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Worksheets

Spring Final Exam Review

Total questions: 172

Worksheet time: 5hrs 34mins

Name
Class
Date
1.
What is the molar mass of C6H12O6?
a)
180.18
b)
180.12
c)
180.24
d)
180.06
2.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
3.
2H2   +   O2  →  2H2O
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
4.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (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
5.
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
6.
2H2  +   O2  →  2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2
b)
4
c)
6
d)
8
7.
O2 + CS2 --> CO2 + SO2
What coefficient would go in front of the O2?
a)
1
b)
2
c)
3
d)
4
8.
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
9.
How many grams are in one mole of Oxygen
a)
16
b)
32
c)
15.99
d)
31.98
10.
What is the molar mass of Mg(NO3)2
a)
148.313g/mol
b)
134.306g/mol
c)
54.311g/mol
11.

How many grams are in 7.8 moles of NaCl?

a)

476grams

b)

460 grams

c)

452 grams

d)

462 grams

12.
How many grams are in 3.3 mol of Potassium Sulfide (K2S)?
a)
363 g
b)
454 g
c)
238 g
d)
132 g
13.

For the reaction 3Fe + 4H2O --> Fe3O4 + 4H2, how many moles of iron oxide are produced from 500 g of iron?

a)

1

b)

3

c)

9

d)

12

14.

For the reaction 2Na + 2H2O --> 2NaOH + H2, how many grams of hydrogen gas are produced if 120. g of sodium and 80. g of water react?

a)

4.5 g

b)

44 g

c)

80. g

d)

200. g

15.

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

16.

A scientist needs to store 28.0 moles of xenon gas at STP in the lab. What size gas tank will he need?

a)

628 L

b)

473 L

c)

219 L

d)

376 L

17.

A sample of gas containing 8.1 moles at STP would fill a container of what volume?

a)

342 L

b)

703 L

c)

475 L

d)

182 L

18.

A water bottle at STP is cooled to -155°C. What is the new pressure?

a)

3.2 atm

b)

0.43 atm

c)

1.8 atm

d)

0.27 atm

19.

A student inflates a balloon with helium then places it in the freezer. The student should expect

a)

the balloon's volume to increase

b)

the balloon's volume to decrease

c)

the balloon's moles to increase

d)

the balloon's moles to decrease

20.

The pressure of a 6.5 L sample of oxygen gas is measured to be 3.8 atm. If the gas is transferred into a 12 L tank, what is the new pressure?

a)

6.6 atm

b)

3.9 atm

c)

4.5 atm

d)

2.1 atm

21.

A student transfers a gas at STP from a 11.0 L tank to a 25.0 L tank. If the pressure remains constant, what is the new temperature?

a)

620 K

b)

393 K

c)

254 K

d)

530 K

22.

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

23.

A sample of gas containing 9.2 moles is transferred from an 13 L tank to a 23 L tank. What is the new number of moles that can be stored in the tank?

a)

10.2 mol

b)

13.7 mol

c)

19.1 mol

d)

16.3 mol

24.

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

25.

When a piston compresses in a chamber the volume of the gas inside decreases. What happens to the pressure and which gas law is this representing?

a)

The pressure decreases - Charles'

b)

The pressure increases - Charles'

c)

The pressure decreases - Boyle's

d)

The pressure increases - Boyle's

26.

What is the volume of a balloon that contains 3.7 moles of helium at 75°C and 5.1 atm?

a)

37 L

b)

13 L

c)

45 L

d)

21 L

27.

Avogadro's Law explains the relationship between

a)

Pressure and Volume

b)

Pressure and Temperature

c)

Volume and Temperature

d)

Volume and Moles

28.

A student places four gases into a container. The pressures of the gases are: N2=2.1 atm, H2=1.3 atm, He=1.9 atm & Ar=3.4 atm. What is the total pressure?

a)

5.1 atm

b)

8.7 atm

c)

7.4 atm

d)

6.9 atm

29.

If a hairspray can is heated, what can be expected of the pressure of the gas inside the can?

a)

The pressure will increase

b)

The pressure will decrease

c)

The pressure will remain constant

d)

The pressure will equalize

30.
How many moles are in 3.01 x 1022 atoms of magnesium?
a)
0.0500 moles
b)
1.81 x 1046 moles
c)
5.00 x 1021 moles
d)
5.00 moles
31.

A mole of potassium chloride, an ionic compound, contains 6.02 x 1023 _____.

a)

atoms

b)

formula units

c)

ions

d)

molecules

32.

How many molecules are in 2.00 moles of H2O?

a)

124x1024 molecules of H2O

b)

1.20x1023 molecules of H2O

c)

12.04 x1023 molecules H2O

d)

124

33.
How many atoms are in 1.50 moles of Hg?
a)
9.03x1023 atoms Hg
b)
9.03x1024 atoms Hg
c)
903 atoms of Hg
d)
9.03 atoms of Hg
34.

Which one has the most molecules or formula units?

a)

1 mole H2O

b)

1 mole Al(OH)3

c)

1 mole NaCl

d)

They are all the same

35.
Which has more molecules?
a)
1 mole CO2
b)
1 mole of N2O4
c)
1 mole of H2O
d)
They are all the same
36.

The sum of the percent by mass of each element in a compound must equal 100%.

a)

True

b)

False

37.

Which of the following sets of empirical formula, molar mass, and molecular formula is correct?

a)

CH, 78 g/mol, C13H13

b)

CH4N, 90 g/mol, C3H12N3

c)

CaO, 56 g/mol, Ca2O2

d)

C3H8O, 120 g/mol, C3H8O2

38.

The empirical formula for a compound is CH2O, and the molar mass is 180.2 g/mol. Which is the molecular formula for this compound?

a)

C6H12O6

b)

C7H16O5

c)

C8H20O4

d)

C3H6O3

39.

How many formula units are in 3.6 grams of NaCl?

a)

0.06

b)

1.0x1021

c)

1.3x1026

d)

3.7x1022

40.

Which is the correct empirical formula for this substance?

a)

CH4O

b)

CHO

c)

C3H12O3

d)

C3H4O

41.

Which substances have the same empirical formula?

a)

Samples 1, 2, and 4

b)

Samples 1 and 4

c)

Samples 1 and 3

d)

Samples 2 and 3

42.

The molecular formula for a compound is the formula with the smallest whole-number mole ratio of the elements.

a)

True

b)

False

43.

88.0 grams of CO2 is about _____________. [Select 2 answers.]

a)

1 mole of CO2

b)

2 moles of CO2

c)

6.02 x 1023 molecules of CO2

d)

two times 6.02 x 1023 molecules of CO2

44.

To find the percent by mass of a compound if you are given the formula, divide the molar mass of that element in one mole of the compound by the total molar mass of the compound.

a)

True

b)

False

45.

For the reaction 2Na + 2H2O --> 2NaOH + H2, how many grams of hydrogen gas are produced if 120. g of sodium and 80. g of water react?

a)

4.5 g

b)

44 g

c)

80. g

d)

200. g

46.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
47.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Linear
48.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
49.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
50.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
51.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
52.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
53.
Choose the correct shape for this molecule:
a)
Tetrahedral
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
54.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
55.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Trigonal planar
56.
A molecule consists of four bonds and no lone pairs. What is its structure? 
a)
square planar
b)
tetrahedral
c)
linear
d)
square pyramidal 
57.
SiCl4 has what shape?
a)
square planar
b)
square pyramidal
c)
tetrahedral
d)
octahedral
58.

A solid acid HX is mixed with water. Two possible solutions can be obtained. Which of the following is true?

a)

In case I, HX is acting like a weak acid, and in case II, HX is acting like a strong acid.

b)

In case I, HX is acting like a strong acid, and in case II, HX is acting like a weak acid.

c)

In both cases, HX is acting like a strong acid.

d)

In both cases, HX is acting like a weak acid.

59.

Which of the following is NOT a strong base?

a)

KOH

b)

Ca(OH)2

c)

LiOH

d)

Al(OH)3

60.

All of the following are weak acids except

a)

HCNO

b)

HBr

c)

HF

d)

HCN

61.

Which of the following is a strong acid?

a)

HF

b)

KOH

c)

HClO4

d)

HClO

62.

Aqueous solutions of sodium sulfide and copper(II) chloride are mixed together. Which statement is correct?

a)

Both NaCl and CuS precipitate from solution

b)

No reaction will occur

c)

CuS will precipitate from solution.

d)

NaCl will precipitate from solution.

63.

Aqueous solutions of potassium sulfate and ammonium nitrate are mixed together. Which statement is correct?

a)

Both KNO3 and (NH4)2SO4 precipitate from solution

b)

A gas is released.

c)

KNO3 will precipitate from solution

d)

No reaction will occur

64.

Which of the following salts is insoluble in water?

a)

Na2S

b)

K2CO3

c)

Pb(NO3)2

d)

All of these are soluble in water.

65.

Which of the following ions is most likely to form an insoluble sulfate?

a)

K1+

b)

Li1+

c)

S2-

d)

Ca2+

66.

Which pair of ions would not be expected to form a precipitate when dilute solutions of each are mixed?

a)

Al3+, S2–

b)

Pb2+, Cl–

c)

Mg2+, SO42–

d)

Ba2+, PO43–

67.

Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride and aqueous barium nitrate. The balanced molecular equation contains which one of the following terms?

a)

AgCl (s)

b)

2AgCl (s)

c)

2Ba(NO3)2 (aq)

d)

BaNO3 (aq)

68.

Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride and aqueous barium nitrate. The balanced complete ionic equation contains which of the following terms?

a)

2Ba2+(aq)

b)

Cl–(aq)

c)

2Ag+(aq)

d)

AgCl(aq)

69.

When sodium chloride and lead(II) nitrate react in an aqueous solution, which of the following terms will be present in the balanced molecular equation?

a)

PbCl(s)

b)

Pb2Cl(s)

c)

NaNO3(aq)

d)

2NaNO3(aq)

70.
KBr
a)
Soluble
b)
Insoluble
71.
Zinc Hydroxide
a)
Soluble 
b)
Insoluble
72.
Silver Iodide
a)
Soluble 
b)
Insoluble 
73.
KOH
a)
Soluble 
b)
Insoluble
74.
Zinc Carbonate
a)
Soluble 
b)
Insoluble 
75.
NiCl2
a)
Soluble 
b)
Insoluble
76.
PbI2
a)
Soluble
b)
Insoluble
77.
NaC2H3O2
a)
soluble
b)
insoluble
78.
K2CO3
a)
soluble
b)
insoluble
79.
FeS
a)
soluble
b)
insoluble
80.
K2SO4
a)
soluble
b)
insoluble
81.
AgCl
a)
soluble
b)
insoluble
82.
Which pairs, below, form a precipitate when mixed together?
a)
sodium chloride, lead(II) nitrate
b)
calcium nitrate, potassium iodide
c)
lithium phosphate, ammonium nitrate
d)
potassium chloride, barium nitrate
83.
A decomposition reaction is a reaction between at least two reactants in which
a)
one breaks down into at least two products.
b)
a compound is decomposed by an electric current.
c)
a compound burns in the presence of oxygen.
d)
a new, more complex compound is formed.
84.
A chemical equation is balanced by changing or adding
a)
chemical symbols.
b)
subscripts
c)
coefficients.
d)
reactants.
85.
A chemical reaction in which the energy is absorbed primarily in the form of heat is ______.
a)
flammable
b)
exothermic
c)
endothermic
d)
endergonic
86.
A substance that speeds up a chemical reaction without undergoing permanent change itself is a(n) 
a)
inhibitor
b)
coefficient
c)
reactant
d)
catalyst
87.
The breaking down of a substance into two or more substances is ______________.
a)
synthesis
b)
decomposition
c)
single-displacement
d)
double-displacement
88.
If energy in the form of heat is given off when a chemical reaction takes place, the reaction is 
a)
exothermic
b)
exerrgonic
c)
cooled
d)
endothermic
89.
What type of chemical reaction is shown in the equation AgNO3 + KCl     〉 AgCl + KNO3?
a)
synthesis
b)
decomposition
c)
single-displacement
d)
double-displacement
90.
A _________ chemical equation has the same number of atoms of each element on both sides of the equation.
a)
simple
b)
balanced
c)
unbalanced
d)
complex
91.
When you activate a hand warmers pack, water mixes with a chemical and the pack gets very warm. This is an example of:
a)
an endothermic reaction.
b)
an exothermic reaction.
c)
a combustion reaction
d)
a physical change.
92.
Which of the following could represent a synthesis reaction?
a)
element + element = compound
b)
compound = element + element
c)
element + compound = element + compound
d)
compound + compound = compound + compound
93.
Which of the following reactions produces water and CO2
a)
synthesis
b)
decomposition
c)
combustion
d)
double displacement
94.
What is wrong with the following chemical equation?
N2 + O2 > N2O
a)
too many oxygen atoms on the reactants side
b)
too many nitrogen atoms on the products side
c)
too many nitrogen atoms on the reactants side
d)
too many oxygen atoms on the products side
95.

What should be done to balance the following equation?

N2 + O2 > N2O

a)

Put a 2 in front of O2 and a 2 in front of N2O

b)

Put 3 in front of N2O

c)

put a 2 in front of N2 and a 2 in front of N2O

d)

put a 2 in front of N2

96.

How many hydrogen atoms are on the product side of the following chemical equation?

N2 + 3H2 > 2 NH3

a)

3

b)

5

c)

2

d)

6

97.
The product of bubbles is a sign that
a)
a chemical change is taking place
b)
a physical change is taking place
c)
oxygen is present
d)
organic chemicals are present
98.
What type of reaction is shown in the chemical equation Mg + 2HCl  -->  MgCl2 + H2?
a)
synthesis
b)
decomposition
c)
single-displacement
d)
double-displacement
99.
What type of reaction is shown in the chemical equation 2Na + Cl2 >  2NaCl?
a)
synthesis
b)
decomposition
c)
single-displacement
d)
double-displacement
100.
What type of reaction is shown in the chemical equation 2Al2O3 --> 4Al + 3O2?
a)
synthesis
b)
decomposition
c)
single-displacement
d)
double-displacement
101.
What type of reaction is shown in the chemical equation Pb(NO3)2 + 2NaCl --> 2NaNO3 + PbCl2?
a)
synthesis
b)
decomposition
c)
single-displacement
d)
double-displacement
102.
What type of reaction is shown in the chemical equation S8 + 12O2 --> 8SO3?
a)
synthesis
b)
decomposition
c)
single-displacement
d)
double-displacement
103.
Which element cannot be replaced by sodium in a single-replacement reaction?
a)
Pb
b)
Fe
c)
Ca
d)
Ag
104.
Is the following chemical equation balanced?
Na + I2 > NaI
a)
yes
b)
no
c)
maybe
d)
all of the above
105.
Which element cannot be replaced by iron in a single-replacement reaction?
a)
Pb
b)
Co
c)
Cu
d)
Zn
106.

When the equation Fe3O4 + Al --> Fe + Al2O3 is correctly balanced, what is the coefficient of Al?

a)

3

b)

4

c)

6

d)

8

107.
What is the small whole number that appears behind a chemical symbol in a formula in a chemical equation?
a)
a subscript
b)
a superscript
c)
a ratio
d)
a coefficient
108.
What are the correct coefficients when this equation is balanced?
Sb + O2 --> Sb4O6 
a)
1,2,10
b)
4,6,1
c)
4,3,1
d)
10,5,1
109.

Consider an aqueous solution of calcium nitrate added to an aqueous solution of sodium phosphate. What is the formula of the solid formed in the reaction?

a)

Ca(PO4)2

b)

CaPO4

c)

Ca3(PO4)2

d)

Ca3(PO3)2

110.

Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride and aqueous barium nitrate. The balanced complete ionic equation contains which of the following terms?

a)

2Ba2+(aq)

b)

Cl–(aq)

c)

2Ag+(aq)

d)

NO3– (aq)

111.

The net ionic equation for the reaction of calcium bromide and sodium phosphate contains which of the following species?

a)

2Br–(aq)

b)

PO43–(aq)

c)

2Ca3(PO4)2(s)

d)

3Ca2+(aq)

112.

The net ionic equation for the reaction of aluminum sulfate and sodium hydroxide contains which of the following species?

a)

3Al3+(aq)

b)

OH–(aq)

c)

3OH–(aq)

d)

2Al(OH)3(s)

113.

A double-replacement reaction takes place when aqueous cobalt(III) chloride reacts with aqueous lithium hydroxide. One of the products of this reaction is

a)

Co(OH)3.

b)

Co(OH)2.

c)

LiCo3.

d)

LiCl3.

114.
What is the molar mass of CO2?
a)
22.0 g/mol
b)
28.0 g/mol
c)
44.0 g/mol
d)
56.0 g/mol
115.
A mole of Neon contains
6.02 x 1023 _____.
a)
atoms
b)
formula units
c)
ions
d)
molecules
116.
How many moles are in 3.01 x 1022 atoms of magnesium?
a)
0.0500 moles
b)
1.81 x 1046 moles
c)
5.00 x 1021 moles
d)
5.00 moles
117.

How many molecules are in 2.00 moles of H2O?

a)

124x1024 molecules of H2O

b)

1.20x1023 molecules of H2O

c)

12.04 x1023 molecules H2O

d)

124

118.
How many atoms are in 1.50 moles of Hg?
a)
9.03x1023 atoms Hg
b)
9.03x1024 atoms Hg
c)
903 atoms of Hg
d)
9.03 atoms of Hg
119.

88.0 grams of CO2 is about _____________. [Select 2 answers.]

a)

1 mole of CO2

b)

2 moles of CO2

c)

6.02 x 1023 molecules of CO2

d)

two times 6.02 x 1023 molecules of CO2

120.

What is the molar mass of NaCl?

a)

58 g/mol

b)

28 g/mol

c)

12 g/mol

d)

6.02 x 1023

121.
Which has more molecules?
a)
1 mole CO2
b)
1 mole of N2O4
c)
1 mole of H2O
d)
They are all the same
122.

The sum of the percent by mass of each element in a compound must equal 100%.

a)

True

b)

False

123.

To find the percent by mass of a compound if you are given the formula, divide the molar mass of that element in one mole of the compound by the total molar mass of the compound.

a)

True

b)

False

124.

Which element has a molar mass of 30.974 g/mol?

a)

potassium

b)

phosphorus

c)

gallium

d)

palladium

125.

Which is the correct molar mass for the compound FeSO4?

a)

103.85 g/mol

b)

151.85 g/mol

c)

415.4 g/mol

d)

247.85 g/mol

126.

How many formula units are in 3.6 grams of NaCl?

a)

0.06

b)

1.0x1021

c)

1.3x1026

d)

3.7x1022

127.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
128.
What is the percent by mass of chlorine in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
129.
What is the percent composition by mass of magnesium in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
130.

The phase of matter in which the atoms are moving freely and are very far apart

a)

solid

b)

liquid

c)

gas

131.
What best describes the motion of atoms in a solid? 
a)
vibrating slowly in place
b)
sliding past each other
c)
moving rapidly in all directions
132.
Adding heat energy causes the atoms to...
a)
move slower
b)
move faster
c)
get bigger
d)
get smaller
133.

Removing energy (cooling) causes the atoms to

a)

spread apart

b)

move closer together

c)

get larger

d)

get smaller

134.

What state/phase is the object likely from points A to B?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

135.

Is the substance gaining or losing energy?

a)

Gaining

b)

Losing

136.

Use the graph below to answer this question. What state of matter would the substance be at point F?

a)

solid

b)

liquid

c)

gas

137.
As substance goes from D to E what happens to the distance between the particles?
a)
particles get closer together
b)
particles disappear
c)
particles get far apart
138.

Are the particles moving faster or slower as time goes on?

a)

Faster

b)

Slower

139.

On which parts of the graph does the temperature remain the same?

a)

Between C and D

b)

Between D and E

c)

At C, D, or E

d)

On both flat sections

140.

What phase change is happening? (hint: solid to liquid)

a)

freezing

b)

condensation

c)

melting

d)

sublimation

141.

What phase change happens when dew forms on leaves? (hint: gas to liquid)

a)

freezing

b)

melting

c)

deposition

d)

condensation

142.

The phase change from liquid to gas is _________

a)

Melting

b)

Evaporation

c)

Deposition

d)

Condensation

143.

Phase change from liquid to solid is ___________.

a)

Freezing

b)

Melting

c)

Sublimation

d)

Condensation

144.

All phase changes need energy added or taken away.

a)

True

b)

False

145.

At what point is the substance liquid?

a)

B

b)

A

c)

C

d)

D

146.

Which point shows evaporation or condensation driving a phase change?

a)

B

b)

E

c)

D

d)

A

147.
A change from solid to gas (without ever being a liquid) is called?
a)
Freezing
b)
Evaporation
c)
Condensation
d)
Sublimation
e)
Melting
148.

Sulfur has a melting point of 215 oC. This means that if Sulfur has a temperateure of 215 oC, what phase(s) of matter can it be in?

a)
Only Solid
b)
Only Liquid
c)
Only Gas
d)
Both Solid and Liqiud
e)
Both Solid, Liquid and Gas
149.

Sulfur has a melting point of 215 oC. This means that if Sulfur has a temperature of 220 oC, what phase(s) of matter can it be in?

a)
Only Solid
b)
Only Liquid
c)
Only Gas
d)
Both Solid and Liqiud
e)
Both Solid, Liquid and Gas
150.

What letter on the diagram represents the substance only in the gas phase?

a)

A

b)

B

c)

C

d)

D

151.

What letter on the diagram represents a substance only in the liquid?

a)

A

b)

B

c)

C

d)

D

152.

What letter on the diagram represents a substance only in the solid phase?

a)

A

b)

B

c)

C

d)

D

153.

What letter on the diagram represents the triple point?

a)

A

b)

B

c)

C

d)

D

154.

What is the melting point of this substance at 1 ATM of pressure?

a)

40

b)

60

c)

100

d)

110

155.

What is the boiling point of this substance at 1 ATM of pressure?

a)

40

b)

60

c)

100

d)

110

156.

What would the state of this substance be at 0.5 ATM of pressure at a 100 degrees Celsius?

a)

Solid

b)

Liquid

c)

Gas

d)

Michigan

157.

What would the state of this substance be at 1 ATM of pressure at a 80 degrees Celsius?

a)

Solid

b)

Liquid

c)

Gas

d)

Michigan

158.

Based on what you have learned... Is this substance likely water?

a)

Yes

b)

No

159.

What happens along the AC line?

a)

Melting/Freezing

b)

Boiling/Condensing

c)

Boiling/melting

d)

freezing/condensing

160.

What happens along the BC line?

a)

Melting/Freezing

b)

Boiling/Condensing

c)

Boiling/melting

d)

freezing/condensing

161.

The critical point is found at point.....

a)

A

b)

B

c)

C

d)

D

162.

What is being measured on the y axis?

a)

Pressure

b)

Temperature

c)

Energy

d)

Mass

163.

What is being measured on the x axis?

a)

Pressure

b)

Temperature

c)

Energy

d)

Mass

164.
Water exists as a _____________ at 700 mmHg and 50 °C.
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
165.

What will occur when the substance changes from 1 atm to 30 at a constant temperature of -15oC? (Diagram A)

a)

condensation

b)

deposition

c)

melting

d)

sublimation

166.

What will occur when the substance changes from 0o C to 100oC at a constant pressure of 30 atm? (Diagram A)

a)

condensation

b)

evaporation

c)

melting

d)

freezing

167.

What is the normal boiling point of this substance? (Diagram C)

a)

150 °C

b)

100 °C

c)

-50 °C

d)

0 °C

168.

What phase change occurs at letter E?

a)

Freezing

b)

Deposition

c)

Condensation

d)

Melting

169.

What phases of water are present at a temperature of 0.01°C and 0.006 atm of pressure?

a)

solid and liquid

b)

solid and gas

c)

solid, liquid, and gas

170.

WHAT IS THE PHASE CHANGE FROM C TO B?

a)

MELTING

b)

FREEZING

c)

VAPORIZATION

d)

CONDENSATION

171.
Which statement is true for carbon dioxide at -60 °C?
a)
All three phases are possible.
b)
It can exist as a solid or a gas, depending on pressure.
c)
It is a solid.
d)
With enough pressure it can be melted.
172.
What state of matter is X?
a)
solid 
b)
liquid
c)
gas
d)
supercritical fluid

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