wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Exam I: CHMY 141 Spring 2020

Total questions: 119

Worksheet time: 5hrs 56mins

Name
Class
Date
1.
5,000 mg = ____ g
a)
50
b)
5
c)
500
d)
5,000
2.

What below is the largest value?

a)

6.3 x 10-10 Gm

b)

6.3 x 10-1 km

c)

6.3 x 1013 nm

d)

6.3 x 103 cm

3.

The unit of mass in the SI metric system is the

a)

gram

b)

kilogram

c)

newton

d)

centigram

4.

Which lists metric units, in order, from smallest to largest?

a)

milligram, centigram, gram

b)

kilogram, gram, centigram

c)

decagram, hectogram, milligram

d)

kilogram, hectogram, decagram

5.
What is another way you can make reference to the metric system?
a)
International de System
b)
English system
c)
Standard 
d)
Inches
6.

What does 105 = ?

a)

100,000

b)

10 x 5

c)

50

d)

500

7.

Convert 298 K to degrees Celsius.

a)

273 °C

b)

571 °C

c)

25.2 °C

d)

-273 °C

e)

0.00 °C

8.
This bullseye demonstrates...
a)
High Accuracy & High Precision
b)
High Accuracy & Low Precision
c)
Low Accuracy & High Precision
d)
Low Accuracy & Low Precision
9.

The density of lead is 11.342 g/mL. What would be the volume of a 200.0 g sample of this metal?

a)

0.05671 mL

b)

17.63 mL

c)

2268 mL

d)

17.634 mL

10.
How many significant figures does the following number have: 0.002040
a)
6
b)
4
c)
3
d)
2
11.
How many significant figures does the following number have: 100.00210
a)
7
b)
5
c)
10
d)
8
12.
Round 0.010229 to four sig figs
a)
1022
b)
1023
c)
0.01023
d)
0.01022
13.
Round 1047.78 to three sig figs
a)
104
b)
105
c)
1050
d)
1050.00
14.
How many sig figs are there?
0.000008
a)
1
b)
2
c)
6
d)
7
15.

How many sig figs are in the following measurements?

300 100 000 g

a)

0

b)

2

c)

4

d)

9

16.

Complete the following calculations. Round off your answers as needed.

52.6 g + 309.1 g +77.214 g

a)

438.9

b)

438.914

c)

438.91

d)

4.38914 x 102

17.
Calculate 1.23 m x 0.89 m and give your answer with the correct number of significant figures.
a)
1.0 m2
b)
1.1 m2
c)
1.0947 m2
d)
1.095 m2
18.
Calculate 7.987 m - 0.54 m and give your answer with the correct number of significant figures.
a)
7.45 m
b)
7.447 m
c)
7.4 m
d)
7.5 m
19.

Calculate 2.998 x 108 m/s ÷ 4.50 x 10-9 m and give your answer with the correct number of significant figures.

a)

1.35 s-1

b)

6.66 x 1016 s-1

c)

6.66 x 10-2 s-1

d)

1.35 x 101 s-1

20.
Gas costs $3.05 a gallon, and your car travels at 27 miles for each gallon of gas. How far can you travel in your car with $95 in your pocket?
a)
11 miles
b)
840 miles
c)
7800 miles
d)
870 miles
21.

Varia is studying abroad in Europe. She is required pay $3,500 (in US dollars) per year to the university, however, she must pay in euros. How many euros can Varia expect to pay per month to the university? (Round to the nearest whole euro.)

0.7306 euros = 1 US dollar

a)

312 Euros

b)

123 Euros

c)

213 Euros

d)

321 Euros

22.
Ann Proctor won the 2007 World Waterski Racing Championship race in her category when she finished the 88-kilometer course in 51.23 minutes. What was her average speed in miles per hour? (Hint: 1 km= 0.62 miles) 
a)
23.66 mph
b)
63.90 mph
c)
46.59 mph
d)
51.23 mph
23.

When solving problems using dimensional, the number of significant figures a conversion factor has is...

a)

variable

b)

zero

c)

three

d)

infinite

24.

The moon is 250,000 miles from earth. How many feet is that?

a)

47, 348 ft.

b)

47 ft.

c)

1.32 X 109 ft.

d)

1.3 X 109 ft.

25.

A family pool holds 10,000.0 gallons of water. How many cubic meters (m3) is this?

a)

37,900.0 cm3

b)

37,900.0 m3

c)

37,900 m3

d)

40,000.0 m3

26.

Santa Maria has an elevation of 6.30 X 105 mm. How many Mm is this elevation?

a)

6.30 X 102 Mm

b)

6.3 X 10-2 Mm

c)

0.00063 Mm

d)

0.000630 Mm

27.

Because our goal in life is to make other people better, you get paid $5.00 every time you do something nice for someone else. You do a minimum of 25 nice things everyday for 1 year. How much money would you make a year?

a)

$45, 625

b)

$21,820

c)

$31,826

d)

$45,900

28.
When using dimensional analysis, the conversion  fact has to equal _____.
a)
100
b)
0.01%
c)
multiples of 10
d)
1
29.

How many minutes are in 1.000 year? Express in Scientific Notation. Assume no leap year

a)

5.256 x 106 min

b)

5.256 x 105 min

c)

5.256 x 104 min

d)

5.256 x 103 min

30.
Which of the following is a sign that a chemical reaction has occurred?
a)
change in shape
b)
melting
c)
formation of a gas
d)
dissolving
31.
Which of the following is NOT an example of a physical change?
a)
crumpled paper
b)
pencil sharpening
c)
shrunken clothing
d)
sour milk
32.
Which is an example of a physical property?
a)
ability to react with acid
b)
 state of matter
c)
flammability
d)
ability to react with oxygen
33.
Which of the following is a chemical change?
a)
human digestion
b)
cutting a tree down
c)
melting a chocolate bar
d)
Has a density of 1 gm/mL
34.

Is it an element, compound, homogeneous or heterogeneous mixture? water

a)

element

b)

compound

c)

homogeneous mixture

d)

heterogeneous mixture

35.

Is it an element, compound, homogeneous or heterogeneous mixture? vinegar

a)

element

b)

compound

c)

homogeneous mixture

d)

heterogeneous mixture

36.

Is it an element, compound, homogeneous or heterogeneous mixture? mint chocolate chip ice cream

a)

element

b)

compound

c)

homogeneous mixture

d)

heterogeneous mixture

37.

Which statement is accurate regarding subatomic particles?

a)

electrons are located in an 'electron cloud' with a mass of 1 amu

b)

protons have a positive charge with a mass of 1 amu and neutrons are neutral with negligible mass

c)

protons have a neutral charge with a mass of 1 amu and neutrons have a positive charge with a mass of 1 amu

d)

protons have a positive charge with a mass of 1 amu and neutrons are neutral with the same mass as a proton

38.

Which of the following is a conclusion of Rutherford's gold foil experiment?

a)

The nucleus is negatively charged

b)

The atom is dense solid and is indivisible

c)

The existence of the electron

d)

The nucleus is very small and the atom is mostly empty space

39.

Dalton theorized that atoms were indivisible. Thomson's findings contradicted this because

a)

Thompson theorized that atoms of the same element are identical

b)

Thomson claimed that atoms of different elements could combine chemically to form new compounds

c)

Thomson discovered the electron, proving that subatomic particles exist

d)

Thompson found that atoms of one element cannot become another element

40.

Which atom has a nucleus that contains 13 protons and 14 neutrons?

a)

Mg

b)

Be

c)

Al

d)

N

41.

In the modern periodic table elements are arranged in order of increasing

a)

mass number

b)

atomic number

c)

oxidation number

d)

valence electron number

42.

Potassium is classified as

a)

an alkali metal

b)

an alkaline earth metal

c)

a halogen

d)

a noble gas

43.

On the periodic table, Periods are

a)

Horizontal rows

b)

Vertical columns

44.

In order to determine the number of neutrons

a)

it is always equal to number of protons

b)

it is always equal to number of electrons

c)

atomic mass minus atomic number

d)

subtract electrons from atomic number

45.

Atoms are most stable when they have

a)

one valence electron

b)

two valence electrons

c)

four valence electrons

d)

eight valence electrons

46.
What scientist first developed 5 rules for atomic theory, and helped kick start modern chemistry?
a)
J.J. Tomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
47.

What is the standard unit of mass at the atomic level?

a)

centigrams

b)

milligrams

c)

amu

d)

nanograms

48.
Most of the mass in an atom is made up of _____________________?
a)
protons and electrons
b)
protons and neutrons
c)
neutrons and electrons
d)
electrons and quarks
49.
What is the electrical charge of a proton?
a)
1+
b)
1-
c)
neutral
d)
2-
50.
How many neutrons does a neutral atom of Barium-137 have?
a)
56
b)
137
c)
81
d)
94
51.
How many protons does Fluorine-19 have?
a)
19
b)
9
c)
10
d)
18
52.
How many electrons does Chlorine have when it becomes an ion?
a)
16
b)
17
c)
18
d)
19
53.
What is the difference between Carbon-12 and Carbon-13?
a)
Carbon-13 has more neutrons.
b)
Carbon-13 has more protons.
c)
Carbon-13 has more electrons.
d)
Carbon-13 has less protons.
54.
What is the mass number of Sodium-23?
a)
23
b)
22.99
c)
11
d)
1
55.
What is the correct isotope symbol for an element that has 8 protons and 9 neutrons?
a)
8O
b)
17O
c)
17F
d)
9F
56.
What is the atomic number of Boron?
a)
5
b)
10.81
c)
11
d)
6
57.
What group has 7 valence electrons?
a)
Alkali Metals
b)
Alkaline Earth Metals
c)
Halogens
d)
Noble Gases
58.

Which has more neutrons: Carbon-13, Nitrogen-14 or Fluorine-16?

a)

Fluorine-16

b)

Carbon-13

c)

Nitrogen-14

d)

All have the same number of neutrons.

59.

What is similar between the elements in the same group?

a)

They have the same atomic mass.

b)

They have the same energy levels.

c)

They have the same number of valence electrons.

d)

They have the same number of protons

60.
If an element has 14 protons, 15 neutrons, and 14 electrons, what is that elements atomic mass
a)
28
b)
14
c)
29
61.

What are the elements in group 2 of the periodic table called?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

62.

What are the elements in group 8A of the periodic table called?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

63.

What are the elements in groups 3-12 of the periodic table called?

a)

Transition metals

b)

Non-metals

c)

Metalloids

d)

Metals

64.

Hydrogen is a:

a)

Alkali metal

b)

Metalloid

c)

Non-metal

d)

Noble gas

65.

What is the Law of Conservation of Mass?

a)

It states that no matter can be created nor destroyed.

b)

It states that energy can not be created nor destroyed.

c)

It states that matter can be created or destroyed during a chemical reaction

d)

It states that energy can be created or destroyed.

66.
How many elements are in C6H12O6?
a)
1
b)
2
c)
3
d)
4
67.

Balance this equation

_Al +_HCl --> _H2 +_AlCl3

a)

2,6,3,2

b)

it's already balanced

c)

4,12,3,4

d)

2,1,4,5

68.

How many Hydrogen are in 4 H2O?

a)

6

b)

8

c)

2

d)

4

69.

Balance this equation and identify the type of reaction:

_N2 + _H2 --> _NH3

a)

1,2,3, Combination

b)

1,3,2, Combination

c)

1,2,3 Decomposition

d)

2,1,1 Combination

70.
What is the percent composition by mass of oxygen in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
71.
Find the percent composition of Cu2S?
a)
%Cu= 67.987 %S= 32.013
b)
%Cu= 79.854   %S= 20.145
c)
%Cu= 35.946   %S= 64.054
72.
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
73.

Which of the following is (are) empirical formula (s)? Check all that apply

a)

CH3COOH

b)

C6H12O6

c)

H2O

d)

Na2SO4

e)

C2H8O2

74.

An organic compound, containing only the elements carbon, hydrogen, and oxygen, was found to contain 54.5% C, 9.1% H by mass, the remainder being oxygen. Determine the empirical formula of the compound.

a)

C3H8O3

b)

CH4O

c)

C2H4O

d)

C4H8O4

75.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
76.
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
77.
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 
78.

Glycerol has a molar mass of 155 g/mol. Its percent composition is: 38.7% C, 9.7% H, and 51.6% O. What is the molecular formula for glycerol?

a)

C4H12O2

b)

CH2O

c)

C5H15O5

d)

CH3O

79.

What is the mass of one mole of H2O?

a)

6.02 x 1023 g

b)

18.02 x 1023 g

c)

18.02 g

d)

15.99999 g

80.

How many atoms are in 1 mole of NaCl?

a)

6.02 x 1023

b)

58

c)

1.20 x 1024

d)

2

81.

How many molecules are there in 31.8 moles of water?

a)

5.28 x 10-23 molecules

b)

1.91 x 1025 molecules

c)

5.28x 10-25 molecules

d)

1.91 x 1023 molecules

82.

How many moles are in 8.30 X 1023 molecules of H2O?

a)

1.38 X 1023 moles H2O

b)

1.38 moles H2O

c)

2 moles H2O

d)

1 mole H2O

83.

How many moles there are in 5.68 x 1024 formula units of AlCl3?

a)

3.42 x 1024 moles

b)

9.44 x 1024 moles

c)

9.44 moles

d)

3.42 moles

84.

How many moles are in 4.5 x 1024 atoms of lithium?

a)

2.71 x 1048 particles

b)

7.47 moles

c)

7.47 x 1024 atoms

d)

2.71 moles

85.

Calculate the number of moles of carbon dioxide contained in 11g of CO2.

a)

0.25

b)

0.5

c)

11

d)

44

86.
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
87.
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
88.
4NH3 + 5O2-->4NO + 6H2O
What is the total number of moles of NO produced when 1 mole of O2 is completely consumed?
a)
1
b)
1.2
c)
0.8
d)
4
89.
How many atoms are in 3.5 moles of arsenic atoms?
a)
5.8 x 10-24
b)
7.5 x 101
c)
2.1 x 1024
d)
1.7 x 1023
90.

4.60 g of H2O contains how many oxygen and how many hydrogen atoms?

a)

6.02 x 1023 molecules

b)

1.54 x 1023 O atoms and 3.07 x 1023 H atoms

c)

1.54 x 1023 O atoms and 1.54 x 1023 H atoms

d)

2.77 X 1024 O atoms and 5.54 x1024 H atoms

91.

What is the molar mass of Sucrose (C12H22O11)?

a)

182.00 g

b)

45.00 g

c)

342.34 g

d)

377.85 g

92.
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
93.

Four students tried to balance the following Reaction:


Mg + Fe2O3 → MgO + Fe


Which student is correct?

a)

3Mg + Fe2O3 → 3MgO + 2Fe

b)

Mg + Fe2O3 → MgO3+ Fe2

c)

2Mg + Fe2O2 → 2MgO + 2Fe

d)

3Mg + 2Fe2O3 → 3MgO + 2Fe

94.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
95.
1)  How many moles of CO2 are in 88.0 grams?
a)
a. 2.00 mol
b)
b. 3.14 mol
c)
c. 0.500 mol
d)
d. 7.63 mol
96.
O2 + CS2 --> CO2 + SO2
What coefficient would go in front of the O2?
a)
1
b)
2
c)
3
d)
4
97.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
98.
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
99.
Cl2 + 2 KBr → Br2 + 2 KCl
How many grams of potassium chloride can be produced from 356 g of chlorine and 356 g of potassium bromide?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
100.

CH4 + 2 O2 → CO2 + 2 H2O

How many moles of carbon dioxide are produced from the combustion of 110. g of CH4?

a)

13.7 mol

b)

2.75 mol

c)

6.11 mol

d)

6.85 mol

101.
Fe (s) + S (l) --> FeS (s)  

In the experiment above, 7.62 g of Fe are allowed to react with 8.67 g of S.
How much FeS is formed?
a)
14.8 g
b)
12.2 g
c)
13.7 g
d)
19.9 g
102.
Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.
 
Mg +  2HCl --> MgCl2  +  H2   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
103.
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
104.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
124 g O2
105.
What is the measured amount of a product obtained from a chemical reaction?
a)
mole ratio
b)
theoretical yield
c)
percentage yield
d)
actual yield
106.
Name the given compound - Fe2(CO3)3
a)
iron (II) carbonate
b)
Iron (III) carbonate
c)
Iron carbonate
d)
Iron carbonate (II)
107.
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
108.

In a lab, a scientist calculate he should produce 12.3 grams of product in his experiment. When he is finished collecting his product it weighs 10.1 grams. What is his percent yield?

a)

82.1 %

b)

0.82%

c)

10.1 %

d)

1.27 %

109.

CH4 + 2H2O --> CO2 + 4H2

What is the limiting reactant when 20. g CH4 react with 15. g H2O and how many grams of hydrogen gas is produced?

a)

CH4, 10. g H2

b)

H2O, 10. g H2

c)

CO2, 3.4 g H2

d)

H2O, 3.4 g H2

110.

What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?

__Ca + __H2O --> __Ca(OH)2 + __H2

a)
2,1 --> 2,1
b)
1,2 --> 1,1
c)
1,2 --> 2,4
d)
1,2 --> 2,1
111.

What are the coefficients for the balanced chemical equation for the complete combustion of butane, C4H10?

a)

1, 13, 4, 5

b)

2, 13, 4, 5

c)

2, 13, 8, 10

d)

1, 8, 4, 5

112.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__AgNO3 + __H2S --> __Ag2S+ __HNO3
a)
2,1 --> 1,2
b)
1,2 --> 1,1
c)
1,2 --> 1,2
d)
1,2 --> 2,1
113.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__MnO2 + __HCl --> __MnCl2 + __H2O __Cl2
a)
4,1 --> 2,1,2
b)
1,2 --> 1,1,4
c)
1,4 --> 1,2,1
d)
1,4 --> 2,2,1
114.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__FeCl3 + __Ca(OH)2 --> __Fe(OH)3 + __CaCl2
a)
4,3--> 2,1
b)
3,2 --> 3,1
c)
2,3 --> 2,2
d)
2,3 --> 2,3
115.
Number of H in 3(NH₄)₂CrO₄
a)
4
b)
6
c)
8
d)
24
116.

What is the mass of 5.22 x 1026 molecules of sodium nitrate?

a)

8.67 x102 g

b)

7.37 x104 g

c)

3.21 x 104 g

d)

4.44 x1028 g

117.
How many atoms of carbon (C) are in C6H12O6?
a)
3
b)
6
c)
12
d)
24
118.
How many O's are in Al₂(SO₄)₃
a)
4
b)
12
c)
7
d)
24
119.
What is the total number of atoms present in 5Na3PO4
a)
5
b)
40
c)
55
d)
8

Similar Resources on Wayground

Element Symbols 1-118

118 questions

Element Symbols 1-118

quiz

Worksheet

•

7th Grade - University

Unit 2 Test REVIEW

118 questions

Unit 2 Test REVIEW

quiz

Worksheet

•

9th - 12th Grade

7.5 Molecular Geometry Bank

122 questions

7.5 Molecular Geometry Bank

quiz

Worksheet

•

10th - 12th Grade

PS Unit 3 Review

115 questions

PS Unit 3 Review

quiz

Worksheet

•

10th Grade

2025 Midterm Exam Review

115 questions

2025 Midterm Exam Review

quiz

Worksheet

•

9th - 11th Grade

Stoichiometry

114 questions

Stoichiometry

quiz

Worksheet

•

10th - 12th Grade

HPS Unit 5 & 6 Test

122 questions

HPS Unit 5 & 6 Test

quiz

Worksheet

•

9th - 12th Grade

Structure of the Atom (Chapter 4)

124 questions

Structure of the Atom (Chapter 4)

quiz

Worksheet

•

10th - 12th Grade