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Chem30s - Review

Total questions: 193

Worksheet time: 6hrs 55mins

Name
Class
Date
1.

What is the mass of one mole of silver?

a)

32.06 g

b)

107.87 g

c)

14.01 g

d)

22.99 g

2.

48.86 g of cobalt is equal to how many moles of cobalt?

a)

2879 moles

b)

8.291 moles

c)

.8291 moles

d)

.829 moles

3.

How many molecules of water are in a 821.3 g sample?

a)

45.58 molecules

b)

8.232 x 1025 molecules

c)

8.909 x 1027 molecules

d)

2.744 x 1025 molecules

4.

What is the mass of 4.98 x 1024 atoms of Zn?

a)

541 g

b)

8.27 g

c)

.122 g

d)

4.59 x 1046 g

5.

How many moles of sodium chloride are in a 321.8 g sample?

a)

18810 moles

b)

3.315 x 1024 moles

c)

5.507 moles

d)

4.767 moles

6.

How many particles of calcium chloride are in a 25.69 g sample?

a)

1.394 x 1023 particles

b)

2851 particles

c)

.2315 particles

d)

3.845 x 1025 particles

7.

What would be the mass of 9.76 x 1022 particles units of SrCl2?

a)

.1622 g

b)

25.7 g

c)

20.0 g

d)

.3589 g

8.

how many atoms are contained in a 456 g sample of carbon dioxide?

a)

10.34 atoms

b)

6.237 x 1024 atoms

c)

1.871 x 1025atoms

d)

2.079 x 1024 atoms

9.

A sample of AlCl3 contains a total of 4.515 x 1027 atoms of chlorine. What must be the mass of this sample?

a)

2.500 x 105 g

b)

1.000 x 106 g

c)

18.75 g

d)

8.4 x 105 g

10.

Convert 86.235 g of diphosphorus pentaoxide to moles.

a)

12240 moles

b)

1.8747 moles

c)

.608 moles

d)

.607 moles

11.

The energy of movement is ___.

a)

potential energy

b)

kinetic energy

c)

mechanical energy

12.

The more energy that particles have, the ___ they move.

a)

slower

b)

faster

13.

The force of attraction between molecules is ___.

a)

intermolecular forces

b)

bridge forces

c)

chemical bonds

14.

These properties describe a ___.

a)

solid

b)

liquid

c)

gas

15.

These properties describe a ___.

a)

solid

b)

liquid

c)

gas

16.

These properties describe a ___.

a)

solid

b)

liquid

c)

gas

17.

Collisions in which particles transfer all their kinetic energy to other particles are called ___.

a)

elastic

b)

inelastic

18.

Which one of these is NOT an Ideal Gas Assumption?

a)

Gas particles are hard, round spheres.

b)

Gas particles are strongly attracted to one another.

c)

Gas particles do not take up space.

d)

Gas particles collide perfectly elastically.

19.

Liquid particles have more energy than ___ particles.

a)

solid

b)

gas

20.

The particles of ___ generally have the least amount of energy.

a)

solids

b)

liquids

c)

gases

21.
Which form of matter take the shape of a container like this juice?
a)
liquid
b)
solid
c)
glass
d)
gas
22.
What happens when my glass of water is sitting in the sun and disappears into a gas?
a)
evaporation
b)
burning
c)
melting
d)
freezing
23.
In a solid, the particles
a)
vibrate in place
b)
slide past one another
c)
overcome the strong attraction
d)
move freely in any direction
24.
Condensation is . . . .
a)
gas to liquid
b)
liquid to gas
c)
gas to solid
d)
solid to liquid
25.
Freezing (or solidification) is . . . .
a)
liquid to solid
b)
solid to liquid
c)
solid to gas
d)
solid to plasma
26.
5. What is it called when a solid turns directly into a gas?
a)
Sublimation
b)
Condensation
c)
Liquid
27.
The phase change from water vapor to liquid water is known as...
a)
evaporation
b)
precipitation
c)
condensation
d)
sublimation
28.
Vaporization includes _____________ and  _____________.
a)
melting and boiling
b)
condensation and boiling
c)
sublimation and freezing
d)
evaporation and boiling
29.
Endothermic phase changes include
a)
conduction, convection and radiation
b)
freezing and condensation
c)
vaporization and condensation
d)
melting, boiling, evaporation and sublimation
30.
Exothermic phase changes include
a)
conduction, convection and radiation
b)
freezing and condensation
c)
vaporization and condensation
d)
melting, boiling, evaporation and sublimation
31.
________________________ is the temperature at which a solid begins to liquefy.
a)
boiling point
b)
condensation point
c)
melting point
d)
evaporation point
32.
Deposition is the opposite of sublimation.
a)
True
b)
False
33.
What is the change from a Solid to a Gas due to the gaining of energy?
a)
Condensation
b)
Vaporization
c)
Sublimation
d)
Deposition
34.
4. What type of state of matter is a gas that has electrons flowing through it?
a)
Gas
b)
Liquid
c)
Plasma
d)
Solid
35.
At higher temperatures
a)
particles in an object have less energy
b)
particles in an object move faster
c)
a gas contracts
36.
Which of these is true?
a)
Solids hold their shape.
b)
Liquids hold their shape.
c)
Gases hold their shape.
d)
Penguins eat pineapples.
37.
True or false: Solids can be squashed or forced into a smaller space
a)
True
b)
False
38.

An amorphous solid has a definite melting point.

a)

True

b)

False

39.

Both gases and liquids are fluids.

a)

True

b)

False

40.

A state of matter with a definite volume, but no definite shape is a(n) _______.

a)

liquid

b)

solid

c)

gas

41.

The ____ of a gas is the force of its outward push divided by the area of the walls of its container.

a)

pressure

b)

gravity

c)

surface tension

d)

structure

42.

All solids have a closely packed, fixed arrangement of particles.

a)

True

b)

False

43.

The _______ is a measure of the average speed of the particles in a substance.

a)

temperature

b)

density

c)

volume

d)

mass

44.

What is a crystal?

a)

A pure material that can’t be changed.

b)

Material with a regular,repeating arrangement of atoms.

c)

A foggy like material.

45.
What type of solid is seen in the picture?
a)
Amorphous solid
b)
Regular solid
c)
Liquid
d)
Gas
46.

long-range order exists

a)

Crystalline material

b)

Amorphous Material

47.

long-range atomic order is absent

a)

Crystalline material

b)

Amorphous Material

48.

means a three-dimensional array of points coinciding with atom positions

a)

Lattice

b)

Amorphous

c)

Unit Cells

d)

FCC

49.

the basic structural unit or building block of the crystal structure and defines the crystal structure by virtue of its geometry and the atom positions within

a)

Lattice

b)

Amorphous

c)

Unit Cells

d)

FCC

50.

Allotropy is

a)

when more than one crystal structure is found in elemental solids

b)

when metals and nonmetals have more than one crystal structure

51.
HCl
a)
Polar 
b)
Nonpolar 
52.
F2
a)
Polar 
b)
Nonpolar 
53.
H2O
a)
Polar 
b)
Nonpolar 
54.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
55.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

56.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

57.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

58.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

59.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

60.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

61.

Why is the molecule polar?

a)

There is a nonbonding pair on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no nonbonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

62.

Classify the following molecule.

a)

polar

b)

nonpolar

63.

Classify the following molecule.

a)

polar

b)

nonpolar

64.

Classify the following molecule.

a)

polar

b)

nonpolar

65.

Classify the following molecule.

a)

polar

b)

nonpolar

66.
Boyle's law : When _______ is held constant, the pressure and volume of a gas are ________  proportional
a)
temperature,  equally
b)
mass, inversely
c)
temperature, inversely
d)
mass, equally
67.
What does Boyle's law relate to?
a)
Temperature and Volume
b)
Volume and Pressure
c)
Temperature and Pressure
68.
When the temperature of matter increases the particles...
a)
speed up and move closer
b)
speed up and move farther apart
c)
slow down and move closer together
d)
slow down and move farther apart
69.
How do gas molecules move? 
a)
in an orderly fashion 
b)
constantly and randomly
c)
in straight line paths
d)
in a circular motion
70.
In Charles' Law the pressure remains constant.
a)
True
b)
False
71.
True or False: Gases can be compressed. 
a)
True
b)
False
72.
What is the formula for Boyle's Law?
a)
P1V1=P2V2
b)
P1V1/P2V2
c)
P1V2=P2V1
d)
P1/V1=P2/V2
73.
When Pressure increases then the Volume must...
a)
Increase
b)
decrease
74.
When Volume increases then Pressure must...
a)
Increase
b)
Decrease
75.
What type of relationship to pressure and volume have?
a)
direct
b)
inverse
c)
no relationship
d)
I don't know
76.
Which container will have a lower pressure?
a)
left
b)
right
c)
they both have the same pressure
d)
I don't know
77.
What causes pressure?
a)
The walls of the container
b)
The vacuum in the container
c)
The collisions of the particles
d)
Atmospheric pressure acting on the outside walls
78.
The relationship of which two variables are compared in Boyle's Law?
a)
pressure & volume
b)
volume & temperature
c)
temperature & pressure
d)
volume & moles (amount of gas)
79.
What type of relationship is Charles' Law?
a)
Inverse
b)
Direct
c)
Not enough information
d)
#goals
80.
What is the formula Charles' Law?
a)
V = T
b)
VT = VT
c)
T1 / V1 = T2 / V2
d)
V1 / T1 = V2 / T2
81.

What type of relationship is Charles' Law?

a)

Inverse

b)

Direct

c)

Not enough information

82.
Gas Laws involve what three terms?
a)
Solid Liquid Gas 
b)
Speed Velocity Acceleration 
c)
Elements Compounds Mixtures 
d)
Pressure Temperature Volume 
83.
Charles' Law States...
a)
As Pressure goes up volume goes down
b)
As Pressure goes up temperature goes up
c)
As Volume goes up temperature goes up 
d)
As Pressure goes down volume goes down 
84.
Whose law states that as pressure goes up, volume goes down?
a)
Charles 
b)
Boyle
c)
Aglow
d)
Mazias 
85.
Which law?
a)
Charles 
b)
Boyle
c)
Hooke
d)
Peter Pan 
86.

Which law?

a)

Boyle

b)

Charles

c)

Landis

d)

Boykin

87.

Which law?

a)

Charles

b)

Boyle

c)

Diegel

d)

Mitchell

88.
A balloon will pop in the atmosphere because..
a)
Pressure goes down volume goes up
b)
Pressure goes up volume goes down
c)
temperature goes down volume goes up
d)
volume goes down temperature goes down
89.
Charles's law shows the relationship between which two factors of a gas ?
a)
volume and temperature 
b)
volume and pressure 
c)
pressure and volume
d)
volume and mass
90.
Directly proportional means that as one value increases ....................
a)
the other stays the same 
b)
the other increases as well
c)
the other decereases
d)
the other goes to zero
91.
Inversely proportional means as one value increases the other............. 
a)
increases 
b)
decreases 
c)
stays the same 
d)
goes to zero
92.
Temperature describes  the ______________ of particles.
a)
volume
b)
mass
c)
motion
d)
conductivity
93.
When a basketball is left outside in the cold it goes flat because the volume of air inside the ball has been reduced. What  gas law does this represent?
a)
Boyle's Law
b)
Charles's Law
94.
a)
this is a graph representing Boyle's law
b)
this is a graph representing Charles's law
95.
a)
This is an example of Charles's law
b)
This is an example of Boyle's law
96.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
97.
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
98.
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
99.
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
100.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
101.
What is 50 °C in Kelvin?
a)
223
b)
323
c)
100
d)
50
102.

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

103.

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

104.

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

105.

Unit inter-conversions allow different scales for measuring temperature, pressure or volume to be compared.

Which sets of pressures are equivalent ?

a)

160.94 kPa, 1260 torr, 1.42 atm

b)

145.95 kPa, 912 torr, 1.50 atm

c)

121.56 kPa, 912 torr, 1.20 atm

d)

0 kPa, 1000 torr, 1.40 atm

106.

A real gas does not exhibit ideal gas behaviour because

a)

there are significant attractions between molecules so that the volume of the gas is reduced

b)

the size of the particles are inconsequential and so their volume can be ignored in calculations

c)

the collisions between the gas particles are perfectly elastic and so no energy is gained or lost

d)

only noble gases are ideal gases and all other gases are called real gases

107.

Out of the following which of the three real gases would you expect to act most like an ideal gas ?

a)

Ammonia

b)

Hydrogen

c)

Nitrogen

d)

All of the gases would act like ideal gases

108.

A 0.0900 L syringe has a volume of :

a)

0.0900 mL

b)

9.0 mL

c)

90 mL

d)

900 mL

109.

Which of the following graphs represents pressure versus volume (V) for a real gas at a constant temperature

a)

A

b)

B

c)

C

d)

D

110.

This graph represents which gas law ?

a)

Grahams law

b)

Avogadros law

c)

Boyles Law

d)

Charles Law

111.

Which of the following is a pair of equivalent values ?

a)

-298 K and O o C

b)

298 K ans -273 o C

c)

319 K and 46 o C

d)

319 K and 592 o C

112.

Find the volume occupied by 22.0 g of helium gas at 25.0 o C and 1.18 atm .

a)

123 L

b)

9.57 L

c)

114 L

d)

159 L

113.

A gas sample has an initial volume of 55.2 mL, an initial temperature of 35.0 o C and an initial pressure of 735 mm Hg. The volume is decreased to 48.8 mL and the temperature is increased to 72.5 o C . What is the final pressure ?

a)

933 mm Hg

b)

186 mm Hg

c)

1.72 x 103 mmHg

d)

84.0 g Kr

114.

Which of the following term does not involve an ideal gas law ?

a)

Pressure

b)

Volume

c)

Temperature

d)

Time

115.

The combined gas law allows us to determine relationships between temperature, pressure and the volume of gases, including those used in a gas balloon. What is the final pressure if 155.0 mL of a gas at 22.0 o C and 374 mmHg is cooled to 0.00 o C and has a final volume of 102.0 mL

a)

526 mm Hg

b)

614 mmHg

c)

73.4 mmHg

d)

39.1 mmHg

116.

Select the dissociation equation for NaCl and show the physical states of all species involved.

a)

NaCl --> Na+ + Cl-

b)

NaCl(s) --> Na+(aq) + Cl-(aq)

c)

NaCl --> Na + Cl

d)

NaCl(s) --> Na(aq) + Cl(aq)

117.

Select the dissociation equation for LiOH and show the physical states of all species involved.

a)

LiOH(aq) --> Li+(s) + OH-(s)

b)

LiOH(s) --> Li+(aq) + OH- (aq)

c)

LiOH(s) --> Li+(aq) + O2(aq) + H2(aq)

d)

LiOH(s) --> Li+(aq) + O22-(aq) + H2+(aq)

118.

Select the dissociation equation for NaOH and show the physical states of all species involved.

a)

NaOH(s) --> Na+(aq) + OH-(aq)

b)

NaOH --> Na+ + OH-

c)

NaOH --> Na + OH

d)

NaOH(s) --> NaO-(aq) + H+(aq)

119.

Select the dissociation equation for KMnO4 and show the physical states of all species involved.

a)

KMnO4(s) --> K+(aq)+ Mn4+(aq) + O4 -(aq)

b)

KMnO4 --> K++ MnO4 -

c)

KMnO4(s) --> K+(aq) + MnO4 -(aq)

d)

KMnO4 --> K++ Mn4+ + O4 -

120.

Select the dissociation equation for AgClO3 and show the physical states of all species involved.

a)

AgClO3(s) --> Ag(aq) + ClO3(aq)

b)

AgClO3(s) -->Ag+(aq) + Cl2 (aq) + O2(aq)

c)

AgClO3(s) -->Ag+(aq) + Cl-(aq) + 3O2-(aq)

d)

AgClO3(s) --> Ag+(aq) + ClO3-(aq)

121.

Select the dissociation equation for PbCrO4 and show the physical states of all species involved.

a)

PbCrO4(s) ↔ Pb2+(aq) + CrO44-(aq)

b)

PbCrO4(s) ↔ Pb2+(aq) + CrO42-(aq)

c)

PbCrO4(s) ↔ Pb+(aq) + CrO4-(aq)

d)

PbCrO4(s) ↔ Pb4+(aq) + CrO44-(aq)

122.

Select the dissociation equation for Fe2O3 and show the physical states of all species involved.

a)

Fe2O3(s) ↔ 2Fe3+(aq) + 3O2-(aq)

b)

Fe2O3(s) ↔ Fe3+(aq) + O2-(aq)

c)

Fe2O3(s) ↔ 2Fe+(aq) + 3O-(aq)

d)

2Fe2O3(s) ↔ 2Fe+(aq) + 3O2-(aq)

123.

Select the dissociation equation for ZnCl2 and show the physical states of all species involved.

a)

ZnCl2(s) --> Zn2+(aq) + Cl-(aq)

b)

ZnCl2(s) --> Zn+(aq) + 2Cl-(aq)

c)

ZnCl2(s) --> Zn2+(aq) + 2Cl-(aq)

d)

ZnCl2(s) --> Zn+(aq) + Cl-(aq)

124.

Select the dissociation equation for Ca(NO3)2 and show the physical states of all species involved.

a)

Ca(NO3)2(s) -->Ca+(aq) + 2NO3- (aq)

b)

Ca(NO3)2(s) -->Ca2+(aq) + 2NO3- (aq)

c)

Ca(NO3)2(s) -->Ca2+(aq) + NO3- (aq)

d)

Ca(NO3)2 -->Ca+ + 2NO3-

125.

How do we define a solute?

a)

Usually a liquid, in which other materials dissolve to form a solution

b)

A substance that is dissolved in a solution

c)

A substance with sulfur in it

d)

When a solution contains a mixture of two substances

126.

amount of solute in a given amount of solvent

a)

concentration

b)

saturated

c)

solution

d)

suspension

127.

As you put in more solute in the solution, the concentration of the solution will...

a)

increase

b)

decrease

c)

stay the same

128.

____________ is the process where particles of a solvent completely surround the particles of a solute.

a)

solvation

b)

immisciblation

c)

dissolution

d)

saturation

129.

Which of these is NOT a factor that affects solvation?

a)

agitation/stirring

b)

increasing temperature

c)

increasing surface area

d)

adding dye

130.

A 'dilute' solution is a solution with a _____ concentration

a)

high or strong

b)

normal

c)

low or weak

131.

Solvation will happen if the attractive forces between the solute and solvent particles are stronger than the individual forces inside the solute and solvent themselves.

a)

True

b)

False

132.

Which of these would be most likely to decrease the rate of solvation?

a)

stirring or shaking

b)

breaking the solute into smaller pieces

c)

lowering the temperature

d)

increasing the temperature

133.

The overall energy change that occurs during the solution formation process is called the

a)

Endothermic change

b)

Exothermic change

c)

Heat of solution

d)

Attractive energy change

134.

What is the most common liquid solvent in Chemistry?

a)

Oil

b)

Water

c)

Hydrochloric Acid

d)

Sodium Chloride

135.
Anna filled a ​cup with hot tea. Then she added a sugar cube. ​Which of these will help to make the sugar cube dissolve more quickly? 
a)
stirring the hot tea
b)
adding more sugar cubes
c)
adding ice to the tea
d)
pouring more tea into the cup
136.
Ernesto and Amanda fill two cups with water. They use hot water in one cup and cold water in the other cup. Next, they will stir a spoon of salt into each cup.     

In which cup will the salt dissolve more slowly? 
a)
The salt will not dissolve in either cup
b)
The salt dissolves more slowly in the hot water
c)
The salt dissolves more slowly in the cold water
d)
The salt dissolves at the same speed in both cups
137.
Look at the diagram. In this diagram, the red dots represent
a)
the solute
b)
the solvent
c)
the solution
138.
Look at the diagram. In this diagram, the blue area represents
a)
the solute
b)
the solvent
c)
the solution
139.

water can't dissolve ...............

a)

sugar

b)

oil

c)

salt

d)

coffe

140.

when a solvent can no longer hold any more solute

a)

saturation

b)

dilute

c)

dissolve

141.
Capable of being dissolved
a)
Soluble
b)
concentration
c)
colloid
d)
molarity
142.
KBr
a)
Soluble
b)
Insoluble
143.
Zinc Hydroxide
a)
Soluble 
b)
Insoluble
144.
Silver Iodide
a)
Soluble 
b)
Insoluble 
145.
Zinc Carbonate
a)
Soluble 
b)
Insoluble 
146.
KOH
a)
Soluble 
b)
Insoluble
147.
Silver acetate
a)
Soluble 
b)
Insoluble
148.
NiCl2
a)
Soluble 
b)
Insoluble
149.
PbI2
a)
Soluble
b)
Insoluble
150.
NaC2H3O2
a)
soluble
b)
insoluble
151.
K2CO3
a)
soluble
b)
insoluble
152.
CaCO3
a)
soluble
b)
insoluble
153.
BaSO4
a)
soluble
b)
insoluble
154.
Ca(OH)2
a)
soluble
b)
insoluble
155.
FeS
a)
soluble
b)
insoluble
156.
K2SO4
a)
soluble
b)
insoluble
157.
AgCl
a)
soluble
b)
insoluble
158.
NH4NO3
a)
soluble
b)
insoluble
159.
BaCl2
a)
soluble
b)
insoluble
160.
Fe(C2H3O2)3
a)
soluble
b)
insoluble
161.

What of these is always soluble?

a)

Nitrates

b)

Phosphates

c)

Carbonates

d)

Hydroxides

162.
Which is an example of a solute?
a)
Egg whites
b)
Sugar
c)
Water
d)
Acetone
163.
Which is an example of a solvent?
a)
Salt
b)
Egg whites
c)
Water
d)
Sugar
164.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
165.
You can make a solution more concentrated by adding __________.
a)
solute
b)
solvent
c)
water
166.

Calculate the Molarity in a solution containing 40.0 g of NaCl dissolved in 500.0 ml of H2O.

a)

0.08 M

b)

12.5 M

c)

1.37 M

d)

0.74 M

167.

How many moles of solute are present in 50.0 mL of 0.20M KNO3?

a)

10.0 moles solute

b)

0.05 moles solute

c)

1.00 moles solute

d)

0.01 moles solute

168.

How many mL of stock solution of 2M NaCl do you need to prepare 100 mL of 0.150M NaCl?

a)

7.5 mL

b)

15 mL

c)

1333 mL

d)

200 mL

169.

As we dilute a solution.....

a)

The volume increases and the molarity (M) increases

b)

The volume increases and the molarity (M) decreases

c)

The volume decreases and the molarity (M) increases

d)

The volume decreases and the molarity (M) decreases

170.

If I have 340 mL of a 0.5 M NaBr solution, what will the concentration be if I add 560 mL more water to it?

a)

.188 M

b)

3.78 M

c)

.389 M

d)

1.76 M

171.

How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?

a)

27.8 mL

b)

.278 mL

c)

2.8 mL

d)

278 mL

172.

The amount of solute dissolved in a given amount of solvent.

a)

dilution

b)

concentration

c)

saturated solution

d)

supersaturated mixture

173.

When you dilute a solution, which of these values remains constant?

a)

The molarity (M)

b)

The total moles of solute

c)

The volume (V)

d)

The concentration

174.
What is the molar mass of (NH4)2CO3 ?
a)
144 g
b)
138 g
c)
96 g
d)
78 g
175.
What is a Excess Reagent?
a)
amount you end with
b)
what you run out of first
c)
what you have left over
d)
what you start with
176.
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
177.
N2 +  3H2 −->  2NH3 
How many moles of ammonia are produced when 3 moles of nitrogen react with hydrogen?
a)
6 moles ammonia
b)
1.5 moles ammonia
c)
9 moles ammonia
d)
9 moles hydrogen
178.
What is the other name for the mole?
a)
El Ocho
b)
Guacamole
c)
Avogadro's number
d)
De Wey
179.
Using the following equation:
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
180.
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
181.
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
182.
Using the following equation:
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
183.
6CO2 + 6H2O --> C6H12O6 + 6O2 
What is the total number of moles of water needed to make 2.5 moles of C6H12O6?
a)
2.5
b)
6
c)
12
d)
15
184.
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
185.
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
186.

N2 + 3H2 → 2NH3

What is the mole ratio between N2 and NH3 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

187.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
188.
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
189.

Given the reaction: 4Al + 3O2 --> 2Al2O3

How many moles of Aluminum oxide, Al2O3, can you produce if you have 2 moles of Al?

a)

3 mole

b)

2 mole

c)

1 mole

d)

0.5 mole

190.
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
191.

2 KClO3 → 2 KCl + 3 O2

How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?

a)

6.7 mol

b)

1.0 mol

c)

10.1 mol

d)

4.5 mol

192.

2 KClO3 → 2 KCl + 3 O2

How many moles of KCl are used when 6.7 moles of KClO3 decompose completely?

a)

6.7 mol

b)

1.0 mol

c)

10.1 mol

d)

4.5 mol

193.

Using the following equation:

Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)

How many moles of water can be made from 6 moles H2?

a)

4 moles water

b)

6 moles water

c)

9 moles water

d)

2 moles water