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Chem Final Exam Review

Total questions: 150

Worksheet time: 6hrs 21mins

Name
Class
Date
1.

______ molecules are found in nature as pairs of two atoms of the same type covalently bonded together.

a)

Diatomic

b)

Monatomic

c)

Polyatomic

d)

Network

2.

Which of the following types of elements can exist in monatomic form?

a)

alkali metals

b)

transition metals

c)

halogens

d)

noble gases

3.
Why do bonds form?
a)
To fill the valence shell of electrons for the elements involved
b)
to release energy stored in the bonds
c)
because whenever you mix two chemicals, there will be a reaction
d)
because of attraction
4.
A substance which has a high melting point, conducts electricity when dissolved in water, and has a crystalline structure probably has what type of bond?
a)
Ionic
b)
Metallic
c)
Covalent
d)
Crystalline
5.
What type of bond is illustrated above?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Wiggly
6.

Bonds formed by transferring electrons from one atom to another are

a)

ionic

b)

metallic

c)

non polar covalent

d)

covalent

7.

Bonds formed by sharing electrons between atoms are

a)

ionic

b)

metallic

c)

covalent

d)

dipole-dipole

8.

A compound is made of two nonmetals. It is

a)

ionic

b)

metallic

c)

covalent

9.

A compound forms between a metal and a nonmetal. It is

a)

ionic

b)

metallic

c)

covalent

10.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
11.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
12.
What is the correct structure for BF3?
a)
Option A.
b)
Option B. 
c)
Option C.
d)
Option D.
13.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
14.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
15.

In HCN (Carbon is usually the central atom) what kind of bond is between the C and N

a)

Single

b)

Double

c)

Triple

16.

Why is this Lewis Structure incorrect? Choose all that apply.

a)

There are too many bonds around Si.

b)

There should only be single bonds in this Lewis Structure.

c)

The Structure is missing a triple bond.

d)

Chlorine only has 6 electrons surrounding it.

17.

SO3 is a ____ molecule.

a)

polar

b)

non-polar

18.

For polarity to occur in a bond, you need two elements with a difference in their electronegativities of ___

a)

0.5 or less

b)

between 0.5 and 1.6

c)

less than 1.6

d)

greater than 1.6

19.

CO2 has charge asymmetry, but is not a polar molecule because it's ___

a)

linear

b)

bent

c)

tetrahedral

d)

trigonal pyramidal

20.

Classify the following molecule.

a)

polar

b)

nonpolar

21.

Which of the following can be considered polar

a)

CO2

b)

H20

c)

CCl4

d)

H2

22.

What is the name of the three-dimensional pattern that forms when ions bond?

a)

a crystal lattice

b)

a chemical compound

c)

an ionic bond

d)

an ionic chalice

23.
Which of the following contains a polyatomic ion?
a)
Cu2CO3
b)
MnO
c)
CrN
d)
BeCl2
24.
What happens to the electrons in a Nonpolar Covalent bond
a)
transferred from one atom to another
b)
shared equally between 2 atoms
c)
shared unequally between 2 atoms
d)
mobile
25.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
26.
When Calcium forms a bond, what will occur? 
a)
Calcium with give away it two valence electrons to form an covalent bond. 
b)
Calcium will share its two valence electrons to form an covalent bond
c)
Calcium will give away its two valence electrons to form an ionic bond
d)
Calcium will share its two valence electrons to form an ionic bond. 
27.
How many Atoms are in FeO2. 
a)
3
b)
2
c)
1
d)
4
28.
Which of the below elements will most likely form an Ionic Bond? 
a)
P and O
b)
Cs and O
c)
Li and Mg
d)
Ne and Cl
29.

Formula for barium sulfide

a)

B2S3

b)

BaS

c)

Ba2S

d)

BaS2

30.

Name for Hg2S

a)

mercury (IV) sulfide

b)

mercury (III) sulfide

c)

mercury (II) sulfide

d)

mercury (I) sulfide

31.

Formula for lead (II) chloride

a)

PbCl2

b)

Pb2Cl

c)

Pb2Cl3

d)

Pb3Cl2

32.

Name for PBr2

a)

phosphorus bromide

b)

phosphorus dibromide

c)

phosphorus dibromine

d)

phosphorus bromine

33.

Formula for Disilicon Heptasulfide

a)

SiS6

b)

SiS7

c)

Si2S6

d)

Si2S7

34.

Name for LiOH

a)

lithium hydrogen oxide

b)

lithium hydroxide

c)

lithium (II) hydroxide

d)

lithium (I) hydroxide

35.

Formula for iron (II) carbonate

a)

FeCO3

b)

Fe2CO3

c)

FeCO2

d)

Fe2CO2

36.

Name for SrBr2

a)

strontium bromine

b)

strontium bromide

c)

strontium dibromide

d)

strontium dibromine

37.

Formula for Cobalt (II) bromide

a)

CoBr

b)

Co2Br2

c)

Co2Br

d)

CoBr2

38.

Formula for aluminum phosphate

a)

Al2P3

b)

Al3PO4

c)

AlP

d)

AlPO4

39.
What is the name of Al(NO3)3?
a)
Aluminum trinitrate
b)
Monoaluminum nitrate
c)
Aluminum (III) nitrate
d)
Aluminum Nitrate
40.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
41.
Name...Fe(NO3)3
a)
Iron nitrate
b)
Iron (III) Nitride
c)
Iron (I) nitrogen
d)
Iron (III) nitrate
42.
Provide formula:
Magnesium nitride
a)
MgN
b)
Mg3N2
c)
Mg(NO3)2
d)
Mg2N3
43.
Provide formula:
Potassium oxide
a)
KO2
b)
K2O
c)
KOH
d)
H2K
44.
Name...Pb(C2H3O2)4
a)
Lead acetate
b)
Lead (II) acetate
c)
Lead (III) acetate
d)
Lead (IV) acetate
45.
Name...P2Br9
a)
Phosphorus nonabromide
b)
Nonaphosphorus dibromide
c)
Diphosphorus nonabromide
d)
Diphosphorus bromide
46.
What is the formula for magnesium phosphide?
a)
Mg3P2
b)
Mg2P3
c)
Mg2PO3
d)
Mg3(PO3)2
47.

What is the formula for manganese (IV) sulfide?

a)

Mn4S2

b)

MnS2

c)

Mn2S4

d)

MnS

48.

According to VSEPR theory, atoms and unshared pairs orient themselves so that

a)

they are all in the same plane.

b)

they are at 90 degree angles.

c)

they are as close to each other as possible.

d)

they are as far apart as possible.

49.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
50.

Which of the following shapes has an unshared pair of electrons on the central atom?

a)

linear

b)

trigonal pyramidal

c)

trigonal planar

d)

tetrahedral

51.

Which molecule shape has three atoms bonded to the central atom and no unshared pairs on the central atom?

a)

tetrahedral

b)

trigonal pyramidal

c)

trigonal planar

d)

bent

52.

Draw the Lewis structure for CF4 and determine its molecular shape.

a)

trigonal planar

b)

trigonal pyramidal

c)

bent

d)

tetrahedral

53.

Which of the following molecular shape is bent?

a)

SCl2

b)

CO2

c)

PH3

d)

NCl3

54.

Choose the correct molecular shape for NH4+.

a)

trigonal planar

b)

trigonal pyramidal

c)

bent

d)

tetrahedral

55.

What is the molecular geometry of this molecule (look at the C)?

a)

Trigonal Planar

b)

Tetrahedral

c)

Linear

d)

T-Shaped

56.

What is the bond angle in a tetrahedral molecular geometry?

a)

90 degrees

b)

109.5 degrees

c)

120 degrees

d)

180 degrees

57.

What is the effect of lone pairs on molecular geometry?

a)

Lone pairs have no effect on molecular geometry.

b)

Lone pairs occupy space and can alter the angles between bonding pairs.

c)

Lone pairs increase the bond length between atoms.

d)

Lone pairs only affect the molecular weight.

58.

What is the VSEPR theory used to predict?

a)

Molecular Shape

b)

Chemical Bonding

c)

Reaction Rates

d)

Electronegativity

59.

What is the bond angle in a trigonal planar molecule?

a)

90 degrees

b)

120 degrees

c)

180 degrees

d)

109.5 degrees

60.

What is the empirical formula of a substance with the molecular formula C2H4?

a)

C2H2

b)

C2H2

c)

C1H1

d)

CH2

61.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
62.
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
63.

How many molecules are in 2.5 mol of NaCl?

a)

1.5 x 1024 molecules

b)

1.5 molecules

c)

4.15 molecules

d)

1.5 x 1023 molecules

64.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
65.
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
66.
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
67.

2.40 g of an explosive, J, contains 0.473 g of nitrogen. J also contains 33.8% carbon and 1.41% hydrogen by mass. The remainder of J is oxygen.


What is the empirical formula of J?

a)

C4HNO2

b)

CH2N2O

c)

C2HNO2

d)

CHNO

68.
What is the percentage of oxygen in carbon dioxide? (CO2)
a)
27.3%
b)
72.7%
c)
30%
d)
70%
69.
What is the percentage of chlorine in sodium chloride? (NaCl)
a)
60.7%
b)
39.3%
c)
60%
d)
40%
70.
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
71.

Calculate the percent water in strontium chloride hexahydrate

a)

6.76%

b)

59.45%

c)

68.21%

d)

40.55%

72.
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
73.
What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.
a)
K2SO4 
b)
K8SO16
c)
K8S4O8 
d)
K8S4O16 
74.

What is the oxidation number for Oxygen?

a)

+1

b)

+2

c)

-1

d)

-2

75.

What is the oxidation number for each Hydrogen in CH4?

a)

+1

b)

+2

c)

+3

d)

+4

76.

What is the oxidation state of Cu in Cu2+?

a)

-1

b)

-2

c)

+2

d)

0

77.

What is the oxidation state of H in H2?

a)

+2

b)

+1

c)

0

d)

None of the above

78.

What is the oxidation state of Pb in PbO ?

a)

+2

b)

+4

c)

0

d)

-2

79.
What is the oxidation number of Sn in SnO2?
a)
+1
b)
+4
c)
+2
d)
-2
80.

When balancing this equation, Fe + Cl2 → FeCl3, the correct coefficient for Cl2?

a)

1

b)

2

c)

3

d)

4

81.

What does this symbol Δ above the arrow mean?

a)

a precipitate is form

b)

heat is supplied

c)

a calalyst is needed

d)

electricity is needed

82.

Balance this equation, AlCl3 + NaOH → Al(OH)3 + NaCl

a)

3,1,3,1

b)

1,3,3,1

c)

1,1,1,3

d)

1,3,1,3

83.

Balance the following equation: Cr(s) + Fe(NO3)2 (ag) → Fe(s) + Cr(NO3)3 (ag)

a)

2,3,3,2

b)

2,3,2,3

c)

4,6,6,2

d)

1,3,3,1

84.

Chemical equations

a)

give directions for naming compounds

b)

describe only biological changes

c)

describe chemical reactions

d)

show how to write formulas

85.
Fill in the blanks with coefficient:
PCl5+_ H2O→_ HCl+H3PO4
a)
4, 5
b)
1, 6
c)
3, 8
d)
2,2
86.
How many atoms of aluminum are on each side of the following equation: 4Al + 3O2 --> 2Al2 O3
a)
2
b)
6
c)
1
d)
4
87.
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
88.
Balance the equation:
Si(OH)4+NaBr--> SiBr4+NaOH
a)
Si(OH)4+2NaBr--> SiBr4+NaOH
b)
Si(OH)4+4NaBr--> SiBr4+4NaOH
c)
Si(OH)4+NaBr--> SiBr4+4NaOH
d)
Si(OH)4+2NaBr--> SiBr4+2NaOH
89.

To balance a chemical equation, it may be necessary to adjust the

a)

formulas of the products

b)

subscripts

c)

coefficients

d)

number of products

90.

Which is the correct coefficient to balance this equation, NH4NO2 → N2 + H2O?

a)

1,1,2

b)

1,3,3

c)

3,2,1

d)

1,3,2

91.

What state of matter is this substance?

a)

solid

b)

liquid

c)

gas

d)

aqueous

92.

Which compound is formed as a solid precipitate in this reaction?

a)

Pb(NO3)2

b)

KI

c)

PbI2

d)

KNO3

93.

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"

94.
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.
95.
How many oxygen atoms are present in the following? 
4Ca(OH)2
a)
4
b)
6
c)
8
d)
1
96.

What happens in a chemical reaction?

a)

Bonds between atoms break and/or are formed

b)

New atoms are created and/or removed

c)

Protons move from one atom to another

d)

Electrons change into protons

97.
Which of the following symbols is not a correct indication of the phase of a substance in a reaction? 
a)
(s)=solid
b)
(g)=grams
c)
(l)=liquid
d)
(aq)= aqueous
98.
Which is NOT an indicator of a chemical change?
a)
temperature change
b)
formation of a precipitate
c)
shape change
d)
production of light
99.
When two substances were combined, bubbles were produced and the temperature dropped.  This most likely means that:
a)
a chemical reaction took place
b)
the two substances had low boiling points
c)
one substance dissolved in the other
d)
the two substances are non-reactive
100.

Copper(II) chloride and aluminum react to produce aluminum chloride and copper. Which of the following is the correctly balanced chemical equation for this reaction?

a)

CuCl2 + Al -> AlCl3 + Cu

b)

3CuCl2 + Al -> AlCl3 + 2Cu

c)

3CuCl2 + 2Al -> 2AlCl3 + 3Cu

d)

CuCl2 + 3Al -> AlCl3 + 2Cu

101.

Translate the following chemical equation into a sentence:

Mg (s) + 2HNO3 (aq) --> Mg(NO3)2 (aq) + H2 (g)

a)

Magnesium and hydrogen nitrate react to produce magnesium nitrate and hydrogen.

b)

Solid magnesium and nitric acid react to produce aqueous magnesium nitrate and hydrogen gas.

c)

Magnesium ribbon and aqueous hydrogen nitrate react to produce a magnesium nitrate precipitate and hydrogen grams.

d)

Smooth magnesium and aquaceous nitrate acid react to produce aquaceous magnesium nitrate reacts with hydrogen gas.

102.

Name this covalent compound: heptasulfur decaoxide

a)

S7O10

b)

S6O10

c)

S7O9

d)

S10O7

103.

Determine the reaction type: 4Si + S8 → 4SiS2

a)

Double displacement

b)

Single Displacement

c)

Synthesis

d)

Decomposition

104.

3Ca + 2AlCl3 → 3CaCl2 + 2Al

a)

Synthesis

b)

Single Displacement

c)

Double Displacement

d)

Decomposition

105.

C10H8 + 12O2 → 10CO2 + 4H2O

a)

Synthesis

b)

Double Displacement

c)

Decomposition

d)

Combustion

106.

CaCO3 → CaO + CO2

a)

Combustion

b)

Double Displacement

c)

Single Displacement

d)

Decomposition

107.
One element replaces another in a compound.
a)
Synthesis
b)
Combustion
c)
Single Replacement
d)
Double Replacement
108.
KOH + H3PO4 --> K3PO4 + H2O
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
109.

3 Pb + 2 H3PO4 ----> 3 H2 + 1 Pb3(PO4)2

a)

Synthesis (or combination)

b)

Decomposition

c)

Single replacement

d)

Double replacement

110.

Combustion reactions will always involve

a)

Oxygen and a solid

b)

Liquid nitrogen and heat

c)

Oxygen and heat/energy

d)

CO and H2O

111.

Classify the following chemical reaction


BaCl2(aq) + K2CrO4(aq) --> BaCrO4(s) + 2KCl(aq)




a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

112.

Identify the type of reaction...

Na2CO3 + heat −>Na_2CO_3\ +\ heat\ ->

a)

Composition

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

113.
Using the balanced equation in question 1,
Mg(s)   +   HCl(aq)  -->   MgCl₂(aq)   +   H₂(g)
How many grams of HCl are consumed by the reaction of 2.50 moles of magnesium?
a)
5.00 g
b)
7.29
c)
182 g
d)
218 g
114.
Using the balanced equation in question 1,
Mg(s)   +   HCl(aq)  -->   MgCl₂(aq)   +   H₂(g)
What is the mass in grams of H₂ gas when 4.0 moles of HCl is added to the reaction?
a)
0.99 g
b)
4.0 g
c)
2.0 g
d)
6.0 g
115.
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
116.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of Mg to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
117.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
118.
2NaClO3 (s) → 2NaCl (s) + 3O2 (g)  
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
119.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
120.
Fe2O3 + 3H2 → 2Fe + 3H2O
About how many grams of H2O will be produced from 150 grams of Fe2O3? 
a)
50 grams H2O
b)
60 grams H2O
c)
5000 grams H2O
d)
6000 grams H2O
121.
Use the following equation:
2NaOH(aq) + H2SO4(aq) --> 2H2O(l) + Na2SO4(aq)
How many grams of sodium sulfate will be formed if you start with 200 grams of sodium hydroxide?
a)
150.22 g Na2SO4
b)
593.44 g Na2SO4
c)
330.04 g Na2SO4
d)
297.65 g Na2SO4
122.

151 grams of Al2O3 are produced. How many grams of Al was needed in the reaction? Al + O2 -------> Al2O3 balance first.

a)

79.91 g

b)

22.4 liters

c)

57.8 g

d)

142.8 g

123.
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
124.

CH4 + 2O2 → CO2 + 2H2O

24 grams of CH4 was added to the above reaction. Calculate the theoretical yield of CO2.

a)

66 grams CO2

b)

132 grams CO2

c)

33 grams CO2

d)

8.72 grams CO2

125.

A student measures the pressure and volume of an empty water bottle to be 1.4 atm and 2.3 L. She then decreases the pressure to 0.65 atm. What is the new volume?

a)

2.1 L

b)

5.0 L

c)

8.2 L

d)

3.9 L

126.

What is the pressure of a car tire that had an initial pressure of 1.8 atm but was heated from 38°C to 123°C?

a)

0.9 atm

b)

2.1 atm

c)

1.6 atm

d)

3.4 atm

127.

Three gases are mixed together in a container with a total pressure of 4.8 atm. If two of the gases have pressures of 1.2 atm and 1.5 atm, what is the pressure of the third gas?

a)

2.5 atm

b)

1.8 atm

c)

2.1 atm

d)

1.3 atm

128.
Which of the following would increase the (gas) pressure of a system?
a)
Increase the Temperature
b)
Pump in more gas
c)
Decrease the volume
d)
All of these
129.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
130.

Determine the temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure.

a)

0 K

b)

107 K

c)

207 K

d)

307 K

131.

Pressure is

a)

defined as the mass that an object exerts when at rest.

b)

not a measurable in gases.

c)

defined as the number of moles of substance divided by the mass of the substance.

d)

created by the force of the gas particles impacting the walls of the container.

132.

A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC. What is the new volume of the gas?

a)

60.0 mL

b)

15.0 mL

c)

27.5 mL

d)

32.5 mL

133.

What is the pressure exerted by 5.00 moles of nitrogen gas contained in a 30.0 Liter container at 25.0 °C?

a)

3670 atm

b)

0.245 atm

c)

4.08 atm

d)

605 atm

134.
What is the limiting reactant if 10 moles of NH3  react  with 30.0 moles of NO?
4NH3+6NO --> 5N2 + 6H2O
a)
NH3
b)
NO
c)
N2
d)
water
135.
When 12 moles of O2 reacts with 1.1 mole of C10H8 what is the limiting reactant?  C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
136.
4NH3 + 5O2 --> 4NO + 6H2O
How many grams of NO are formed if 6.30g of ammonia react with 1.80g of oxygen? 
a)
0.37g
b)
0.045g
c)
1.35g
d)
11.1g
137.
How many grams of FeS are formed from 7.62g of Fe reacted with excess S?
a)
3.82g
b)
7.62g
c)
12.2g
d)
11.4g 
138.
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
139.

In the image, which reactant is limiting?

a)

The white molecules, because there are extra.

b)

The black atoms, because they are completely used up.

c)

The white molecules, because they are completely used up.

d)

The black atoms, because there are extra.

140.

Identify the limiting and excess reactants in the reaction shown.

a)

N2 is limiting and H2 is excess. 

b)

H2 is limiting and N2 is excess. 

c)

NH3 is both limiting and excess.

d)

There is no limiting reactant. 

141.

Why is it important to identify the limiting reagent?

a)

The limiting reagent speeds up the reaction.

b)

The limiting reagent controls the amount of product formed.

c)

If there is no limiting reagent, the reaction will not occur.

d)

No stoichiometry calculations can be done without a limiting reagent.

142.
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
a)
164 g
b)
64 g
c)
146 g
d)
164 moles
143.

A sample of silver contains 5.71 x 1022 atoms. How many moles of silver are present?

a)

3.43 x 1046 moles

b)

0.0529 moles

c)

0.0948 moles

d)

10.5 moles

144.

What is the total mass, in grams, of a 0.75 mole sample of SO2?

a)

16 g

b)

24 g

c)

32 g

d)

48 g

145.
Calculate the mass of iron in a sample of iron ore containing 2.61x1023 iron atoms.
a)
0.433g
b)
24.2g
c)
44g
d)
6.02g
146.
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
147.
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
148.
What is the mole ratio of H2O to H3PO4 in the following chemical equation?   P4O10 + 6 H2O --> 4 H3PO4 
a)
6:4
b)
4:6
c)
1:3
d)
3:1
149.

3CaCO3 + 2FePO4 --> Ca3(PO4)2 + Fe2(CO3)3


Assuming we start with 100. g of CaCO3 and 45 g of FePO4, identify the limiting reactant. (CaCO3 = 100.09 g/mol; FePO4 = 150.82 g/mol)

a)

iron(V) phosphate

b)

calcium carbonate

c)

iron(III) phosphate

d)

calcium(II) carbonate

150.

Which of the following describes an excess reactant?

a)

The reactant that is not completely consumed during a reaction

b)

None of this reactant is left over after the reaction take place

c)

The reactant that is completely consumed during the reaction

d)

Some of this reaction is left over after the reaction

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