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CHM 130 Mid-Term Exam Review (Spring 2025)

Total questions: 93

Worksheet time: 5hrs 51mins

Name
Class
Date
1.

How many sig figs?

12 m

a)

2

b)

1

c)

0

d)

42

2.

How many sig figs?

0.0010 mg

a)

1

b)

2

c)

4

d)

5

3.

How many sig figs?

21.10 cm

a)

4

b)

3

c)

2

d)

1

4.

How many sig figs?

3805 mL

a)

5

b)

4

c)

3

d)

2

5.

Wood has a density of 5.53g/cm3. What must the volume of 33.3 g of wood be?

a)

0.16 cm3

b)

184 cm3

c)

6.02 cm3

d)

10.84 cm3

6.

The volume of a metal block is 5 cm3. If the density of the block is 250 g/cm3, what is the mass of the block ?

a)

1250 g

b)

1300 g

c)

1350 g

d)

50 g

7.

Organize these options into the right categories

Categorize the following

Color

Texture

Taste

Odor

Boiling Point

Reaction with Sulfur (Tarnish)

Reaction with Oxygen (Rust)

Physical Properties
Chemical Properties
8.

Organize these options into the right categories

Categorize the following

Flammability

Acidity or Basicity (pH)

Magnetic Ability

Density

Viscosity

Melting/Freezing Point

Chemical Properties
Physical Properties
9.

What are the units of molar mass?

a)

grams

b)

moles

c)

mol/gram

d)

grams/mol

10.

Place the steps of calculating the molar mass of a compound in the correct order.

a)

Write compound formula and list each element

b)

Count the number of each atom in the formula

c)

Get mass of each element from periodic table

d)

Multiply number of atoms of each element by the mass

e)

Add these values together for compound molar mass.

1)
2)
3)
4)
5)
11.

What is the molar mass of CO2?

a)

12 g/mol

b)

16 g/mol

c)

32 g/mol

d)

44 g/mol

12.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
13.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
14.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
15.

Calculate the moles in 12.7g of CaF2

a)

0.20 mol

b)

1,000.76 mol

c)

6.14 mol

d)

0.16 mol

16.
What is the mass of 0.89 mol of CaCl2?
a)

111 grams

b)

0.008 grams

c)

98.9 grams

d)

none of the choices

17.
How many molecules are in 9.44 moles of AlCl3?
a)
5.68 molec AlCl3
b)
5.68x1024 molec AlCl3
c)
0.705 molec AlCl3
d)
1.25x1023 molec AlCl3
18.
How many water molecules are in 5.2 moles of water?
a)
6.02 x 1023
b)
5.2
c)
3.1304 x 1024
d)
8.638 x 10-24
19.
How many moles are in 3.01 x 1022 atoms of magnesium?
a)
0.050 moles
b)
1.81 x 1046 moles
c)
5.00 x 1021 moles
d)
5.00 moles
20.

Rows (going across from left to right) in the Periodic Table are called

a)

Periods

b)

Groups/Families

c)

Cousins

d)

Metals

21.

Columns (going vertically from top to bottom) in the Periodic Table are called

a)

Periods

b)

Groups/Families

c)

Cousins

d)

Metals

22.

The element in Group 18, Period 2, of the Periodic Table is

a)

F

b)

Ne

c)

Cl

d)

He

23.

Formula for barium sulfide

a)

B2S3

b)

BaS

c)

Ba2S

d)

BaS2

24.

Name for PBr2

a)

phosphorus bromide

b)

phosphorus dibromide

c)

phosphorus dibromine

d)

phosphorus bromine

25.

Name for CO

a)

carbon monoxide

b)

carbon oxide

c)

monocarbon oxide

d)

carbide monoxide

26.
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
27.
H2+Cl2-->2HCl
How many moles of Cl2 are needed to react with 3 moles of H2?
a)
5
b)
2
c)
3
d)
6
28.

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

A problem asks how many moles of oxygen gas are needed to react completely with 6 moles of ethane (C2H6). What is the second step in setting up the problem?

a)
b)
c)
d)
29.

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

A problem asks how many moles of oxygen gas are needed to react completely with 6 moles of ethane (C2H6). What is the final answer for this problem?

a)

13 mol C2H6

b)

3 mol O2

c)

21 mol O2

d)

42 mol O2

30.

Given the equation:

2NaClO3 (s) → 2NaCl (s) + 3O2 (g)

2.00 moles of NaClO3 will produce how many grams of O2? (mass of O2 = 32g/mol)

a)

56 g of O2

b)

96 g of O2

c)

64 g O2

d)

32 g O2

31.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.27 g
b)
2.6 g
c)
690 g
d)
45 g
32.

2NaClO3 (s) → 2NaCl (s) + 3O2 (g)

12.00 moles of NaClO3 will produce how many grams of O2?

a)

576g of O2

b)

288 g O2

c)

256 g O2

33.

What type of elements make up covalent compounds?

a)

metal and non-metal

b)

non-metal and non-metal

c)

polyatomic ion + non-metal

d)

metal + polyatomic ion

34.

What type of elements make up ionic compounds?

a)

metal and non-metal

b)

non-metal and non-metal

c)

metal + metal

35.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
36.
In an endothermic reaction, heat is ,,,
a)
taken in
b)
given out
37.
During an endothermic reaction in a beaker if we are part of the surroundings and touched the beaker, it would feel _______. 
a)
Warm
b)
Cold
38.

P1 is 450mmHg and the Ptotal is 750mmHg. What is the pressure of the second gas, P2?

a)

200mmHg

b)

300mmHg

c)

450mmHg

d)

750mmHg

39.

Which of these is a chemical reaction?

a)

Cutting a piece of paper in half

b)

Lighting a match

c)

Mixing sugar and water

d)

Boiling water

40.

Which of these are reactants?

H2 + O2 -> H2O

a)

H2

b)

O2

c)

H2O

d)

All of the above

41.

Select the products:

CH4 + O2 -> H2O + CO2

a)

CH4

b)

O2

c)

H2O

d)

CO2

42.

…N2+…H2 → …NH3\ldots N_2+\ldots H_2\ \rightarrow\ \ldots NH_3  

(a)  

43.

…NaCl + …F2 → …NaF +…Cl2\ldots NaCl\ +\ \ldots F_2\ \rightarrow\ \ldots NaF\ +\ldots Cl_2  

(a)  

44.

The reaction A + B --> AB is classified as a _____ reaction.

a)

combination

b)

decomposition

c)

single replacment

d)

double replacement

45.

What class of reaction best describes the equation below: 2HI --> H2 + I2

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

46.

What class of reaction best describes the equation below: Zn + H2S --> ZnS + H2

a)

synthesis

b)

combustion

c)

single replacement

d)

double replacement

47.

What class of reaction best describes the equation below: FeS + HCl --> H2S + FeCl2

a)

synthesis

b)

combustion

c)

single replacement

d)

double replacement

48.
substance that dissolves
a)
solvent
b)
solution
c)
solute
d)
unsaturated
49.

Some lasers rely on a mixture of gases. In one gas laser, a mixture of carbon dioxide (CO2 ), nitrogen gas (N2 ), and hydrogen gas (H2 ) has a total pressure of 1.00 atm. If PCO2 is 0.39 atm and PN2 is 0.24 atm, what is the partial pressure of the hydrogen gas?

a)

1.63 atm

b)

0.37 atm

c)

0.63 atm

d)

0.92 atm

50.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

51.

If the pH of a solution is 4.0, what is the pOH?

a)

4.0

b)

10.0

c)

1.0 x 10 -4

d)

cannot be determined from the information

52.

The pH of a solution is 8.43. What is the [H3O+]concentration?

a)

3.7 x 10 -9

b)

1.0 x 10-8.43

c)

2.7 x 10-6

d)

1.0 x 10-14

53.

If the [H3O+] of a solution is 1 x 10-3 M, the pH is

a)

11

b)

-3

c)

3

d)

1

54.

Oranges have a [H3O+] of 1.7 x 10-2 M. Their pOH is

a)

1.77

b)

12.23

c)

10.91

d)

3.09

55.

If the [OH-] of a solution is 2.7 x 10-4 M, the pOH of the solution is

a)

10.44

b)

1.00

c)

3.57

d)

-4.43

56.

Find the pH of a solution with [OH-] = 8.41 x 10-4.

a)

3.08

b)

10.92

c)

9.88

d)

11.23

57.
What is the conjugate acid in the following equation?
a)
PO43- 
b)
HNO3 
c)
NO3- 
d)
HPO42-
58.
What is the conjugate base in the following reaction?
a)
HCO3- 
b)
HCl
c)
 H2CO3 
d)

Cl-

59.

How do Bronsted-Lowry conjugate acid-base pairs differ?

a)

differ by one H+

b)

Differ by one OH-

c)

Differ by two H+

d)

Differ by some number of H+

60.

What is NH4+ classified as?

a)

Acid

b)

Base

c)

Conjugate Acid

d)

Conjugate Base

61.
A compound that donates H+ ions is 
a)
A Bronsted-Lowry Acid
b)
An Arrhenius Acid
c)
A Bronsted-Lowry Base
d)
An Arrhenius Base
62.
What is the conjugate acid in the following equation?
a)
PO43- 
b)
HNO3 
c)
NO3- 
d)
HPO42-
63.

Given the reaction above, which compound is the acid?

a)

NH3

b)

HCl

c)

NH4+

d)

Cl-

64.

The conjugate acid of HCO3- is ___ and the conjugate base of HCO3- is ___.

a)
H2CO3; CO3-2
b)
CO3-2; CO3-2
c)
H2CO3; H2O
d)
H2O; H2CO3
65.

Calculate the molar mass of KOH.

a)

28 g/mol

b)

56 g/mol

c)

84 g/mol

d)

112 g/mol

66.

Calculate the molar mass of Cu2O.

a)

37 g/mol

b)

45 g/mol

c)

79.5 g/mol

d)

143 g/mol

67.
Isotopes are atoms of the same element that have the same number of __________ but different number of __________ . Therefore, isotopes of the same element have different masses. 
a)
protons, neutrons
b)
protons, electrons
c)
neutrons, protons
d)
electrons, protons
68.

76 protons and 114 neutrons

a)

Osmium-114

b)

Osmium-76

c)

Osmium-190

d)

Osmium-190.23

69.

What is the molarity of a solution containing 4 moles of KCl in 2.5 L of solution?

a)

1.6 M

b)

0.63 M

c)

10 M

d)

2.6 M

70.

What volume is needed to make a 2.45 M solution of KCl using 0.50 mol of KCl?

a)

4.9 L

b)

0.20 L

c)

1.2 L

71.
What is the molarity of 4 grams of sodium chloride in 3,800 mL of solution?
a)
0.018 M
b)
0.018 mol
c)
1.052 M
d)
1.052 mol
72.

What volume, in milliliters, of 10.0 M NaOH is needed to prepare 300.0 mL of 2.00 M NaOH by dilution?

a)

0.067 mL

b)

60.0 mL

c)

100 mL

d)

125 mL

73.

If I have 340.0 mL of a 0.500 M NaBr solution, what will the concentration be if I add 560.0 mL more water to it? (Remember to use the total new volume)

a)

.188 M

b)

3.78 M

c)

.389 M

d)

1.76 M

74.

What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250.0 mL?

a)

15.9 M

b)

0.636 M

c)

0.642 M

d)

1.59 M

75.

The chemical bond between a non-metal and another non-metal will be a ________ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

76.

Organize these options into the right categories

Categorize the following

O2

Cl2

CO

H2O

F2

NaCl

MgO

C6H12O6

P4

Homoatomic
Heteroatomic
77.

Organize these options into the right categories

Categorize the following

C6H12O6

H2

H2O

Na2CO3

BaOH

O3

HCl

NaCl

CH4

Polyatomic
Diatomic
Triatomic
78.

Convert: 150 ⁰F to ⁰C: (a)  

Choose from the below words
66 ⁰C
101 ⁰C
339 ⁰C
118 ⁰F
79.

Convert: 186.5 K to C (a)  

Choose from the below words
-86.4 C
-50 C
-68.4 C
180 K
80.

Convert 24 ⁰F to Kelvin (a)  

Choose from the below words
269 K
90 K
140 K
250 K
81.

Convert 1350 mmHg to atm (a)  

Choose from the below words
1770 atm
17.7 atm
1026000 atm
1.78 atm
82.

Solve the following problem:

What is the volume of a balloon if it contains 3.2 moles of helium at a temperature of 20⁰C and 1.2 atm?

a)

106.55 K

b)

53.3 L

c)

293 K

d)

64.15 L

83.

Solve the following probem:

What pressure is required to contain 0.23 moles of nitrogen gas in a 4.2 L container at a temperature of 20⁰C?

a)

1.32 atm

b)

0.048 atm

c)

2.49 atm

d)

19.32 atm

84.

What does the variable "R" represent in the ideal gas law?

a)

pressure

b)

volume

c)

moles

d)

the gas constant

e)

temperature

85.

A gas tank carrying 55L of Cl2 has a pressure of 2.6atm and a temperature of 289K. How many moles of chlorine gas are in the tank?

a)

6.03 mol

b)

0.55 mol

c)

1.45 mol

d)

0.75 mol

86.

What is the ion formed from Sulfur?

a)

S+2

b)

S-2

c)

S+6

d)

S-6

87.
What charge will an Oxygen ion have? 
a)
+1
b)
-1
c)
+2
d)
-2
88.
Group 17 always has ions with a charge of 
a)
+1
b)
+2
c)
-1
d)
-2
89.

What is the charge of a sodium ion?

a)

+2

b)

+1

c)

-1

d)

-2

90.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
91.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
92.

Atomic size generally increases as we move __________.

a)

down a group and from right to left across a period

b)

up a group and from left to right across a period

c)

down a group and from left to right across a period

d)

up a group and from right to left across a period

93.

An electron that resides in the outermost energy level of an atom

a)

periodic trend

b)

electron shell

c)

ionic radius

d)

valence electron

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