wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Semester 2 Overview

Total questions: 108

Worksheet time: 3hrs 52mins

Name
Class
Date
1.

2H2  +   O2  →  2H2O How many moles of oxygen are consumed if 8 moles H2 react?

a)
2
b)
4
c)
6
d)
8
2.
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
3.

2Na + 2H2O → 2NaOH+ H2 How many grams of hydrogen are produced if 120 g of Na are available? (Na = 22.99g/mol)

a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
4.
What is a Limiting Reagent?
a)
speeds up a reaction
b)
what you run out of first
c)
what you have left over
d)
slows down a reaction
5.
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
6.
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
7.
The mass of one mole of substance is called...
a)
molecular mass
b)
mole constant
c)
molar mass
d)
atomic weight
8.

Molarity is measured in _____.

a)

moles per g.

b)

mols per L.

c)

moles per mm.

d)

moles per mL.

9.

When you make a dilution, which of these values remains constant?

a)

The molarity (M)

b)

The total moles of solute

c)

The volume (V)

d)

The concentration

10.

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

11.
The rate of a reaction increases as temperature__________________.
a)
Decreases
b)
Increases
c)
Stays the Same
12.

Identify the reaction type:

C2H6 + O2 --> CO2 + H2O

a)

Double replacement

b)

Synthesis

c)

Acid base

d)

Combustion

13.

Endothermic Reaction

a)

reaction that takes heat from the surroundings

b)

reaction that gives heat to the surroundings

c)

reaction at constant pressure

d)

reaction at a constat speed

14.

Exothermic Reaction

a)

reaction that gives heat to the surroundings

b)

reaction that takes heat from the surroundings

c)

reaction at constant pressure

d)

reaction at a constat speed

15.
Which is the name of the kind of solid substance formed in this figure?  
a)
aqueous 
b)
precipitate
c)
acid
d)
synthesis 
16.
Strong acids and bases...
a)
do not break apart into ions (non-electrolyte)
b)
partially break apart into ions (weak electrolyte)
c)
completely break apart into ions (non-electrolyte)
d)
completely break apart into ions (strong electrolyte)
17.
Which set of coefficients properly balances the reaction below?
_Cu + _H2O →_ CuO3 + _H2
a)
1,3,1,5
b)
2,6,2,6
c)
1,3,1,3
d)
1,2,3,4
18.
Is the reaction below exothermic or endothermic?
CH4 + 2O2 → CO2 + H2O + heat
a)
exothermic
b)
endothermic
19.
The Law of Conservation of Mass states
a)
that matter exists in all states and reacts the same
b)
that matter can only be changed into new substances by introducing a catalyst
c)
that matter exists in the same state throughout any chemical change
d)
that matter cannot be created or destroyed and that the mass of the products must equal the mass of the reactants
20.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
21.
Which phase of matter has the greatest motion and least orderly arrangement?
a)
solid
b)
liquid
c)
gas
22.
Endothermic reactions feel
a)
warm
b)
cold
23.
Define 'Enthalpy'
a)
a) Energy stored in the movement of molecules in a substance
b)
b) The opposite of temperature
c)
c) The temperature of a molecule
d)
d) Energy stored in the chemical bonds in a substance
24.

Consider a chemical reaction A+B-->C. If reactant A runs out before reactant B, the reaction

a)

continues, but more slowly

b)

stops

c)

reverses direction

25.

The reaction:

A + B → C

ΔH = + 25 kJ

is a(n):

a)

Exothermic Reaction

b)

Endothermic Reaction

c)

Neutralization Reaction

d)

Spontaneous Reaction

26.
If 6.0 mol H2 reacts
with 1.5 mol N2
 3H2 + N2 → 2 NH3 
the limiting reagent is:
a)
ammonia
b)
hydrogen
c)
nitrogen
d)
there is no limiting reagent
27.
If a student calculates a theoretical yield of 5.0 g but only collects 3.0 g of product, the % yield of the reaction is:
a)
30 %
b)
20 %
c)
167 %
d)
60 %
28.
Which is true for the reaction:
Y → Z + heat
a)
Endothermic, ΔH < 0 kJ
b)
Endothermic, ΔH > 0 kJ
c)
Exothermic, ΔH < 0 kJ
d)
Exothermic, ΔH > 0 kJ
29.
2 NO + Cl2  → 2NOCl
When 3.0 mol Cl2 reacts with 1. 5 mol NO:
a)
there is no limiting or excess reagent
b)
NO is limiting reagent
c)
Cl2 is limiting reagent
d)
NOCl is the limiting reagent
30.
Calculate the mass (in kg) of water produced from the combustion of 1.0 gallon (3.8 L) of gasoline (C8H18). The  density of gasoline is 0.79 g/mL [Mr C : 12.0; H : 1.0]
a)
3.33 kg
b)
7.12 kg
c)
4.27 kg
d)
6.57 kg
31.

2CO + O2 −-> 2CO2

How many liters of carbon dioxide at STP are produced from 10.0 L of carbon monoxide at STP?

a)

10.0 L

b)

22.4 L

c)

44.8 L

d)

0.045

32.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
33.

How many molecules of benzene (C6H6) are combusted if there are 134.4 liters of carbon dioxide produced at STP?

a)

6.02 x 1023 molecules of benzene

b)

1 mole of benzene

c)

78.1 grams of benzene

d)

22.4 liters of benzene

34.

You react 5.00 moles of iron with excess oxygen and collect 385 grams of iron (III) oxide. What is your % yield?

a)

96.5% yield of iron (III) oxide

b)

399 gram of iron (III) oxide

c)

104% yield of iron (III) oxide

d)

82.4% yield of iron (III) oxide

35.

How many mL of 0.5M HNO3 would be needed to react with 85mL of 0.75M KOH?

a)

127.5mL

b)

0.1275mL

c)

31.9mL

d)

0.031875mL

36.

Molarity is:

a)

moles per liter of solution

b)

written with a unit of M

c)

calculated by dividing the moles of a substance by the liters of solvent

d)

all of the above

37.
With the increase in temperature, the average kinetic energy of the molecules increases, leading to a decrease in number of collisions per unit time.
a)
True
b)
False
38.
More collisions correspond to a: 
a)
Faster reaction rate  
b)
Slower reaction rate
c)
Constant reaction rate 
d)
None of the above
39.

What is the rate of reaction?

a)

How much energy is needed for a reaction to occur.

b)

The energy required to break a bond.

c)

The time it takes for a reaction to occur.

d)

Collision Theory

40.

The correct name for the CO32- ion is

a)

carbon oxide

b)

nitrate

c)

sulphate

d)

carbonate

41.

The insoluble salt barium sulphate has the formula

a)

BaS

b)

BaSO4

c)

Ba4SO2

d)

BaSO2

42.

What is the name of the compound whose formula is CuSO4 ?

a)

Copper sulphate

b)

Copper sulphide

c)

Copper(II) sulphate

d)

Culcium sulphide

43.

The formula for Magnesium hydroxide is

a)

Mg(OH)2

b)

MgO

c)

HMgO

d)

Mg(OH)

44.

The formula for sodium manganate is Na2MnO4. The manganate ion has the formula

a)

MnO4-

b)

MgO42-

c)

MnO42-

d)

MnO2-

45.

Sodium tetraborate is a soluble salt used in laundry products. Its formula is Na2B4O7. The ions present are

a)

Na2+ and B4O7-

b)

B4O7- and Na+

c)

B4O72- and Na+

d)

Na2O7+ and B4-

46.

When magnesium sulphate dissolves in water, the ions formed are

a)

Mg+ and S2-

b)

S2- and Mg2+

c)

SO42- and Mg2+

d)

Mg+ and SO42-

47.

In reactions like the combustion, as shown by the equation CH4 + 2O2 -> CO2 + 2H2O, one key event that must occur in order for the reaction to proceed is

a)

CH4 molecules must dissolve into the oxygen molecules

b)

CO2 molecules must mix with O2 molecules

c)

collisions between CH4 molecules and O2 molecules

d)

CH4 molecules must collide with H2O molecules

48.

An aqueous solution is:

a)

any liquid with another compound dissolved in it.

b)

an ionic compound with water dissolved in it.

c)

water with another compound dissolved in it.

d)

none of the above

49.

In writing the chemical equation for a precipitation reaction, what abbreviation of the physical state must appear with one of the products?

a)

(s)

b)

(g)

c)

(l)

d)

(w)

50.

When some ionic compounds form through reactions in solution, they fall out as a ___

a)

consolidated element

b)

heavy sludge

c)

dense discharge

d)

solid precipitate

51.

Anions are ___

a)

positively charged ions

b)

negatively charged ions

c)

attracted to bar magnets

d)

repelled by bar magnets

52.

Cations are ___

a)

positively charged ions

b)

negatively charged ions

c)

attracted to bar magnets

d)

repelled by bar magnets

53.
What unit do you use to measure Thermal Energy?
a)
J/Kg ºC
b)
Kg
c)
ºC
d)
J
54.
What is the equation to measure change in Thermal Energy?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ∆mct
d)
m=QC
55.
Water has a specific heat of 4184 J/KgºC.  Wood has a specific heat of 1760 J/KgºC.  What material needs more energy to raise the temperature 1ºC
a)
Wood
b)
Water
c)
Both are the same
56.
A material was cooled from 100ºC to 40ºC.  What is the temperature change?
a)
60ºC
b)
40ºC
c)
-60ºC
d)
-40ºC
57.
What does temperature measure?
a)
Heat
b)
ºC
c)
Kinetic Energy
d)
Thermal Energy
58.
The specific heat is the amount of energy needed to raise the temperature one degree Celsius of 1 gram of a substance.
a)
True
b)
False
59.
Using the heat equation, what would the formula look like if we were solving for change in temperature?
a)
Q m = ∆T Cp
b)
Q / (m Cp)  =  ∆T
c)
Q m / Cp  =  ∆T
d)
m c Q  =  ∆T
60.
A high specific heat means...
a)
It heats up quickly with energy added
b)
It requires more energy to change temperature
61.
How many molecules of sugar (C6H12O6) are in a mole?
a)
24 molecules
b)
180 molecules
c)
180 g
d)
6.02 x 1023 molecules
62.
How many grams are in 1.2 x 1024 molecules of CO?
a)
28 grams
b)
56 grams
c)
6.02 grams
d)
1.2 grams
63.
How many atoms of carbon are in 6.00g of carbon?
a)
1.20x1024atoms C
b)
6.02x1023atoms C
c)
3.01x1023atoms C
d)
1.50x1023atoms C
64.
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
65.
How many steps are in a gram to molecule conversion?
a)
1
b)
2
c)
3
d)
4
66.
How many moles are in 19.82 g Mg? 
a)
1.226mol Mg
b)
481.7mol Mg
c)
1.000mol Mg
d)
 0.8156 mol Mg
67.

How many grams are in 0.375 mol KBr

a)

39.1 g

b)

44.6 g

c)

0.003 g

d)

56.5 g

68.
What does Boyle's law relate to?
a)
Temperature and Volume
b)
Volume and Pressure
c)
Temperature and Pressure
69.
What type of relationship is Charles' Law?
a)
Inverse
b)
Direct
c)
Not enough information
d)
#goals
70.
What is the formula for Boyle's Law?
a)
P1V1=P2V2
b)
P1V1/P2V2
c)
P1V2=P2V1
d)
P1/V1=P2/V2
71.
True or False: Gases can be compressed. 
a)
True
b)
False
72.
When Pressure increases then the Volume must...
a)
Increase
b)
decrease
73.
When Volume increases then Pressure must...
a)
Increase
b)
Decrease
74.
Which container will have a lower pressure?
a)
left
b)
right
c)
they both have the same pressure
d)
I don't know
75.
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
76.
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
77.
How do I change from moles to liters?
a)
divide by 22.4
b)
multiple by Avo number
c)
multiply by 22.4
d)
multiply by molar mass
78.
How many liters are in a mole?
a)
6.022x10^23
b)
1
c)
Molar Mass
d)
22.4
79.
In the ideal gas law, _____ represents moles of a gas.
a)
T
b)
V
c)
R
d)
n
80.
What is standard temperature?
a)
0K
b)
0oC
c)
173 K
d)
173.15 K
81.
Which of the following is NOT a value for standard pressure?
a)
101.3 kPa
b)
760 mm Hg
c)
1 atm
d)
1 torr
82.

N2 + 3H2 → 2NH3

How many moles of hydrogen are needed to react with 1.5 moles of nitrogen?

a)

6

b)

4.5

c)

3

d)

1.5

83.
The force of attraction between nonpolar molecules:
a)
Hydrogen Bonding
b)
Dipole - Dipole Forces
c)
LDF
d)
Ionic Forces
84.
The bond formed between atoms of the same element:
a)
nonpolar covalent
b)
polar covalent
c)
ionic bond
d)
hydrogen bond
85.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

86.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

87.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

88.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

89.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

90.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

91.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

92.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

93.

List the strongest to weakest IMFs.

a)

Hydrogen Bond, London Dispersion, Dipole-dipole

b)

London Dispersion, Dipole-dipole,

Hydrogen Bond

c)

Hydrogen Bond, Dipole-dipole, London Dispersion

d)

Dipole-dipole, Hydrogen Bond, London Dispersion

94.

A strong IMF increases

a)

boiling point

b)

solubility

c)

flammability

d)

malleability

95.

Predict the IMF

a)

London Dispersion

b)

Dipole-dipole

c)

Hydrogen Bond

96.

Predict the IMF

a)

London Dispersion

b)

Dipole-dipole

c)

Hydrogen Bond

97.

Predict the IMF

a)

London Dispersion

b)

Dipole-dipole

c)

Hydrogen Bond

98.

Type of intermolecular force present in I2, Br2, and Cl2.

a)

dipole dipole

b)

H-bond

c)

London dispersion

d)

metallic

99.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

100.

Intermolecular forces for: CO2

a)

London dispersion Forces

b)

Dipole dipole

c)

Hydrogen bonding

101.

Water has an unusually high boiling point for a molecular compound because it has

a)

hydrogen bonding

b)

ion-ion attractions

c)

a high density

d)

a large gram formula mass

102.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

103.

Which noble gas should have the highest boiling point? (Hint: Think about how size affects IMFs)

a)

He

b)

Ne

c)

Kr

d)

Xe

104.

Which of the following will NOT have hydrogen bonding?

a)
b)
c)
d)
105.

Which of the following will have the lowest melting point?

a)
b)
c)
d)
106.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

107.
Does HF have hydrogen bonding?
a)
yes
b)
no
108.
A substance capable of hydrogen bonding has a ___________ boiling point than a similar substance that doesn't hydrogen bond.
a)
higher
b)
lower

Similar Resources on Wayground

SAE Practice 1

109 questions

SAE Practice 1

quiz

Worksheet

•

9th - 12th Grade

Quarter 2 Review for final

104 questions

Quarter 2 Review for final

quiz

Worksheet

•

10th Grade

Chemistry Midterm Review

108 questions

Chemistry Midterm Review

quiz

Worksheet

•

10th Grade

Unit 1

104 questions

Unit 1

quiz

Worksheet

•

7th - 10th Grade

Matter | Grade 10

104 questions

Matter | Grade 10

quiz

Worksheet

•

10th Grade

Chemistry pentatlon 2018

107 questions

Chemistry pentatlon 2018

quiz

Worksheet

•

10th - 11th Grade

19.3 Acid-Base Nomenclature

106 questions

19.3 Acid-Base Nomenclature

quiz

Worksheet

•

10th - 12th Grade

Ch. 18 - Chemical Bonds

113 questions

Ch. 18 - Chemical Bonds

quiz

Worksheet

•

7th - 12th Grade