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Regents Chemistry midterm Review

Total questions: 174

Worksheet time: 4hrs 52mins

Name
Class
Date
1.
How many significant figures does the following number have: 0.002040
a)
6
b)
4
c)
3
d)
2
2.
What is 78.5 rounded to one significant figure?
a)
79
b)
78.5
c)
70
d)
80
3.
Determine the number of Significant Figures in 10-L.
a)
4
b)
3
c)
2
d)
1
4.
What would be the effect on the particles if more heat is supplied to the system?
a)
They would slow down
b)
They would stop moving
c)
They would speed up
d)
There would be no effect
5.

If two objects have different temperatures when they come in contact, heat will flow from the warmer object to the cooler one UNTIL ____________

a)

one reaches a temperature of zero

b)

they both have an equal temperature

c)

one runs out of energy

6.
The SI unit of heat and energy is the __________.
a)
calorie
b)
heat
c)
joule
d)
watt
7.

1. Which of the following molecules is the most polar?

a)

H − Cl

b)

H − Br

c)

H − I

d)

H − F

8.

Which of the following compounds is the most ionic?

a)

KF

b)

HF

c)

LiF4

d)

CF4

9.

Which of the following correctly lists the molecule and its type of bond?

a)

CaO Ionic bond

b)

Br2 Polar covalent bond

c)

CH4 Polar covalent bond

d)

NaI Coordinate covalent bond

10.

What is the type of bond X?

a)

Ionic

b)

Pure covalent

c)

Polar covalent

d)

Nonpolar covalent

11.
This particle is found in the nucleus and has no charge
a)
Neutron
b)
Proton
c)
Electron
12.
This particle is found in the nucleus and has a positive charge
a)
Electron
b)
Proton
c)
Neutron
13.
This is a negatively charged particle found outside the nucleus
a)
Electron
b)
Proton
c)
Neutron
14.
This contains most of the mass of an atom
a)
Electron Cloud
b)
Nucleus
c)
Electron
15.
All matter is made of what?
a)
energy 
b)
atoms 
c)
electrons 
d)
compounds 
16.
Rutherford's gold foil experiment provided evidence that...
a)
negative and positive charges are spread evenly throughout the atom.
b)
alpha particles have a positive charge.
c)
gold is not a dense as previously thought.
d)
there is a dense positively charged nucleus at the center of an atom.
17.
An atom's overall charge is ________.
a)
positive 
b)
depends
c)
neutral 
d)
negative 
18.
What does the nucleus of an atom contain?
a)
Electrons and neutrons
b)
Protons and neutrons
c)
Neutrinos and positrons
d)
DNA and RN
19.
True or False: The majority of an atom is made up of empty space
a)
True
b)
False
20.
Contributes basically no mass to an atom.
a)
protons
b)
neutrons
c)
electrons
d)
protons and neutrons
21.
The majority of an atom's mass exists where?
a)
In the nucleus
b)
In the electron cloud
c)
In the space between the nucleus and the electrons
d)
In the neutrons
22.
Which particle is responsible for the chemical properties of an atom?
a)
Neutron
b)
Protons
c)
Valence Electrons
d)
Nucleus
23.
Neon has an atomic number of 10 and an atomic mass of 20.180.  How many protons, electrons, and neutrons will it have?
a)
P=10 E=10 N=11
b)
P=5  E=5  N=10
c)
P=10  E=10  N=10
d)
P=10  E=5  N=5
24.
What element is pictured?
a)
Hydorgen
b)
Boron
c)
Beryllium
d)
Arsenic
25.
The atomic number for Oxygen is 8, so
a)
there are 8 protons in the atom
b)
the atomic mass is less than 8
c)
the mass of the atom is 8
d)
the atom is decaying
26.

-183 oC to Kelvin

a)

-20 K

b)

183 K

c)

90 K

d)

83 K

27.

100 K to Celsius

a)

273 o C

b)

373 0 C

c)

-273oC

d)

-173 o C

28.

What is the symbol for the SI base unit of mass?

a)

g

b)

lb

c)

mg

d)

kg

29.

What is the unit symbol for temperature?

a)

C

b)

K

c)

F

d)

cd

30.

Convert 273 K to oC

a)

0oC

b)

100oC

c)

-273oC

d)

50oC

31.

Convert 5900 K to oC

a)

6173 oC

b)

5627 oC

32.
Which is a quality that only gasses display
a)
Spread out to fill all available space
b)
Take the shape of their container
c)
Can't be compressed
d)
All of these
33.
How do you convert Celsius to Kelvin?
a)
Add 273
b)
Subtract 273
c)
You can't convert those
d)
They are the same thing
34.
Endothermic reactions feel
a)
warm
b)
cold
35.
Exothermic reactions feel
a)
warm
b)
cold
36.
energy in endothermic reactions are
a)
released
b)
ended
c)
absorbed
37.
energy in exothermic reactions are
a)
released
b)
absorbed
38.
Heat is measured in 
a)
joules
b)
grams
c)
degrees celcius
39.

A covalent bond is formed when two atoms

a)

share an electron with each other.

b)

share one or more pairs of electrons with each other.

c)

gain electrons.

d)

gain and lose electrons.

40.

A single covalent bond involves the sharing of

a)

only one electron.

b)

two electrons.

c)

three electrons.

d)

a variable number of electrons, which depends on the bonding atoms.

41.

Use the table below to choose the pair of elements that will most likely have the least ionic character.

Element = Na

Electronegativity = 0.9

Element = O

Electronegativity = 3.5


Element = Cl

Electronegativity = 3.0


Element = H

Electronegativity = 2.1

a)

Na and Cl

b)

O and Cl

c)

H and O

d)

Na and O

42.
(4B) When sodium and fluorine atoms combine to produce the compound NaF, the ions formed have the same electron configuration as the atom(s) of
a)
Argon, only
b)
Neon, only
c)
Both argon and neon
d)
Neither argon nor neon
43.
(4G) Which statement is true concerning the reaction: 
N(g) + N(g) --> N2(g)
a)
A bond is formed and energy is released
b)
A bond is formed and energy is absorbed
c)
A bond is broken and energy is released
d)
A bond is broken and energy is absorbed
44.
(4G) When a bond is broken in compounds, energy is generally
a)
released, and the reaction is exothermic
b)
released, and the reaction is endothermic
c)
absorbed, and the reaction is exothermic
d)
absorbed, and the reaction is endothermic
45.
(4G) Given the balanced equation representing a reaction:
Cl2(g) + energy --> Cl + Cl
Describe energy change during this reaction
a)
Energy is released as a bond is formed
b)
Energy is absorbed as a bond is formed
c)
Energy is released as a bond is broken
d)
Energy is absorbed as a bond is broken
46.
(4C) In which pair of elements will electrons be transferred from one another?
a)
H to O
b)
Li to Cl
c)
N to F
d)
H to C
47.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

48.

How many valence electrons should Lithium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

49.

This is a correct dot diagram for nitrogen (N)

a)

true

b)

false

50.

Which is the correct Lewis Dot Structure for H2S?

a)
b)
c)
51.

Which is the correct Lewis Dot Structure for NH3?

a)
b)
c)
52.
When chlorine reacts it wants to ______________ electron.
a)
gain 1
b)
lose 1
c)
gain 2
d)
lose 2
53.
When Aluminum forms an ionic compound then it will ________________ electron(s).
a)
gain 1
b)
gain 2 
c)
gain 3
d)
lose 3 
54.
Traveling down a family the atomic radii ______________.
a)
Increases
b)
Decreases
c)
Stays the same
55.
Traveling across a period the atomic radii ______________.
a)
Increases
b)
Decreases
c)
Stays the same
56.
How does ionization energy change as I go across a period ?
a)
It doesn't
b)
It increases
c)
It decreases
57.
How does ionization energy change as I go down a family?
a)
It doesn't
b)
It increases
c)
It decreases
58.
Each element wants to gain or lose electrons so that it can have the same electron configuration as......
a)
a Nobel gas
b)
other elements in its family
c)
other elements in its period
d)
it used to have before reacting
59.
Most elements will gain or lose electrons so that they end up with _______ valence electrons.
a)
2
b)
6
c)
8
d)
10
60.
Ionization Energy is defined as.....
a)
The smallest amount of energy possible to excite an electron to a higher energy level
b)
The amount of energy given off when an electron returns to a ground state
c)
The amount of energy in one photon
d)
The energy required to remove one electron from a neutral atom
61.
How many valence electrons does Helium have?
a)
1
b)
2
c)
8
62.
When Nitrogen reacts with sodium, then _______nitrogen takes _____________.
a)
2 N takes 1 N from each sodium
b)
3 Nitrogen takes 2 electrons from each of 3 sodium
c)
1N takes 1 electron from each of 3 sodium
d)
1 N takes 2 electrons from each sodium
63.
When electrons are swapped or traded then ______________ bonds are formed.
a)
Ionic
b)
Covalent
c)
double
d)
single
64.
When electrons are shared then ____________ bonds / compounds are formed.
a)
Ionic
b)
Covalent
c)
single
d)
double
65.
A anion will be a ____ ion.
a)
negative
b)
positive
66.
A cation is a ____ ion.
a)
negative
b)
positive
67.

In a ___ bond, the atoms share electrons equally because of no difference in electronegativity.

a)

polar covalent

b)

nonpolar covalent

c)

ionic

68.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
69.
What happens in ALL chemical changes?
a)
Change in state of matter
b)
A new substance is formed
c)
Bubbles are produced
d)
An explosion
70.
Is wood burning a physical or chemical change?
a)
Physical 
b)
Chemical
71.

A phase change is a...

a)

physical change

b)

chemical change

72.

During which phase change does a substance absorb energy?

a)

freezing

b)

condensation

c)

evaporation

d)

deposition

73.

During which phase change does a substance release energy?

a)

condensation

b)

evaporation

c)

melting

d)

sublimation

74.

Which phase change is endothermic?

a)

condensation

b)

deposition

c)

melting

d)

freezing

75.

What is happening to the kinetic energy at interval AB?

a)

increasing

b)

decreasing

c)

staying constant

76.

What is happening to the potential energy at interval AB?

a)

increasing

b)

decreasing

c)

staying constant

77.

What is happening to the kinetic energy at interval BC?

a)

increasing

b)

decreasing

c)

staying constant

78.

What is happening to the potential energy at interval BC?

a)

increasing

b)

decreasing

c)

staying constant

79.

Which particle diagram shows a solid?

a)
b)
c)
80.

When particles of a substance move faster, their kinetic energy...

a)

increases

b)

decreases

c)

stays constant

81.

When temperature increases, kinetic energy...

a)

increases

b)

decreases

c)

stays constant

82.

At what time interval is the substance melting?

a)

AB

b)

BC

c)

CD

d)

DE

83.

At what time interval is the substance evaporating?

a)

AB

b)

BC

c)

CD

d)

DE

84.

Which particle diagram shows a liquid?

a)
b)
c)
85.

Which particle diagram shows a gas?

a)
b)
c)
86.

Which formula would you use to calculate the heat absorbed when ice is melted at its melting point?

a)
b)
c)
87.

Which formula would you use to calculate the heat absorbed when water is heated from 10°C to 20 °C?

a)
b)
c)
88.

Which formula would you use to calculate the heat absorbed when water is boiled at 100°C?

a)
b)
c)
89.

Which formula would you use to calculate the heat released when water is frozen at 0°C?

a)
b)
c)
90.

Which formula would you use to calculate the heat released when water vapor condenses to a liquid?

a)
b)
c)
91.

How much heat is released when 20.0 grams of water is cooled from 65°C to 55°C?

a)

300 J

b)

836 J

c)

6,680 J

d)

10,800 J

92.

How much heat is required to completely vaporize a 37 gram sample of water at its boiling point of 100°C?

a)

370 J

b)

3,700 J

c)

12,358 J

d)

83,620 J

93.

The temperature of a sample of water changes from 55°C to 77°C when the sample absorbs 1,103.5 joules of heat. What is the mass of the sample?

a)

7 grams

b)

12 grams

c)

50 grams

d)

72 grams

94.

A 25-gram sample of H2O(l) at 25°C absorbs 731.5 joules of heat. What will be the final temperature of the water?

a)

32°C

b)

21.8°C

c)

-18°C

d)

7°C

95.

During a flame test, sodium chloride produces an intense yellow flame. This yellow color is produced when electrons in excited atoms

a)

are gained by the atoms

b)

are lost by the atoms

c)

move to higher energy states within the atoms

d)

move to lower energy states within the atoms

96.

In an atom, an orbital represents

a)

the most probably location of a proton

b)

the most probable location of an electron

c)

the least probably location of a neutron

d)

photons emitted as electrons move to lower energy levels

97.

Which particle has a mass so small, it is considered to be 0 amu?

a)

proton

b)

hydrogen nucleus

c)

neutron

d)

electron

98.

What quantity is the same among atoms of the same element?

a)

mass number

b)

atomic number

c)

number of neutrons

d)

number of nucleons

99.

An atom that has 8 protons and 10 neutrons is an isotope of the element

a)

nitrogen

b)

oxygen

c)

fluorine

d)

neon

100.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

101.
subatomic particles found on the outermost shell & responsible for the atom's reactivity
a)
neutrons
b)
valence electrons
c)
isotopes
d)
ions
102.

Measure mainly of the nuclear particles: protons + neutrons

a)

Subatomic Particles

b)

Atomic Number

c)

Mass Number

d)

Gluons

103.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
104.
The smallest particle of an element that shows all the properties of that element.
a)
Subatomic Particles
b)
Atom
c)
Quarks
d)
Gluons
105.
Rutherford's gold foil experiment provided evidence that...
a)
negative and positive charges are spread evenly throughout the atom.
b)
alpha particles have a positive charge.
c)
gold is not a dense as previously thought.
d)
there is a dense positively charged nucleus at the center of an atom.
106.
J.J. Thomson provided evidence that an atom...
a)
is the smallest particle of matter
b)
contains negatively charged particles
c)
has an overall negative charge
d)
has an overall positive charge
107.

According to the wave-mechanical model of the atom, an orbital is a region of the most probable location of

a)

an alpha particle

b)

a gamma ray

c)

an electron

d)

a proton

108.

Which particles have approximately the same mass?

a)

an electron and an alpha particle

b)

an electron and a proton

c)

a neutron and an alpha particle

d)

a neutron and a proton

109.

Compared to the energy and charge of the electrons in the first shell of a Be atom, the electrons in the second shell of this atom have

a)

less energy and the same charge

b)

less energy and a different charge

c)

more energy and the same charge

d)

more energy and a different charge

110.
A tiny but very dense, positively charged portion of the atom that holds most of the atomic mass
a)
Electron Shells
b)
Orbitals
c)
Electron Cloud
d)
Nucleus
111.
Calculation used to find the number of neutrons in an atom
a)
Atomic Mass - Atomic Number
b)
Atomic Number - Atomic Mass
c)
Atomic Mass - Electrons
d)
none of these
112.

Based on the information in the table, which two atoms are isotopes of the same element?

a)

A and D

b)

A and Z

c)

X and D

d)

X and Z

113.

What is the structure of a krypton-85 atom?

a)

49 electrons, 49 protons, and 85 neutrons

b)

49 electrons, 49 protons, and 49 neutrons

c)

36 electrons, 36 protons, and 85 neutrons

d)

36 electrons, 36 protons, and 49 neutrons

114.

The nucleus of an atom of cobalt-58 contains

a)

27 protons and 31 neutrons

b)

27 protons and 32 neutrons

c)

59 protons and 60 neutrons

d)

60 protons and 60 neutrons

115.

Which two notations represent different isotopes of the same element?

a)
b)
c)
d)
116.

Which statement best explains why most atomic masses on the Periodic Table are decimal numbers?

a)

Atomic masses are determined relative to an H–1 standard.

b)

Atomic masses are determined relative to an O–16 standard.

c)

Atomic masses are a weighted average of the naturally occurring isotopes.

d)

Atomic masses are an estimated average of the artificially produced isotopes.

117.

Based on the information in the table, which numerical setup can be used to calculate the atomic mass of the element bromine?

a)

(78.92 u)(50.69) + (80.92 u)(49.31)

b)

(78.92 u)(49.31) + (80.92 u)(50.69)

c)

(78.92 u)(0.5069) + (80.92 u)(0.4931)

d)

(78.92 u)(0.4931) + (80.92 u)(0.5069)

118.

If 75.0% of the isotopes of an element have a mass of 35.0 amu and 25.0% of the isotopes have a mass of 37.0 amu, what is the atomic mass of the element?

a)

37.0 amu

b)

35.5 amu

c)

36.0 amu

d)

35.0 amu

119.

The average isotopic mass of chlorine is 35.5. Which mixture of isotopes (shown as percents) produces this average mass?

a)

50% 12C and 50% 13C

b)

50% 35Cl and 50% 37Cl

c)

75% 12C and 25% 13C

d)

75% 35Cl and 25% 37Cl

120.

Location of an electron

a)

outside the nucleus

b)

inside the nucleus

121.

Charge of an electron

a)

negative charge

b)

positive charge

c)

neutral

122.

Why is an atom neutral?

a)

same number of protons and electron

b)

fewer neutrons than electrons

c)

more protons than electrons

123.
Valence electrons are the...
a)
Innermost electrons
b)
Middle electrons
c)
Outermost electrons
d)
Any electrons
124.

How many valence electrons does carbon have?

a)

4

b)

5

c)

6

d)

7

125.

USE THE PERIODIC TABLE

How many valence electrons does sodium have?

a)

1

b)

2

c)

3

d)

4

126.

USE THE PERIODIC TABLE

How many valence electrons does Phosphorus have?

a)

31

b)

5

c)

15

d)

4

127.

USE THE PERIODIC TABLE

How many valence electrons does Phosphorus have?

a)

31

b)

5

c)

15

d)

4

128.
How many electrons should Beryllium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
129.
How many electrons should Aluminium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
130.

Which of the following is the correct electron-dot diagram for an atom with an electron configuration of 2-8-18-5?

a)
b)
c)
d)
131.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

132.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
133.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

134.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Helium

135.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

136.

The diagram represents the bright-line spectra of four elements and a bright-line spectrum produced by a mixture of three of these elements. Which element is not present in the mixture?

a)

A

b)

D

c)

X

d)

Z

137.

Which energy level of Calcium has the most energy?

a)

1st

b)

2nd

c)

3rd

d)

4th

138.
Barium atoms want to form...
a)
an anion
b)
a cation
c)
an onion
d)
a cuddly kitten friend
139.
Cations are...
a)
Positive
b)
Negative
c)
Neutral
d)
Purring
140.
Anions are...
a)
Positive
b)
Negative
c)
Neutral
d)
Crying
141.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
142.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
143.
What is a Rubidium ion's symbol?
a)
Rb-
b)
Rb+
c)
Rb-2
d)
Rb+2
144.

Which pair of atoms will form ionic bonds?

a)

S and F

b)

Mg and O

c)

F and Cl

d)

H and Ne

145.

How would you classify NaCl?

a)

element

b)

compound

c)

heterogeneous mixture

d)

homogeneous mixture

146.

How many electron pairs are shared between the atoms in an N2 molecule?

a)

1

b)

2

c)

3

d)

4

147.

As the elements in Group 2 in the periodic table are considered in order of increasing atomic number, there is a general increase in

a)

stability

b)

atomic radius

c)

electronegativity

d)

first ionization energy

148.

When iron is mixed with sulfur, the iron

a)

becomes a covalent compound

b)

retains its magnetic properties

c)

loses its magnetic properties

d)

transfers its magnetic properties to sulfur

149.

Which compound has both ionic and covalent bonds?

a)

CH4

b)

CO

c)

CaCl2

d)

MgSO4

150.

Which formula represents a polar molecule?

a)

Cl2

b)

CH4

c)

HCl

d)

CO2

151.

Which electron configuration represents the atoms of a bromine atom in the excited state?

a)

2-8-18-7

b)

2-8-18-8

c)

2-8-17-8

d)

2-8-18-7-1

152.

What is the overall charge of an ion that has 9 protons, 11 neutrons, and 10 electrons?

a)

+1

b)

-1

c)

+2

d)

-2

153.

Which atom has the lowest electronegativity?

a)

Nitrogen

b)

Oxygen

c)

Fluorine

d)

Neon

154.

In a bond between an atom of hydrogen and an atom of chlorine, the hydrogen atom has a

a)

weaker attraction for electrons

b)

stronger attraction for electrons

c)

smaller number of first-shell atoms

d)

larger number of first-shell atoms

155.

Which elements have the most similar chemical properties?

a)

Ge, As, and Sb

b)

Mn, Fe, and Co

c)

S, Se, and Te

d)

P, S, and Cl

156.

Most elements on the periodic table are classified as ____________.

a)

Gases

b)

Metalloids

c)

Metals

d)

Nonmetals

157.

Which accurately describes nonmetals?

a)

Poor conductors of electricity

b)

Often used in computer parts

c)

Both malleable and ductile

d)

Both dull and brittle

158.

Groups on the periodic table are arranged...

a)

Vertically

b)

Horizontally

c)

Diagonally from bottom right corner

d)

Diagonally from top right corner

159.

Which group on the periodic table is the most reactive?

a)

Group 1

b)

Group 2

c)

Group 13

d)

Group 18

160.

How many Valance electrons does Iodine Have?

a)

6

b)

16

c)

7

d)

17

161.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
162.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
163.

Electronegativity is

a)

How much an atom wants an electron

b)

How hard it is to remove an electron

c)

How many electrons an atom has

d)

How negative an electron is

164.

Ionization energy is

a)

The energy required gain an electron

b)

How hard it is to remove an electron

c)

The energy required to combine two elements

d)

None of the above

165.

What is the name of PbO2

a)

Lead Oxide

b)

Lead (II) Oxide

c)

Lead (IV) Oxide

d)

Lead Hydroxide

166.

Which element consists of positive ions immersed in a "sea" of mobile electrons?

a)

Sulfur

b)

Nitrogen

c)

Calcium

d)

Chlorine

167.

What is the chemical formula for sodium oxalate?

a)

NaO

b)

Na2O

c)

NaC2O4

d)

Na2C2O4

168.

What is the number of moles of CO2 in a 220.-gram sample of CO2 (gram-formula mass = 44 g/mol)?

a)

0.20 mol

b)

5.0 mol

c)

15 mol

d)

44 mol

169.

Which formula represents an asymmetrical molecule?

a)

CH4

b)

CO2

c)

N2

d)

NH3

170.

A measured value for the atomic radius of platinum atoms was determined to be 143 picometers. Based on Table S, what is the percent error of this measured value?

a)

0.10%

b)

9.1%

c)

10.%

d)

13%

171.

The results of these tests suggest that

a)

both solids contain only ionic bonds

b)

both solids contain only covalent bonds

c)

Solid A contains only covalent bonds and solid B contains only ionic bonds

d)

Solid A contains only ionic bonds and solid B contains only covalent bonds

172.

Which phrase describes the distribution of charge and the polarity of a CH4 molecule?

a)

symmetrical and polar

b)

symmetrical and nonpolar

c)

asymmetrical and polar

d)

asymmetrical and nonpolar

173.
What is the molar mass of Mg(NO3)2
a)
148.313g/mol
b)
134.306g/mol
c)
54.311g/mol
174.
Molar mass is in units of ________.
a)
grams
b)
grams/mole
c)
mole
d)
moles/gram

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