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Chemistry FINAL REVIEW - Covid-19

Total questions: 86

Worksheet time: 2hrs 13mins

Name
Class
Date
1.

What is the first thing you must do to solve a stoichiometry problem?

a)

Write a Balanced Equation

b)

Panic

c)

cry

d)

Ask for help

2.
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
3.
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
4.
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
5.
You need 2 pieces of bread, 1 tablespoon of peanut butter and 2 tablespoons of jelly to make a sandwich.  If you have 10 pieces of bread, 4 tablespoons of peanut butter and 20 tablespoons of jelly, what is the limiting reactant?
a)
bread
b)
jelly
c)
peanut butter
d)
sandwich
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.
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
8.

A student measures the pressure and volume of an empty water bottle to be 1.4 atm and 2.3 L. She then decreases the pressure to 0.65 atm. What is the new volume?

a)

2.1 L

b)

5.0 L

c)

8.2 L

d)

3.9 L

9.

A sample of hydrogen at 1.5 atm had its pressure decreased to 0.50 atm producing a new volume of 750 mL. What was its original volume?

a)

245 ml

b)

345 ml

c)

123 ml

d)

250.mL

10.

(Charles Law) There are 65 liters of helium in a balloon at 35 K. If the temperature of the balloon is increased to 40 K, what will the new volume of the balloon be?

a)

40 L

b)

70 L

c)

74.3 L

d)

75.9 L

11.
When Pressure increases then the Volume must...
a)
Increase
b)
decrease
12.
When Volume increases then Pressure must...
a)
Increase
b)
Decrease
13.

A scientist records 8 moles of gas. The scientist does not check the pressure of this gas. At t later time the scientist measures the volume of gas to be 150 ml and the new number of moles of gas to be 48 what was the orginal volume of the gas

a)

25 ml

b)

0.39 ml

c)

2.56 ml

d)

2.5 ml

14.
Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure. 
a)
0 K 
b)
107 K 
c)
207 K 
d)
307 K 
15.
Water is the universal solvent since it's:
a)
water
b)
such a small molecule 
c)
polar
d)
essential to life
16.
What is the property of water that allows it to stick to other water molecules?
a)
Capillary Action
b)
Solubility
c)
Adhesion
d)
Cohesion
17.
What two atoms make up water?
a)
Hydrogen and Oxygen
b)
Helium and Oxygen
c)
Sulfur and Arsenic
d)
Uranium and Sodium
18.
What is Surface Tension?
a)
surfactant
b)
the skin-like outside of water
c)
the ability to move upward against gravity
d)
a polar molecule
19.

Describe COHESION.

a)

Water molecules attracted to other substances.

b)

Water molecules climbing upwards against the force of gravity.

c)

Water molecules dissolving many substances because of its polarity.

d)

Water molecules attracted to other water molecules.

20.

Describe ADHESION.

a)

Water molecules attracted to other substances.

b)

Water molecules climbing upwards against the force of gravity.

c)

Water molecules dissolving many substances because of its polarity.

d)

Water molecules attracted to other water molecules.

21.

Describe CAPILLARY ACTION.

a)

Measure of how difficult it is to break the surface of a liquid.

b)

Water molecules climbing up against the force of gravity.

c)

Water molecules attracted to other substances.

d)

Water molecules dissolving many substances because of its polarity.

22.

A water droplet sticking to a glass is an example of...

a)

Cohesion

b)

Adhesion

c)

Surfactant

d)

Meniscus

23.
Which term refers to water having partial positive and a partial negative charge?
a)
cohesion
b)
surface tension
c)
polarity
d)
adhesion
24.
Which of the following is a polar molecule?
a)
CH4
b)
Xe
c)
H2O
d)
CO2
25.

You are given a small beaker of solution at room temp. You add a bit of solute to the solution and it dissolves. The solution was:

a)

saturated

b)

unsaturated

c)

concentrated

d)

warm

26.
__________ are made up of solutes and solvents.
a)
Solutions
b)
Suspension
c)
Colloid
d)
mixtures
27.
When a solution is saturated:
a)
No additional material will dissolve in it
b)
You need to stir it more 
c)
Two materials have combined to create a clear liquid
d)
Crystals form 
28.

How do you know when you have a saturated solution?

a)

You don't see anymore material in the solution. It has dissolved.

b)

The material dissolves and no more will dissolve because you see it collect at the bottom.

c)

The solution is bubbling and cloudy.

d)

The solution is clear and there is nothing at the bottom.

29.
What is a solute?
a)
The substance that does the dissolving in a solution.
b)
The substance that is dissolved into the solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
30.
What is a solvent?
a)
The substance that does the dissolving in a solution.
b)
The substance that is being dissolved in a solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
31.
Water is a universal solvent
a)
true
b)
false
32.
KBr
a)
Soluble
b)
Insoluble
33.
Zinc Hydroxide
a)
Soluble 
b)
Insoluble
34.
Silver Iodide
a)
Soluble 
b)
Insoluble 
35.
CaCO3
a)
soluble
b)
insoluble
36.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
37.
How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?
a)
0.625 g NaCl
b)
625 g NaCl
c)
36.5 g NaCl
d)
0.04 mol NaCl
38.

If 0.775 L of 1.00 M NaOH is diluted to 1.00 L, the resulting solution contains

a)

0.225 mol NaOH

b)

0.775 mol NaOH

c)

1.25 mol NaOH

d)

2.45 mol NaOH

39.

If I dilute 250 mL of 0.10 M lithium acetate solution to a volume of 750 mL, what will the concentration of this solution be?

a)

2 M

b)

0.02 M

c)

0.03 M

d)

0.08 M

40.
A neutralization reaction will (almost) always produce...
a)
water & salt
b)
water
c)
salt
d)
water & carbon
41.
H3PO4 is an example of a ...
a)
acid
b)
base
c)
salt
42.
Identify the salt in the following equation:
Zn(OH)2 + HNO3   ---> H2O  + Zn(NO3)2
a)
Zn(OH)2
b)
HNO3
c)
H2O
d)
Zn(NO3)2
43.

Complete the following reaction:

HCl + Mg(OH)2 -->

a)

MgCl2 + H2O

b)

Mg +H2O

c)

MgCl2 + H2

d)

MgCl2 + H2O + CO2

44.
What is the formula for phosphorous acid?
a)
H3PO4
b)
H2PO4
c)
H3P
d)
H3PO3
45.
What is the formula for Hydrosulfuric Acid?
a)
H2(SO3)
b)
H2S
c)
H2(SO2)
d)
H2(SO4)
46.
What is the formula for Nitric Acid?
a)
HNO2
b)
HNO3
c)
HNO4
d)
H2NO3
47.
Name HF
a)
hydrofluoric acid
b)
Hypofluoric acid
c)
hydrogen fluorine acid
d)
fluoric acid
48.
HNO2
a)
hydronitrogen
b)
hydrogen nitrogen oxygen
c)
nitrous acid
d)
nitric acid
49.
How many sig. fig. are in the number below:
350.540
a)
4
b)
5
c)
6
d)
7
50.
How many sig. fig. are in the number below:
0.0005
a)
1
b)
2
c)
3
d)
4
51.
How many sig figs are there?
0.00400
a)
1
b)
3
c)
5
d)
6
52.
Which value has only 4 significant digits? 
a)
6.930
b)
0.450
c)
8450
d)
0.392
53.
What are the three states of matter?
a)
solid, volume, mass
b)
density, volume, mass
c)
solid, liquid, gas
d)
density, gas, volume
54.
Something that takes up space and has mass.
a)
volume
b)
matter
c)
mass
d)
density
55.
A pure substance containing only one kind of atom.
a)
element
b)
mixture
c)
compound
56.
Physical or Chemical Property?  The temperature of boiling water is 100 degrees Celsius.
a)
Physical
b)
Chemical
c)
Neither
57.
Define a Physical Property
a)
A property of matter not involving in its manifestation a chemical change
b)
A property in which stops a chemical reaction from occuring.
c)
A property or behavior of a substance which undergoes a chemical change or reaction.
d)
A property which makes the object smell or taste different.
58.
Boiling point,melting point, and density are some of an element's
a)
pure properties
b)
physical properties
c)
chemical properties
59.
Is  blood a mixture?
a)
No
b)
Yes
60.
The air around was is  a mixture of gases.
a)
True
b)
False
61.
What does it mean if a mixture is homogeneous?
a)
you can see the different parts
b)
cannot tell one part from another
c)
chunks of particles
d)
made of elements
62.
What does it mean if a mixture is heterogeneous?
a)
you can see the different parts
b)
cannot tell one part from another
c)
very well blended
d)
made of elements
63.

Properties that DO depend on the amount of matter present.

a)

Mass

b)

Hardness

c)

Extensive

d)

Intensive

64.

Properties that depend on the identity of substance.

a)

Mass

b)

Hardness

c)

Extensive

d)

Intensive

65.

Which of the following is an extensive property?

a)

Hardness

b)

Boiling Point

c)

Density

d)

Weight

66.

Which of the following is an intensive property?

a)

Color

b)

Mass

c)

Volume

d)

Weight

67.

Blue color

a)

Physical Property

b)

Chemical Property

68.

Density

a)

Physical Property

b)

Chemical Property

69.

Melting point

a)

Intensive Property

b)

Extensive Property

70.

Color

a)

Intensive Property

b)

Extensive Property

71.
What would be the mass of 1.5mol H2O
a)
20
b)
27
c)
32
d)
40
72.
If I need 20.4 moles of sodium chloride, how much should I weigh out?
a)
0.549 g
b)
112 g
c)
1192 g
d)
5077 g
73.

Record the following in cm

a)

1.0

b)

1.2

c)

1.25

d)

1.250

e)

1.30

74.
What is the measurement using the correct number of sig. figs.?
a)
8.5mL
b)
8.50mL
c)
8.45mL
d)
8.4mL
75.
What is the measurement using the correct number of sig. figs.?
a)
89cm
b)
88.9cm
c)
88.90cm
d)
88cm
76.
Solve. Round using SigFig math rules.
12.5-mL + 20.05-mL + 2.69-mL
a)
35-mL
b)
35.2-mL
c)
35.24-mL
d)
35.240-mL
77.
Solve. Round using SigFig math rules.
98.7°C - 97.25°C 
a)
1°C
b)
1.4°C
c)
1.45°C
d)
1.450°C
78.

1200 light years - 5 light years = ?

a)

1195 light years

b)

2000 light years

c)

1000 light years

d)

1200 light years

79.

67 seconds + 10.1 seconds = ?

a)

77.1

b)

77

c)

70

d)

80

80.
What is the formula for sodium nitrate?
a)
Na3(NO)
b)
Na(NO)
c)
Na3(NO3)
d)
Na(NO3)
81.
What is the formula for copper(I) sulfate?
a)
Cu(SO3)
b)
Cu(SO4)
c)
Cu2(SO3)
d)
Cu2(SO4)
82.
Name this compound: 
KF
a)
Potassium fluoride
b)
Potassium fluorite
c)
Fluorine potasside 
d)
Potassium fluorate
83.
P2O5
a)
Phosphorus Oxide
b)
Pentaphosphorus Dioxide
c)
Diphosphorous pentoxide
d)
Phosphoric Oxygen
84.
CO
a)
Carbon Oxide
b)
Carbon Oxygen
c)
Dicarbon dioxide
d)
Carbon Monoxide
85.
What is the name for FeO
a)
Iron oxide
b)
Iron (I) oxide
c)
Iron (II) oxide 
d)
Iron (III) oxide
86.

The name of  Cu3N2Cu_3N_2 is

a)

copper (III) nitride

b)

copper (II) nitride

c)

copper nitride

d)

tricopper dinitride

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