wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Chemical Equations and the Mole (Ch. 10, 11)

Total questions: 159

Worksheet time: 1hrs 6mins

Name
Class
Date
1.

Determine the number of atoms of each element that appears on each side of the equation: 2Al + 6HCl → 3AlCl₃ + 3H₂. The number of atoms of Al on the left side is _____, and on the right side is _____.

(a)  

2.

Determine the number of atoms of each element that appears on each side of the equation: Ba(ClO₃)₂ → BaCl₂ + 2O₂

a)

Ba: 1, Cl: 2, O: 6 on both sides

b)

Ba: 1, Cl: 2, O: 3 on both sides

c)

Ba: 1, Cl: 1, O: 6 on both sides

d)

Ba: 2, Cl: 2, O: 6 on both sides

3.

Balance the following equation: ___SiCl₄(l) + ___H₂O(l) → ___SiO₂(s) + ___HCl(aq)

a)

SiCl₄(l) + 2H₂O(l) → SiO₂(s) + 4HCl(aq)

b)

SiCl₄(l) + H₂O(l) → SiO₂(s) + HCl(aq)

c)

2SiCl₄(l) + 4H₂O(l) → 2SiO₂(s) + 8HCl(aq)

d)

SiCl₄(l) + 4H₂O(l) → SiO₂(s) + 2HCl(aq)

4.

Balance the following equation: ___Au₂S₃ + ___H₂ → ___Au + ___H₂S

a)

1, 3, 2, 3

b)

2, 6, 4, 6

c)

1, 2, 2, 3

d)

2, 3, 4, 6

5.

Solid barium and oxygen gas react to produce:

a)

solid barium oxide

b)

liquid barium oxide

c)

gaseous barium oxide

d)

barium hydroxide

6.

Liquid bromine reacts with solid phosphorus (P₄) to produce:

a)

solid diphosphorus pentabromide

b)

liquid diphosphorus pentabromide

c)

gaseous diphosphorus pentabromide

d)

aqueous diphosphorus pentabromide

7.

Gaseous hydrogen chloride reacts with gaseous ammonia to produce:

a)

Solid ammonium chloride

b)

Liquid ammonium chloride

c)

Gaseous ammonium chloride

d)

Aqueous ammonium chloride

8.

Write the balanced chemical equation for the reaction in which sodium hydroxide and calcium bromide react to produce solid calcium hydroxide and sodium bromide. The reaction occurs in water.

a)

2 NaOH + CaBr2 → Ca(OH)2 + 2 NaBr

b)

NaOH + CaBr2 → Ca(OH)2 + NaBr

c)

2 NaOH + CaBr2 → Ca(OH)2 + NaBr2

d)

NaOH + CaBr2 → Ca(OH)2 + 2 NaBr

9.

2Mo(s) + 3O2(g) → 2MoO3(s) is an example of which type of reaction?

a)

Combustion

b)

Synthesis

c)

Decomposition

d)

Single displacement

10.

What is the product when dinitrogen tetrahydride (l) reacts with oxygen (g)?

a)

Nitrogen dioxide (g) and water (l)

b)

Ammonia (g) and water (l)

c)

Nitrogen monoxide (g) and hydrogen (g)

d)

Nitrogen (g) and water (l)

11.
AB + CD →AD + CB
a)
Double Replacement
b)
Single Replacement
c)
Synthesis
d)
Decomposition
12.

Identify this type of reaction, Cl2 + 2KI -->  I2 + 2KCl

a)

Synthesis

b)

Single replacement

c)

Double replacement

d)

Decomposition

13.
2 C5H5 + Fe --> Fe(C5H5)2 
a)

single replacement

b)

double replacement

c)

decomposition

d)

synthesis

14.
Which of the following is the general formula for a decomposition reaction?
a)
A + B  → AB
b)
AB → A + B
c)
AB + C → AC + B
d)
AB + CD → AC + BD
15.
Si + S8 --> Si2S4
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
16.
Ca + AlCl3 --> CaCl2 + Al
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
17.
Mg + N2 --> Mg3N2
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Combustion
18.
C3H8 + O2 --> H2O + CO2
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Combustion
19.

The reaction XY --> X + Y is an example of _____.

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

20.

The reaction AB + XY --> XB + AY is an example of ______.

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

21.

Which of the following is an example of a single replacement reaction?

a)

2NaF --> 2 Na + F2

b)

P2O5 + 3 H2O --> 2H3PO4

c)

2FeCl3 + 3Zn --> 2Fe + 3ZnCl2

d)

C6H12O6 + 6O2 --> 6CO2 + 6 H2O

22.

Which of the following is an example of a decomposition reaction?

a)

2NaF --> 2 Na + F2

b)

P2O5 + 3 H2O --> 2H3PO4

c)

2FeCl3 + 3Zn --> 2Fe + 3ZnCl2

d)

C6H12O6 + 6O2 --> 6CO2 + 6 H2O

23.

Which of the following chemical equations is an example of a double replacement reaction?

a)

2Al2O3 --> 4Al + 3O2

b)

2C5H10 + 15O2 --> 10CO2 + 10H2O

c)

2MgCl2 + Na2CO3 --> 2 NaCl + MgCO3

d)

K2O + H2O --> 2 KOH

24.

Which of the following chemical equations is an example of a combustion reaction?

a)

2Al2O3 --> 4Al + 3O2

b)

2C5H10 + 15O2 --> 10CO2 + 10H2O

c)

2MgCl2 + Na2CO3 --> 2 NaCl + MgCO3

d)

K2O + H2O --> 2 KOH

25.

What class of reaction best describes the equation below:

2HgClO3 ----> 2HgO + Cl2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

26.
What is it about the water molecule that makes it a great solvent?
a)
water demonstrates polarity; a partial charge on each side of the molecule
b)
due to its molecular formula
c)
it has a liner molecular shape
d)
due to it's non-polar molecular structure
27.

Define: Net Ionic Equation

a)

a balanced chemical equation in which all the reactants and products are given by their chemical formula.

b)

a chemical equation that shows all soluble species broken into their respective ions.

c)

a chemical equation showing only the species which are actively involved in the reaction.

28.

Write the chemical equation that represents the dissociation of the ionic compound Na2(SO4) .

a)

Na+2 + (SO4)-1

b)

2 Na+1 + (SO4)-1

c)

Na+2 + (SO4)-4

d)

2 Na+1 + (SO4)-2

29.

Which of the following shows the correct disassociation of the reaction for BaCl2?

a)

Ba 2+ (aq) + Cl2 - (aq) → BaCl2 (s)

b)

Ba 2+ (aq) + 2 Cl - (aq) →BaCl2 (s)

c)

BaCl2 (aq) →Ba 2+ (aq) + 2 Cl - (aq)

d)

BaCl2(s)→Ba 2+(aq)+ 2Cl- (aq)

30.

What 2 ions appear on both sides of the equation?

Na+ (aq) + Cl- (aq) + Ag + (aq) + (NO3)+ (aq) → Na+ (aq) + (NO3) + AgCl(s)

a)

Ag and NO3

b)

Na and Cl

c)

Na and NO3

d)

Ag and Cl

31.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
32.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
33.

Identify the complete ionic reaction for products of this reaction: (final answer is not balanced)

HCl + Mg(OH)2 →

a)

→ MgCl2 + H2O(l)

b)

→ Mg2+ + Cl-1 + H2O(l)

c)

→ Mg2+ + Cl-1 + H+1 + O2-

d)

→ MgCl2 + H2O(l) + CO2(g)

34.

A balanced chemical equation is a direct presentation of which law?

a)

law of multiple proportions

b)

law of conservation of mass

c)

ideal gas law

d)

law of conservation of momentum

35.

In a chemical equation, the number written in front of the chemical formula is called the _________.

a)

equation

b)

product

c)

coefficient

d)

reactant

36.

Considering the following precipitation reaction:

Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq)

What is the correct complete ionic equation?

a)

Pb2+ + (NO3)2- + 2K+ + 2I- → PbI2(s) + 2K+ + 2NO3-

b)

Pb2+ + 2NO3- +2K+ + I- → PbI2(s) + 2K+ + NO3-

c)

Pb2+ + 2NO3- + 2K+ + 2I- → PbI2(s) + 2K+ + 2NO3-

d)

Pb2+ + 2NO3- + 2K+ + 2I- → Pb2+ + 2I- + 2K+ + 2NO3-

37.

When some ionic compounds form through reactions in solution, they fall out as a ___

a)

consolidated element

b)

heavy sludge

c)

dense discharge

d)

solid precipitate

38.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
39.

In writing the chemical equation for a reaction that produces a precipitate, what abbreviation of the physical state must appear with one of the products?

a)

(s)

b)

(g)

c)

(l)

d)

(w)

40.

Considering the following precipitation reaction:

Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq)

Which compound would not form ions in the complete ionic equation?

a)

PbI2

b)

KNO3

c)

Pb(NO3)2

d)

KI

41.

Considering the following precipitation reaction:

Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq)

What is the correct complete ionic equation?

a)

Pb2+ + (NO3)2- + 2K+ + 2I- → PbI2(s) + 2K+ + 2NO3-

b)

Pb2+ + 2NO3- +2K+ + I- → PbI2(s) + 2K+ + NO3-

c)

Pb2+ + 2NO3- + 2K+ + 2I- → PbI2(s) + 2K+ + 2NO3-

d)

Pb2+ + 2NO3- + 2K+ + 2I- → Pb2+ + 2I- + 2K+ + 2NO3-

42-51.

Answer the questions below after watching the video

42.

What are net ionic equations primarily used to represent?

a)

The theoretical yield of a chemical reaction

b)

The actual species involved in a chemical reaction

c)

The role of spectator ions in a reaction

d)

The complete molecular structure of compounds

43.

What happens to sodium chloride (NaCl) when it is dissolved in water?

a)

It changes into a different compound

b)

It forms Na+ and Cl- ions

c)

It remains undissolved as a solid

d)

It reacts immediately to form a gas

44.

What does the term 'aqueous' signify in a chemical equation?

a)

The substance is a pure solid

b)

The substance is dissolved in water

c)

The substance is in a plasma state

d)

The substance is in a gaseous state

45.

Which compound is formed as a precipitate in the reaction between silver nitrate and sodium chloride?

a)

Sodium Nitrate (NaNO3)

b)

Silver Nitrate (AgNO3)

c)

Silver Chloride (AgCl)

d)

Sodium Chloride (NaCl)

46.

Which ions are involved in forming the precipitate in the discussed reaction?

a)

Na+ and Cl-

b)

Ag+ and Cl-

c)

Na+ and NO3-

d)

Ag+ and NO3-

47.

What state does Silver Chloride (AgCl) assume in the reaction?

a)

Aqueous

b)

Gas

c)

Plasma

d)

Solid

48.

Why is it important to understand the solubility of compounds when writing net ionic equations?

a)

To determine which compounds form precipitates

b)

To predict the color change in the reaction

c)

To calculate the pH of the solution

d)

To measure the conductivity of the solution

49.

What is the role of spectator ions in a net ionic equation?

a)

They react to form new compounds

b)

They remain unchanged and do not participate in the reaction

c)

They increase the rate of the reaction

d)

They decrease the solubility of compounds

50.

In the reaction, which compound remains dissolved and does not form a precipitate?

a)

Silver Chloride (AgCl)

b)

Sodium Nitrate (NaNO3)

c)

Sodium Chloride (NaCl)

d)

Silver Nitrate (AgNO3)

51.

What is the purpose of writing a total ionic equation?

a)

To calculate the amount of energy released

b)

To predict the products of the reaction

c)

To display all ions, indicating which are spectators

d)

To show only the ions that participate in the reaction

52.

Magnesium can be burned in oxygen to produce solid magnesium oxide.

a)

Mg + O2→ MgO

b)

Mg+ O→ MgO

c)

Mg + CO2 → MgO + C

d)

Mg + O2→ Mg2O2

53.

Sodium reacts with chlorine gas to produce sodium chloride.

a)

NaCl→ Cl + Na

b)

Na+ CO2 → NaCO2

c)

Na + Cl2→ NaCl

d)

Na + Cl → NaCl

54.

Magnesium + ________ --> magnesium oxide


What is missing?

a)

Hydrogen

b)

Sulphur

c)

Oxygen

d)

Oxide

55.

Identify the product(s) in this word equation

a)

Sodium

b)

Sodium chloride

c)

Sodium and Chlorine

d)

Sodium and sodium chloride

56.

The new substances formed in a chemical reaction are called

a)

Reactants

b)

Atoms

c)

Products

d)

Reagents

57.

In this chemical reaction zinc is a...

a)

Product

b)

Reactant

c)

Neither

58.

What does the symbol inside the circle mean?

a)

"yields, or produces"

b)

"dissolved in water"

c)

"forms a precipitate"

d)

"released as a gas"

59.

Which of the following statements is TRUE?

a)

A molecule is smaller than an atom.

b)

A molecule is made of atoms.

c)

Molecules are found inside of atoms.

60.

Which of the following symbols represents a compound?

a)

Co

b)

Br

c)

Fe

d)

CO

61.

What does the symbol CaCO3 represent?

a)

An element

b)

A compound

c)

An atom

d)

None of the above

62.

Which of these is NOT the correct way to read the symbol in a chemical equation?

a)

(g) = grams

b)

(aq) = solution

c)

(s) = solid

d)

(l) = liquid

63.

Which of the following chemical equations is correct for the word equation:

Solid magnesium is burned in oxygen gas to produce solid magnesium oxide.

a)

Mg + O2→ MgO (aq)

b)

Mg+ O→ MgO (s)

c)

Mg + CO2 → MgO (s) + C

d)

Mg + O2→ MgO (s)

64.
How many Hydrogen (H) atoms are in NH3O5
a)
3
b)
4
c)
5
d)
1
65.
How many hydrogens are in 4H2O?
a)
6
b)
8
c)
2
d)
4
66.
What are the coefficient used to balance the equation below?
__Ag2O →__ Ag +___O2
a)
2,4,1
b)
1,1,1
c)
2,1,2
d)
2,2,2
67.
Which problem is balanced?
a)
PbO2 + 2H2--> H2SO4
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
d)
2Na + 2H2O --> 2NaOH + H
68.
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
69.

Identify the correct equation (may not be balanced) for the following word equation: Iron reacts with solid sulfur to produce iron (II) sulfide powder.

a)

Fe + S → Fe2S

b)

Fe + S → FeS

c)

Fe2 + S→ Fe2S2

d)

Fe + S2 → Fe2S

70.

Identify the correct equation (may not be balanced) for the following word equation: sodium phosphate and calcium chloride produce calcium phosphate and sodium chloride

a)

Na3PO4 + CaCl2 --> Ca3(PO4)2 + NaCl

b)

Na3PO4 + CaCl2 --> Ca4PO2 + NaCl

c)

NaPO4 + CaCl2 --> Ca(PO4)2 + NaCl

d)

NaPO4 + CaCl2 --> Ca2(PO4)3 + NaCl

71.

Potassium iodide + lead nitrate --> _____________ + lead iodide


What is missing?

a)

lead nitrate

b)

potassium nitrate

c)

nitrogen

d)

potassium iodide

72.

When lead reacts with oxygen, a yellow lead(II) oxide powder is produced.

a)

Pb + O2 → PbO

b)

Pb + O2→ PbO2

c)

Pb2 + O2→ Pb2O

d)

Pb + O → PbO

73.

When hydrogen reacts with sulfur, a smelly gas, dihydrogen monosulfide, is produced.

a)

H2 + S → HS

b)

H2 + S → H2S

c)

H + S→ HS

d)

H + S→ H2S

74.

Hydrogen gas and nitrogen monoxide gas forms water and nitrogen gas.

a)

H2 + NO --> H2O + N2

b)

H + NO --> H2O + N

c)

H2 + N2O3 --> H2O + N2

d)

H + NO --> H2O + N2

75.

Barium metal and water yields barium hydroxide and hydrogen gas

a)

Ba + H2O --> Ba(OH)2 + H2

b)

Ba2 + H2O --> Ba(OH)2 + H

c)

Ba + H2O --> BaOH2 + H

d)

Ba2 --> Ba(OH)2 + H2

76.

Calcium oxide and water produces calcium hydroxide

a)

CaO + H2O --> Ca(OH)2

b)

Ca2O2 + H2O --> Ca(OH)2

c)

CaO + H2O --> CaOH

d)

Ca2O2 + H2O --> Ca(OH)2

77.

Aluminum and oxygen produces aluminum oxide

a)

Al + O2 --> Al2O3

b)

Al + O --> Al2O3

c)

Al3 + O2 --> Al2O3

d)

Al + O --> AlO

78.

1. The Best Friend's Club uses "invisible ink" to write notes to each other. The invisible ink is actually lemon juice that is clear when it dries on paper, but turns brown when a club member holds a burning candle under the paper. Once it is heated, it is never invisible again.

What type of change is occurring when the paper is heated?

a)

Chemical Change

b)

Physical Change

c)

Elemental Change

d)

Temperature Change

79.

A student mixes two clear liquids together. After a few minutes, a white powdery solid can be seen settling on the bottom of the test tube. Which of the following is a conclusion that the student can draw based on these observations? The two clear liquids-

a)

were pure substances before they were mixed

b)

are toxic and should be handled with extreme caution

c)

have gone through a chemical change in which a new substance called a precipitate was produced

d)

have been stored too long and are no longer good

80.

Shredding paper is an example of a

a)

chemical change

b)

physical change

c)

physical property

d)

chemical property

81.

A student added white crystals to a clear liquid. The crystals dissolved in the liquid. After a few seconds, the liquid became quite warm and then turned bright red in color. Indications that a chemical change was taking place could be observed when –

a)

the white crystals were added to the clear liquid.

b)

the crystals dissolved in the liquid leaving only the liquid visible

c)

There are no indications of chemical change

d)

the temperature of the liquid increased and an unexpected color change occurred.

82.

A student observes some sugar as it is heated and burns. The student concludes that a chemical reaction has occurred. Which of the following observations about the burning sugar provides evidence of a chemical reaction?

a)

Heat is added to the sugar crystals.

b)

The sugar melts and becomes a liquid.

c)

Gas is produced as the sugar turns black.

d)

No evidence of chemical reaction is present.

83.

The brown color of a cut apple can be called

a)

physical change

b)

chemical change

c)

evidence of chemical reaction

d)

all of the above

84.

Which results in a change of identity in matter?

a)

Physical

b)

Chemical

c)

Both

d)

Identity doesn't change

85.

Is rust on a car physical or chemical?

a)

Physical

b)

Chemical

c)

Both

d)

Neither

86.

What are examples of physical properties?

a)

Color

b)

Temperature

c)

Malleability

d)

Flammability

87.
Evidence of a chemical reactions is anything that shows - 
a)
a new substance has formed
b)
a solid dissolved in a liquid
c)
interaction between 2 gases
d)
a change in the state of matter
88.
Which of the following is NOT evidence that that a chemical reaction has occurred?
a)
produces light/heat
b)
production of a gas
c)
formation of a precipitate
d)
melting
89.

Which is not evidence that a chemical reaction has occured

a)

Production of flames

b)

Change in temperature or heat

c)

freezing

d)

Production of light

90.
A chemical reaction is...
a)
when a substance is mixed with another substance
b)
when a substance undergoes a change to form a new substance
c)
when a substance is dissolved into another substance
d)
when a substance is heated or exposed to another substance
91.
Which of the following is not evidence of a chemical reaction?
a)
Formation of a precipitate
b)
Production of gas
c)
Change in temperature
d)
Change in state of matter
92.

Which of the following does not exhibit a chemical change?

a)

a phase change

b)

productions of gas

c)

change in color

d)

all of the choices

93.

Dynamite explosion  

a)

Physical Change

b)

Chemical Change

94.

Melting of salt 

a)

Physical Change

b)

Chemical Change

95.

Physical change is a type of change in which a substance does not transform into another substance. 

a)

True

b)

False

96.

Chemical reaction is a process in which one or more substances are converted to one or more different substances with a new set of properties.

a)

True

b)

False

97.

Endothermic reaction is a formation of bubbles due to production of a gaseous substance. 

a)

True

b)

False

98.

Which is NOT an empirical formula?

a)

Al2(SO4)3

b)

C6H6

c)

C3H8O

d)

NH4Br

99.

How many moles of Cl are in 3 moles of CaCl2?

a)

1

b)

2

c)

3

d)

6

100.

How many moles of H are in one mole of the compound (NH4)3PO4?

a)

4

b)

3

c)

12

d)

7

101.

You have 19.7 grams of a material and wonder how many moles were formed. Your friend tells you to multiply the mass by grams/mole. Is your friend correct?

a)

Yes, you multiply mass by molar mass

b)

No, you divide mass by molar mass

c)

No, you multiply by Avogadro's number

d)

No, you divide by Avogadro's number

102.

What is the formula for calculating percent composition?

a)
b)
103.

What information do you need to calculate percent composition by mass?

a)

Temperature of the system in Kelvin

b)

Chemical formula or actual masses

c)

The abundance of each isotope

d)

Number of protons and electrons

104.

How many atoms are in 1 mole of Iodine (I)?

a)

6.022 x 1023

b)

4.022 x 1023

c)

6.022 x 1025

d)

4.022 x 1025

105.
What are the units for molar mass?
a)
grams
b)
amu
c)
grams/mole
d)
liters
106.

What is Avogadro's number?

a)

6.02 x 1023

b)

1 mole

c)

600 million

d)

6.02

107.

How do you find the molar mass for an element?

a)

Add the atomic masses of all the atoms in the compound.

b)

You convert into molar mass from a mass given to you

c)

You can only be given molar mass, it can't be calculated

108.

What is the Molar Mass of Platinum (Pt)?

a)

195.08 g/mol

b)

78 g/mol

c)

106.4 g/mol

d)

145 g/mol

109.

What is the difference in molar mass and formula weight?

a)

You get molar mass from the periodic table, but you get formula weight from Avogadro's number.

b)

Formula weight is the weight of 1 mole, while molar mass is the mass of only 1 particle

c)

There is no difference.

d)

Molar mass is the mass of 1 mole, while formula weight is the weight (mass) of only 1 particle

110.

What are the units of molar mass and of formula weight?

a)

molar mass: g/mol

formula weight: amu

b)

molar mass: amu

formula weight: g/mol

c)

g/mol for both

d)

amu for both

111.

What is the correct equation to determine how many calcium ions (Ca2+) in 2 moles?

a)
b)
c)
d)

This cannot be determined as calcium is not bonded.

112.

How many moles of Na contain 1.45 x 1021 atoms of Na?

a)

8.73 x 1044 moles

b)

8.73 moles

c)

0.00241 moles

d)

2.41 x 1044 moles

113.

What is the correct equation to calculate the number of moles in 3.13 x 1026 molecules of H2O2?

a)
b)
c)
d)
114.

How many moles are in 6.02 x 1023 molecules of H2O?

a)

1 mole

b)

2 moles

c)

6.02 moles

d)

602000000000000000000000 moles

115.

A mole is:

a)

The SI unit for mass

b)

The SI unit for the amount of a substance

c)

The SI unit for volume

d)

The SI unit for area

116.

Which has the most particles?

a)

1 mole H2

b)

1 mole Na1+

c)

1 mole Al(OH)3

d)

These are all the same

117.

Why is the mole used in chemistry?

a)

The mass of atoms is in AMUs which is too hard to convert to grams.

b)

A dozen is not a scientific amount.

c)

Chemists needed to make chemistry easier to understand.

d)

It makes counting large numbers of small particles easier.

118.

How is moles abbreviated?

a)

M

b)

m

c)

mol

d)

ml

119.
What is the mole used for? 
a)
To measure the amount of grams in a substance
b)
To measure the amount of atoms or molecules in a substance
c)
To measure the amount of energy in a substance
d)
To measure the amount of bonding in a substance 
120.
How many atoms are in 1 mole of NaCl? 
a)
6.02 x 1023
b)
58 
c)
11
d)
17
121.

The mole is 6.022 x 1023 atoms or molecules of any substance. This number is also named after the scientist who calculated it. This was:

a)

Perrin

b)

Avogadro

c)

Einstein

d)

Newton

122.

How many grams is one mole of Sodium?

a)

32.07

b)

118.71

c)

150.36

d)

22.99

123.

How many grams is 2 moles of Helium?

a)

4.00

b)

8.00

c)

2.02

d)

4.04

124.

Find the molecular weight of Vitamin A - C20H30O

a)

286.46 amu

b)

240.22 amu

c)

29.019 amu

d)

129.46 amu

125.

Find the molecular weight of carbon monoxide - CO

a)

16 amu

b)

12.011 amu

c)

28.011 amu

d)

29.019 amu

126.

What are the units used for Gram Formula Mass?

a)

amu

b)

grams

c)

mol

d)

g/mol

127.

Determine the gram formula mass of KCl

a)

74.548 amu

b)

35.45 amu

c)

74.548 g/mol

d)

35.45 g/mol

128.

When a question asks you to calculate mass, your units should be

a)

liters

b)

grams

c)

molecules

d)

atoms

129.

When a question asks you to calculate volume, your units should be

a)

liters

b)

grams

c)

molecules

d)

atoms

130.

When a question asks you to calculate atoms, your units should be

a)

liters

b)

grams

c)

molecules

d)

atoms

131.
A mole of Neon contains
6.02 x 1023 _____.
a)
atoms
b)
formula units
c)
ions
d)
molecules
132.

What is the difference between a formula unit and a molecule?

a)

formula unit - ionic compound

molecule - covalent/molecular compound

b)

formula unit - big

molecule - small

c)

formula unit - covalent/molecular compound

molecule - ionic compound

d)

formula unit - small

molecule - big

133.

When translating coefficients in a chemical reaction, "atoms" describes

a)

ionic compounds

b)

single elements

c)

molecular compounds

d)

diatomic molecules

134.

When translating coefficients in a chemical reaction, "formula units" describes

a)

ionic compounds

b)

single elements

c)

molecular compounds

d)

diatomic molecules

135.

When translating coefficients in a chemical reaction, "molecules" describes

a)

ionic compounds

b)

single elements

c)

molecular compounds

d)

diatomic molecules

136.

Name this compound: Br2

a)

dibromine

b)

bromine gas

c)

dibromide

d)

bromide gas

137.

Name this compound: Cl2

a)

dichlorine

b)

chlorine gas

c)

dichloride

d)

chloride gas

138.

Atoms, molecules, or formula units?

H2

a)

one formula unit of hydrogen gas

b)

one atom of hydrogen gas

c)

one molecule of hydrogen gas

139.

Atoms, molecules, or formula units?

2 CBr4

a)

two formula units of carbon tetrabromide

b)

two atoms of carbon tetrabromide

c)

two molecules of carbon tetrabromide

140.

Atoms, molecules, or formula units?

Br2

a)

one formula unit of bromine gas

b)

one atom of bromine gas

c)

one molecule of bromine gas

141.

Atoms, molecules, or formula units?

5 PF3

a)

five formula units of phosphorus trifluoride

b)

five atoms of phosphorus trifluoride

c)

five molecules of phosphorus trifluoride

142.

Atoms, molecules, or formula units?

3 PbI2

a)

three formula units of lead (II) iodide

b)

three atoms of lead (II) iodide

c)

three molecules of lead (II) iodide

143.

Atoms, molecules, or formula units?

6 NH4NO3

a)

six formula units of ammonium nitrate

b)

six atoms of ammonium nitrate

c)

six molecules of ammonium nitrate

144.

Atoms, molecules, or formula units?

4 Ca

a)

four formula units of calcium

b)

four atoms of calcium

c)

four molecules of calcium

145.

Atoms, molecules, or formula units?

8 P

a)

eight formula units of phosphorus

b)

eight atoms of phosphorus

c)

eight molecules of phosphorus

146.

Atoms, molecules, or formula units?

4 NaCl

a)

four formula units of sodium chloride

b)

four atoms of sodium chloride

c)

four molecules of sodium chloride

147.

Determine the amount of moles in CuBr that are in 276.9 g of the compound.

a)

3.2 mol

b)

1.7 mol

c)

2.1 mol

d)

1.9 mol

148.

Determine the number of moles of AlNO3 that are in 264 g of the compound.

a)

2.97 mol

b)

3.45 mol

c)

2.73 mol

d)

1.86 mol

149.

Find the mass of 3.8 mol of H2O. Round to the nearest tenth.

a)

57.9 g

b)

54.8 g

c)

68.4 g

d)

62.3 g

150.

Find the mass of 5.82 mol of MgCl2. Round to the nearest tenth.

a)

552.9 g

b)

436.8 g

c)

55.2 g

d)

554.1 g

151.

What is correct equation that should be used to determine how many molecules is 0.75 moles of (NH4)3PO4?

a)
b)
c)
d)
152.

What percentage of the total atomic mass of carbon monoxide (CO) is composed of carbon?

a)

29%

b)

43%

c)

57%

d)

73%

153.

What percentage of the total atomic mass of carbon monoxide (CO) is composed of oxygen?

a)

29%

b)

43%

c)

57%

d)

73%

154.

What percentage of the total atomic mass of magnesium bromide (MgBr2) is composed of bromine? Hint - consider the mass of both atoms of bromine in your calculation.

a)

13%

b)

43%

c)

63%

d)

87%

155.

What percentage of the total atomic mass of lithium phosphide (Li3P) is composed of phosphorus?

a)

13%

b)

29%

c)

40%

d)

60%

156.

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

157.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

158.
Which pair has the same empirical formula?
a)

NaCrO4 and Na2Cr2O7

b)

C2H4O2 and C6H12O6

c)

C3H6O3 and C2H6O2

d)

CH4 and C2H6

159.

How would you calculate the molar mass for C4H6?

a)

12.0111 + 1.00794

b)

4(12.0111) + 6(1.00794)

c)

2(12.0111) + 3(1.00794)

d)

6(12.0111) + 4(1.00794)

160.

The empirical formula of a substance is CH2O. The molar mass is 180g/mol. What is the molecular formula?

a)

CH2O

b)

C3H6O3

c)

C6H12O6

d)

C12H6O12

161.
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
162.
Name the following ionic compound: MgSO4*7H2O
a)
magnesium sulfate * hexahydarte
b)
magnesium sulfate hexahydarte
c)
magnesium sulfate heptahydrate
d)
magnesium sulfate* heptahydrate
163.
Name the following hydrate:  NaCl * 5H2O
a)
sodium chloride 
b)
sodium monochloride pentahydrate
c)
sodium chloride pentahydrate
d)
pentahydrate
164.
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
165.

What is the correct chemical formula for barium hydroxide octahydrate?

a)

Ba(OH)2 . 8H2O

b)

Ba(OH)2 . H2O

c)

8Ba(OH)2 . H2O

d)

Ba . 8(OH)2

166.

Find the percent composition of Cu2S?

a)

Cu= 67.987%; S= 32.013%

b)

Cu= 79.854%: S= 20.145%

c)

Cu= 35.946%; S= 64.054%

d)

Cu= 39.925%; S= 20.151%

167.

Select all empirical formulas

a)

C8H12

b)

C2H3

c)

CH3

d)

C4H10

e)

C2H5

168.
Name the following hydrate:  NaCl * 5H2O
a)
sodium chloride 
b)
sodium monochloride pentahydrate
c)
sodium chloride pentahydrate
d)
pentahydrate

Similar Resources on Wayground

1.2 Atomic Origins Part 1

168 questions

1.2 Atomic Origins Part 1

quiz

Worksheet

•

9th Grade

Spring 23-24 Practice Final Exam

174 questions

Spring 23-24 Practice Final Exam

quiz

Worksheet

•

9th - 12th Grade

PS - Final Exam Review (2019)

169 questions

PS - Final Exam Review (2019)

quiz

Worksheet

•

9th - 12th Grade

U3-MOCK EXAM COMPLETO

164 questions

U3-MOCK EXAM COMPLETO

quiz

Worksheet

•

9th Grade