oxygen?
a)
CO2Li3
b)
Li2CO3
c)
Li3CO2
d)
LiCO5
45.
What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?
a)
CH2O
b)
C2H4O2
c)
C4H8O4
d)
C6H12O6
46.
Find the percent composition of hydrogen in ammonium sulfide.
a)
11.8%
b)
41.1%
c)
47.1%
47.
Which of the following dimensional analysis setups will correctly convert 27.76g of Li to atoms of Li?
a)
A
b)
B
c)
C
d)
D
48.
What is the mole ratio in the following reaction:
2CO + O2 → 2CO2
2CO + O2 → 2CO2
a)
2:1:2
b)
1:1:1
c)
1:2:1
d)
Have no clue what a mole ratios is!!
49.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
50.
The limiting reactant
a)
slows the reaction down
b)
is used up first
c)
is the reactant that is left over
d)
controls the speed of the reaction
51.
A formula with the lowest whole # ratio of elements in a compound is called
a)
empirical formula
b)
chemical formula
c)
covalent formula
d)
molecular formula
52.
KMnO4
a)
Empirical
b)
Molecular
53.
C2H6
a)
Empirical
b)
Molecular
54.
You need 2 pieces of bread, 1 tablespoon of peanut butter and 2 tablespoons of jelly to make a sandwich. If you have 10 pieces of bread, 4 tablespoons of peanut butter and 20 tablespoons of jelly, what is the limiting reactant?
a)
bread
b)
jelly
c)
peanut butter
d)
sandwich
55.
Which is limiting for the reaction below:
3 A + 4B + 2C --> A3B4C2
If you start with the following quantities:
10 moles of A
9 moles of B
6 moles of C
3 A + 4B + 2C --> A3B4C2
If you start with the following quantities:
10 moles of A
9 moles of B
6 moles of C
a)
A is limiting
b)
B is limiting
c)
C is limiting
d)
None are limiting
56.
1 Body + 4 Tires --> 1 car
How many cars can you make with 92 tires and 34 bodies?
a)
23
b)
34
c)
68
d)
46
57.
1 Cheese + 2 Bread --> 1 grilled cheese
How many grilled cheeses can you make with 26 slices of bread and 14 pieces of cheese?
a)
14
b)
13
c)
26
d)
12
58.
Fe + S --> FeS
How many moles of FeS are formed from 2 moles of Fe reacted with excess S?
a)
1 mole
b)
3 moles
c)
2 moles
d)
4 moles
59.
If 15 grams of copper (II) chloride react with 20 grams of sodium nitrate, how much sodium chloride can be formed?
a)
13.04 g
b)
130.4 moles
c)
130.4 g
d)
13.04 moles
60.
How many grams of ammonia (NH3) can be produced from the reaction of 28 g of nitrogen gas and 25 grams of hydrogen gas?
a)
43 g
b)
34 moles
c)
25 grams
d)
34 grams
61.
Silver nitrate and sodium phosphate are reacted in equal amounts of 200 g each. How many grams of silver phosphate are produced?
3AgNO3 + Na3(PO4) ---> Ag3(PO4) + 3NaNO3
3AgNO3 + Na3(PO4) ---> Ag3(PO4) + 3NaNO3
a)
164 g
b)
64 g
c)
146 g
d)
164 moles
62.
Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.
Mg + 2HCl --> MgCl2 + H2
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
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