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Honors: Stoichiometry

Total questions: 67

Worksheet time: 4hrs 44mins

Name
Class
Date
1.

How many grams are there in 4 moles of H2O?

a)

64

b)

38

c)

72

2.

How many moles are there in 51 grams of NH3?

a)

1 mole

b)

2 moles

c)

3 moles

3.

How many grams are there in 2 moles of NH3?

a)

17 grams

b)

28 grams

c)

34 grams

d)

51 grams

4.

Fluorine is diatomic. What is the molar mass of Fluorine gas?

a)

19.0 g/mol

b)

9 g/mol

c)

38.0 g/mol

d)

18.0 g/mol

5.

What is the mass of 4.5moles of CH4?

a)

72.0 g

b)

68 g

c)

72.0 mol

d)

0.3 mol

6.

How many moles are in 150 grams of Na2SO4?

a)

142.1 g/mol

b)

1.1 mol

c)

21 315 g

d)

21 315 mol

7.
If I need 20.4 moles of sodium chloride, how much should I weigh out?
a)
0.549 g
b)
112 g
c)
1192 g
d)
5077 g
8.
Which is heaviest - a mole of copper or a mole of lithium?
a)
mole of copper
b)
mole of lithium
c)
they have the same mass
9.
A scientist shows you a 2.25-mol sample of carbon and a 2.25-mol sample of selenium.  Which of the following is true?
a)
they have the same mass
b)
they have the same volume
c)
they have the name number of atoms
d)
they have the same density
10.
How many atoms are there in 3.2 grams of sulfur?
a)
6.022 x 1023 atoms S
b)
6.022 x 1022 atoms S
c)
0.031 atoms S
d)
1.66 x 10-24 atoms S
11.
A weather balloon containing helium gas is 1000 grams. How many atoms of He are in the balloon?
a)
4 atoms
b)
250 atoms
c)
1.5 x 1026 atoms
12.

How many grams are in 1.204 x 1024 molecules of H2O? (molar mass = 18g/mol)

a)

36 g

b)

18 g

c)

9 g

d)

54 g

13.

How many grams are in 3.01 x 1023 atoms of Kr? (molar mass = 84 g/mol)

a)

42 g

b)

84 g

c)

168 g

d)

200 g

14.
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. 
15.
N2 +  3H2 → 2NH3 
What is the mole ratio between Nitrogen and Ammonium in the above reaction?
a)
1 moles NH3 / 2 moles N2 
b)
2 moles NH3 / 1 moles N2 
c)
2 moles N2 / 3 moles NH3 
d)
1 moles N2 / 3 moles NH3 
16.
4NH3 + 5O2-->4NO + 6H2O
What is the total number of moles of H2O produced when 12 mole of NH3 is completely consumed?
a)
15
b)
18
c)
20
d)
24
17.
H2+Cl2-->2HCl
How many moles of Cl2 are needed to react with 3 moles of H2?
a)
5
b)
2
c)
3
d)
6
18.
Which of the following represent a mole ratio between silver nitrate and copper(II) nitrate in the following reaction:
2AgNO3 + Cu --> Cu(NO3)2 + 2Ag
a)
2 mol AgNO3 / 2 mol Ag
b)
2 mol Ag / 2 mol AgNO3 
c)
2 mol AgNO3 / 2 mol Cu(NO3)2
d)
2 mol AgNO3 / 1 mol Cu(NO3)2
19.

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

New problem: If 16 moles of carbon dioxide are formed by this reaction, how many moles of water were also produced?

a)

4 mol H2O

b)

6 mol H2O

c)

24 mol H2O

d)

96 mol H2O

e)

384 mol H2O

20.
What is the mass of 0.89 mol of CaCl2?
a)
111 grams
b)
0.008 grams
c)
98.9 grams
d)
none of the choices
21.

What is the percent composition by mass of magnesium in the compound MgSO4

a)

20%

b)

27%

c)

46%

d)

53%

22.
What is the empirical formula for the following molecular formula: C6H14
a)
C6H14
b)
C3H7
c)
CH2
d)
CH3
23.
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
24.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
25.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
26.
A chemical formula that shows the actual # and kinds of atoms present in one molecule of a compound is called_________
a)
ionic formula
b)
covalent formula
c)
empirical formula
d)
molecular formula
27.

Find the percent composition of Cu and S in the compound Cu2S.

a)
%Cu= 67.987 %S= 32.013
b)
%Cu= 79.854   %S= 20.145
c)
%Cu= 35.946   %S= 64.054
28.

Phosphorus combines with oxygen to form an oxide that reacts with water to produce phosphoric acid, which is an important industrial compound used to produce fertilizers. A balanced equation for the production of phosphoric acid is shown here:

P4O10(s) + 6H2O(L) → 4H3PO4(aq) + energy

Write the empirical formula of the solid reactant in the equation.



(a)  

29.

Phosphorus combines with oxygen to form an oxide that reacts with water to produce phosphoric acid, which is an important industrial compound used to produce fertilizers. A balanced equation for the production of phosphoric acid is shown here:

P4O10(s) + 6H2O(L) → 4H3PO4(aq) + energy

Show a numerical setup for calculating the percent composition by mass of phosphorus in P4O10 (formula mass is 283.89 u).

(a)  

30.

Given the balanced equation for the reaction of butane and oxygen:

2C4H10 + 13O2 → 8CO2 + 10H2O + energy

How many moles of carbon dioxide are produced when 5.0 moles of butane react completely?

a)

5.0 mol

b)

20.0 mol

c)

10.0 mol

d)

40.0 mol

31.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
32.

How many atoms are present in a 13.5 gram sample of beryllium?

a)

1.5 particles

b)

9 particles

c)

4.03 x1023 particles

d)

9.02 x1023 particles

33.
Name the following ionic compound: MgSO4*7H2O
a)
magnesium sulfate * hexahydarte
b)
magnesium sulfate hexahydarte
c)
magnesium sulfate heptahydrate
d)
magnesium sulfate* heptahydrate
34.
Na2CO3 · 10H2O is known as sodium sulfate ______
a)
Hydroxide
b)
Hydrate
c)
Decahydrate
d)
None of the above
35.
A 15.67 g sample of a hydrate of magnesium carbonate was heated to drive off the water. The mass was reduced to 7.58 g. What is the formula of the hydrate?
a)
MgCO3 · 5H2O
b)
MgCO3 · 4H2O
c)
MgCO3 · 6H2O
d)
MgCO3 · 1H2O
36.
A compound is a hydrate when it...
a)
is composed of only hydrogen and oxygen
b)
is a state of water
c)
traps water inside of the compound
d)
repels water from the compound
37.
An empirical formula:
a)
is a formula that calculates the coefficients of a compound in a balanced equation.
b)
is the simplest whole-number ratio of moles of elements in the compound.
38.

A 4.175 gram sample of a certain hydrate of copper (II) sulfate, CuSO4•xH2O, is heated until all the water is driven off. The resulting anhydrous compound weighs 3.120 grams. What is the formula of the hydrate?

a)

CuSO4•H2O

b)

CuSO4•3H2O

c)

CuSO4•6H2O

d)

CuSO4•4H2O

39.

A sample with a molar mass of 34.00 g/mol is found to consist of 0.44 g H and 6.92 g O. Find its molecular formula.

a)

HO

b)

H2O2

c)

H2O

d)

H1/2O1/2

40.

What type of reaction is Fe + Cl2 → FeCl3

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

41.

What type of reaction is C2H2 + O2 → CO2 + H2O

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

42.

What type of reaction is BF3 + Li2SO3 → B2(SO3)3 + LiF

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

43.

What type of reaction is Ag2O → Ag + O2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

44.

What type of reaction is Zn + HCl → H2 + ZnCl2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

45.

What type of reaction is H2 + N2 → NH3

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

46.

What type of reaction is KClO3 → KCl + O2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

47.
At the end of chemical reactions, what is the total mass of the reactants compared to the total mass of the products?
a)
the product is doubled
b)
the product is half the mass of the reactants
c)
the mass is the same
d)
the mass changes depending on the reaction
48.
In chemical reactions, what does the principle of conservation of mass mean?
a)
Matter is not created or destroyed.
b)
The total mass of the reactants is greater than the total mass of the products.
c)
The total mass of the reactants is less than the total mass of the products.
d)
Matter is not changed.
49.
The substances at the beginning of a chemical equation are called the ____
a)
product
b)
yield
c)
chemical symbol
d)
reactants
50.

What is the right part of a chemical equation called...

H2 + O2 --> H2O

a)

Reactants

b)

Products

c)

Yields

d)

Chemical Equation

51.

What is the arrow in a chemical equation...

H2 + O2 --> H2O

a)

Reactants

b)

Products

c)

Yields

d)

Chemical Equation

52.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__Al + __O2--> __Al2O3
a)
4,1 --> 2
b)
4,3 --> 4
c)
3,4 --> 1
d)
4,3 --> 2
53.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__H2SO3 + __KOH--> __H2O+ __K2SO3
a)
2,1 --> 2,1
b)
1,2 --> 1,1
c)
1,2 --> 1,2
d)
1,2 --> 2,1
54.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__H2 + __S --> __H2S
a)
1,1 --> 1
b)
2,2 --> 2
c)
1,2 --> 1
d)
1,2 --> 2
55.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__AgNO3 + __H2S --> __Ag2S+ __HNO3
a)
2,1 --> 1,2
b)
1,2 --> 1,1
c)
1,2 --> 1,2
d)
1,2 --> 2,1
56.

When balancing a chemical equation, you can only change _________, you can never change _______!

a)

coefficients, subscripts

b)

subscripts, coefficients

c)

formulas, subscripts

d)

coefficients, formula units

57.
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
58.
What is the measured amount of a product obtained from a chemical reaction?
a)
mole ratio
b)
theoretical yield
c)
percentage yield
d)
actual yield
59.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
60.
What is the first thing you must do to solve a stoichiometry problem?
a)
Write a Balanced Equation
b)
Panic
c)
Write an Unbalanced Equation
d)
Ask for help
61.
What is the empirical formula if you have 36.84% nitrogen and 63.16% oxygen?
a)
NO
b)
N2O3
c)
N2O4
d)
N2O5
62.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements. (keep two decimal places throughout calculations)
a)
SO
b)
SO2
c)
SO3
d)
SO4
63.
What is the empirical formula for the following:
32.40% sodium, 22.5% sulfur; 45.1 % oxygen, 37.75% water?
a)
Na2SO4H6O3
b)
Na2SO4 . 2H2O
c)
Na2SO4 . 3H2O
d)
Na2SO4 . (H2O)3
64.
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
65.
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
66.

Epinephrine (adrenaline) is a hormone secreted into the bloodstream in times of stress. It contains 59.0% C, 7.15% H, 26.20%O, 7.65%N and has a molar mass of 183 g/mol. What is its molecular formula?

a)

C9H13NO3

b)

C5H11N3O2

c)

C8H12NO2

d)

C7H9N2O

67.
Glycerol has a molar mass of 92.09g/mol. Its percent composition is: 39.12% C, 8.75% H, and 51.12% O. What is the molecular formula for glycerol?
a)
C2H3O2
b)
CH2O
c)
C2H4O2
d)
C3H8O3

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