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Unit 6 Practice Test Energy & Stoichiometry

Total questions: 46

Worksheet time: 2hrs 4mins

Name
Class
Date
1.

Energy that is stored, and can be converted to other forms of energy in the future, is called ___

a)

potential energy

b)

kinetic energy

c)

heat

d)

hidden energy

2.

Chemical energy, due to the position of the particles in a molecule, is a kind of ___

a)

kinetic energy

b)

radiation

c)

thermal energy

d)

potential energy

3.

What type of energy transformation occurs when a piece of wood burns?

a)

Electrical energy is released as radiant energy

b)

Stored chemical energy is released as thermal energy

c)

Mechanical energy is stored as chemical energy

d)

No transformation occurs

4.
Which of the following energy transformations occur when a lamp that is plugged into a wall socket is functioning correctly?
a)
Chemical to light
b)
Electrical to chemical
c)
Electrical to light
d)
Chemical to electrical
5.
According to the Law of Conservation of Energy, energy cannot be _________ or ____________. 
a)
destroyed, destroyed
b)
created, saved
c)
created, destroyed
d)
lost, found
6.
Energy of motion is which type of energy?
a)
Potential
b)
Kinetic
c)
Sound
d)
Gravitational
7.

Complete the following reaction equation so it is balanced:

C2H4 + 3 O2 -->

a)

C2O2 + H4

b)

CO2 + H2O

c)

CO + H

d)

2 CO2 + 2H2O

8.
Incomplete combustion is when there is a limited amount of oxygen.
a)
True
b)
False
9.
What does incomplete combustion produce that complete combustion doesn't?
a)
Carbon monoxide
b)
Water
c)

blue flame

d)
Carbon dioxide
10.
Complete combustion is when there is plenty of oxygen to react with. 
a)
True
b)
False
11.

What are the two PRODUCTS in a complete combustion reaction?

a)

Carbon Dioxide and Water

b)

Carbon Monoxide and Methane

c)

Carbon and Water

d)

Fuel and Oxygen

12.

What are the two REACTANTS in a combustion reactions?

a)

Methane and Carbon Dioxide

b)

Hydrocarbon and Oxygen

c)

Carbon Dioxide and Water

d)

Hydrocarbon and Carbon Dioxide

13.
How many HCl molecules do you need to balance this equation? 
Mg +  __HCl --->  MgCl2 + H2
a)
1
b)
2
c)
3
d)
4
14.

Which of the following shows this reaction correctly balanced? Fe + O2 -> Fe2O3

a)
4Fe + 3O2 -> 2Fe2O3
b)
2 Fe + 3O2 -> Fe2O6
c)
4 Fe + O6 -> 2Fe2O3
d)
None of the options are correctly balanced.
15.
What does the Law of Conservation of Mass state?
a)
Matter cannot be gained or lost in a chemical reaction.
b)
Matter can only be lost in a chemical reaction.
c)
Matter can only be gained in a chemical reaction.
d)
Matter can be gained and lost in a chemical reaction. 
16.

Which of the following is the correct balanced reaction equation for magnesium reacting with oxygen gas to form magnesium oxide?

a)

2Mg + O2→ 2MgO

b)

Mg + O2 → MgO

c)

2Mg + CO2 → 2MgO + C

d)

2Mg + 2O2 → 2MgO

17.

Which of the following is the correct balanced reaction equation for:

Sodium reacts with chlorine gas to produce sodium chloride.

a)

NaCl → Cl + Na

b)

Na + CO2 → NaCO2

c)

2Na + Cl2 → 2NaCl

d)

Na + Cl2 → NaCl

18.

2H2  +   O2  →  2H2O

How many moles of oxygen would be needed to react with 8 moles H2?

a)
2
b)
4
c)
6
d)
8
19.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of MgO to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
20.
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
21.

2Na + 2H2O → 2NaOH + H2 How many grams of hydrogen are produced if you have 120 g of Na and unlimited water?

a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
22.
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
23.
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
24.

Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.   __Mg +  __HCl --> __MgCl2  +  __H2    

a)
Mg
b)

H2

c)

MgCl2

d)
HCl
25.

What is a Limiting Reactant?

a)
speeds up a reaction
b)
what you run out of first
c)
what you have left over
d)
slows down a reaction
26.

What is the molar mass of table salt (NaCl)?

a)

116.89 g/mol

b)

35.45 g/mol

c)

22.99 g/mol

d)

58.44 g/mol

27.

From the reaction: B2H6 + 3O2 -->2 HBO2 + 2 H2O

How many liters of O2 will be needed to burn 36.1 g of B2H6?

B2H6 = 27.68 g/mol

a)

13.8 g O2

b)

22. 4 L of O2

c)

87.6 L O2

d)

41.7 L O2

28.

2Al + 6HCl --> 2AlCl3 + 3H2

Aluminium reacts with hydrochloric acid. How many grams of aluminum are necessary to produce 11 L of hydrogen gas at STP?

a)

13

b)

8.8

c)

0.99

d)

1.0

29.
What is the molar mass of Mg(NO3)2
a)
148.313g/mol
b)
134.306g/mol
c)
54.311g/mol
30.
What is the volume of 2 moles of gas at STP?
a)
22.4 L
b)
44.8 L
c)
11.2 L
d)
2 L
31.

2C2H2 + O2 −-> 2CO2 + H2O

How many liters of carbon dioxide at STP would be produced from 10 L of oxygen at STP?

a)

10.0 L

b)

20.0 L

c)

5010 L

d)

5 L

32.

What is STP?

a)

A medical condition you really don't want

b)

Standard temperature and pressure - 273K, 1 atm

c)

Stoichiometry Time's Painful

d)

Standard Testing Procedure - 100C, high stress

33.

A group of friends gather around a fire to stay warm. This is an example of ________.

a)

conduction

b)

convection

c)

radiation

34.

Near the ceiling of a room the air is warmer. The warm air rises because of ________.

a)

conduction

b)

convection

c)

radiation

35.

A pot is placed directly on a stove. The pot gets hot due to ________.

a)

conduction

b)

convection

c)

radiation

36.

In a lab, you react Na with Cl2 to form NaCl and calculate that you should get 13 g, but you only end up with 12.5 g. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

37.
Another name for a "oxidation-reduction" reaction is
a)
chemical reaction
b)
neutralization reaction
c)
redox reaction
d)
nuclear reaction
38.

A reaction that involves the transfer of electrons.

a)

Precipitation

b)

Acid-Base

c)

Redox

d)

Double replacement

39.

A reaction in which dissolved substances react to form one (or more) solid products.

a)

Precipitation

b)

Acid-Base

c)

Redox

d)

Single Replacement

40.

A reaction in which a hydrogen ion, H+, is transferred from one chemical to another.

a)

Precipitation

b)

Acid-Base

c)

Redox

d)

Single Replacement

41.

The amount of energy required to raise the temperature 1ºC for every gram is called____?

a)

Thermal Energy

b)

Specific Heat

c)

Temperature

d)

Kinetic Energy

42.

If the specific heat of water is 4.18 J/g∙°C, how much heat is required to increase the temperature of 1.25 g of water from 23 °C to 39 °C? (show your work)

a)

-83.6 J

b)

83.6 J

c)

0.209 J

d)

5.23 J

43.
A reaction is performed in a beaker with a temperature probe recording the temperature changes of the reaction.  If the temperature began at 15.0 degrees Celsius and ended at 27.5 degrees Celsius. Is the reaction endothermic or exothermic?
a)
Exothermic
b)
Endothermic
44.

What type of reaction is this?

a)

Exothermic

b)

Endothermic

c)

Energy Producing

d)

No way to tell

45.

Fire is an example of

a)

exothermic reaction

b)

endothermic reaction

c)

none

d)

both

46.

An ice pack in an example of

a)

exothermic

b)

endothermic

c)

both

d)

none

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