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Unit 8 & 9 Review (Moles/Rxns)

Total questions: 61

Worksheet time: 3hrs 4mins

Name
Class
Date
1.
Which is the Law of Conservation of Matter?
a)
matter cannot be created or destroyed, it only changes form
b)
matter can be created but it cannot be destroyed, it never changes form
c)
matter can be destroyed but it cannot be created, it usually just changes form
d)
matter is an unproven theory created by Hans Geiger
2.

What are the coefficients that will balance the skeleton equation below?

__Na + __MgF₂ → __NaF + __Mg

a)

2,1,1,2

b)

1,2,1,2,

c)

2, 1, 2, 1

d)

1,2,2,1

3.

What are the coefficients that will balance the skeleton equation below?

__Na + __F₂ → __NaF

a)

1, 2, 1

b)

2, 1, 2

c)

1,1,1

d)

2,2,2

4.

A + B > AB

What type of chemical reaction is this?

a)
single
b)
double
c)
synthesis
d)
decomposition
5.

2Ca + O2 > 2CaO 

What is the 2 located behind oxygen (O) called?

a)
coefficient
b)
reactant
c)
subscript
d)
product
6.
What type of chemical reaction is this one?
Al(OH)3 --> Al2O3  + H2O
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement 
7.
What type of chemical reaction is this one?
CUO + CO2 --> CuCO3
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement 
8.
What type of chemical reaction is this one?
Ca + MgCl2 --> CaCl2 + Mg
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement 
9.
What type of chemical reaction is this one?
C2H2 + O2 --> CO2 + H2O
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement 
10.

What type of chemical reaction is this?

3KOH + H3PO4 --> K3PO4 + 3H2O

a)
Combination
b)
Decomposition
c)
Single replacement
d)
Double replacement
11.

What type of reaction is illustrated below?

Zn + H2S --> ZnS + H2

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

12.
Which of the following is an example of synthesis?
a)
Na + Br2 --> NaBr
b)
KClO3 --> KCl + O2
c)
HgO + Cl2-->HgCl + O2
d)
Cl2 + NaBr --> NaCl + Br2
13.
What is a coefficient?
a)
The small number on the right of the chemical symbol.
b)
The large number to the left of a formula.
14.

Why must chemical equations be balanced?

a)

So that the equation doesn't explode

b)

The reaction won't happen until it is balanced

c)

Based on the Law of Conservation of Matter, matter cannot be created or destroyed.

d)

Based on the Law of Conservation of Energy, energy cannot be created or destroyed.e

15.

Which type of chemical reaction has the following configuration?


Element + Compound --> Element + Compound


A + BC --> B + AC

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

16.

Which type of chemical reaction has the following configuration?


Hydrocarbon + Oxygen --> Carbon Dioxide + Water


CxHy + O2 --> CO2 + H2O

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

17.

What type of chemical reaction has the following configuration?


Compound --> Substance + Substance


AB --> A + B

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

18.
The following is what type of reaction:
PbCl2 + AgNO3 → Pb(NO3)2 + AgCl
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
19.
One reactant into several products.
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
20.
Always starts with a Hydrocarbon that reacts with oxygen and produces carbon dioxide and water. 
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
21.
Two Reactants and One Product
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
22.

If an element is diatomic it should have a subscript of___

a)

1, always

b)

2, only when it is an element

c)

it shouldn't have a subscript, it should have a coefficent

d)

2, when bonded in a compound

23.

How many oxygen atoms are in this chemical formula?

a)

6 oxygen atoms

b)

2 oxygen atoms

c)

3 oxygen atoms

d)

4 oxygen atoms

24.
If a reaction starts with a total 75g of reactants it should produce 
a)
a total of 40g of products
b)
a total of 75g of products
c)
a total of 180 g of products
d)
None of the above
25.
What is the molar mass of Mg3N2?
a)
191.6 g/mol
b)
76.64 g/mol
c)
38.32 g/mol
d)
100.95 g/mol
26.
What is the mass of one mole of Al2(SO4)3?
a)
75.04 g
b)
342.14 g 
c)
75.04 mol
d)
342.14 mol
27.
How many moles of carbon atoms are there in 5g of carbon?
a)
60 mol
b)
17 mol
c)
0.42 mol
d)
7 mol
28.
How many molecules are there in 5.9 moles of NaCl?
a)
3.5x1024molecules
b)
9.79x10-24molecules
c)
1.02x1023molecules
29.
How many molecules are present in 69.0 moles of SrO?
a)
4.16x1025molecules
b)
8.72x1021molecules
c)
7,149.78 molecules
d)
6,893.32 molecules
30.
What is the mole used for? 
a)
To measure the amount of grams in a substance
b)
To measure the amount of atoms or molecules in a substance
c)
To measure the amount of energy in a substance
d)
To measure the amount of bonding in a substance 
31.
What is Avogadro's Number? 
a)
6.02 x 1023
b)
- 6.02 1023
c)
6.02 x 1022
d)
6,020,000,000,000
32.
The molar mass of an element is the mass of one ____ of the element.
a)
atom
b)
molecule
c)
mole
d)
gram
33.
What is the mass of 9.4 moles of B2(Cr2O7)3?
a)
6.41 x 1022g
b)
5.67x1024 g
c)
49.11 g
d)
4,339.23 g
34.

Which of the following statements regarding the mole is INCORRECT?

a)

A mole is a unit of quantity equal to 6.02 x 1023 particles.

b)

The number of particles in a mole is known as Avogadro’s number.

c)

A mole of particles of an element is numerically equal to the atomic mass of the element.

d)

none of the above

35.
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
d)
1.91 x 1022
36.
What is the mole used for? 
a)
To measure the amount of grams in a substance
b)
To measure the amount of atoms or molecules in a substance
c)
To measure the amount of energy in a substance
d)
To measure the amount of bonding in a substance 
37.
What is the molar mass of C6H12O6?
a)

180 g/mol

b)

150 g/mol

c)

220 g/mol

d)

105 g/mol

38.

Which of the following is a diatomic element?

a)

NaF

b)

CO2

c)

N2

d)

H2O

39.

What is the formula for Zinc (II) fluoride?

a)

ZnF2

b)

ZnF

c)

Zn2F

d)

Zn2F4

40.

What is the formula for Potassium hydroxide?

a)

POH

b)

KOH

c)

KHO

d)

PHO

41.

What is the formula for Strontium nitrate?

a)

Sr(NO3)2

b)

SrNO3

c)

Sr2NO3

d)

St(NO3)2

42.

What type of reaction is this?

2 C6H14 + 19 O2 → 12 CO2 + 14 H2O

a)

Single Replacement

b)

Double Replacement

c)

Combustion

d)

Decomposition

43.
Is the following equation balanced?...
Al + O2 --> 2Al2O3
a)
Yes!
b)
No!
44.
How many HCl molecules do you need to balance this equation? 
Mg +  __HCl --->  MgCl2 + H2
a)
1
b)
2
c)
3
d)
4
45.

48.86 g of cobalt is equal to how many moles of cobalt?

a)

2879 moles

b)

8.291 moles

c)

.8291 moles

d)

.829 moles

46.

How many molecules of water are in a 821.3 g sample?

a)

45.58 molecules

b)

8.232 x 1025 molecules

c)

8.909 x 1027 molecules

d)

2.744 x 1025 molecules

47.

How many moles of sodium chloride are in a 321.8 g sample?

a)

18810 moles

b)

3.315 x 1024 moles

c)

5.507 moles

d)

4.767 moles

48.

A solution that contains all of the solute it can hold at a given temperature is

a)

diluted.

b)

saturated.

c)

supersaturated.

d)

unsaturated.

49.

A solution that is able to dissolve additional solute is best described as

a)

supersaturated.

b)

concentrated.

c)

saturated

d)

unsaturated.

50.
The _____is the part that gets dissolved. 
a)
solute 
b)
solvent 
c)
solution 
d)
Sacajawea 
51.
The universal solvent is ______. 
a)
sodium 
b)
acid 
c)
water 
d)
wind 
52.
This is the part of the solution that does the dissolving. 
a)
solute
b)
solvent 
c)
salt water 
d)
First Continental Congress 
53.

If you have 2.5 moles of glucose in 0.5 L of solution, what is the concentration of the solution?

a)

0.5 M

b)

1.25 M

c)

2.5 M

d)

5 M

54.

What is the molarity of 3 mole of hydrochloric acid in 3 L of water. 

Remember, M =  molL\frac{mol}{L}  

a)

3 M

b)

1 M

c)

6 M

d)

9 M

55.

Calculate the molarity of the following solution: 1.0 mole of KCl in 750 mL of solution.  (HINT:  1000 mL = 1 L)

M = molLM\ =\ \frac{mol}{L}  

a)

0.750 M

b)

99 M

c)

1.3 M

d)

2.0 M

56.

If you have 2.5 moles of glucose in 0.5 L of solution, what is the concentration of the solution?

M = molLM\ =\ \frac{mol}{L}  

a)

0.5 M

b)

1.25 M

c)

2.5 M

d)

5 M

57.

What is the molarity of a solution prepared by dissolving 2 moles of sodium chloride (NaCl) in 1 liter of water?

a)

1 M

b)

2 M

c)

0.5 M

d)

4 M

58.

What volume of water (in liters) is required to dissolve 1 mole of sucrose (C 12_{12} H 22_{22} O 11_{11} ) to make a 0.5 M solution?

a)

0.5 L

b)

1 L

c)

2 L

d)

4 L

59.
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
60.
The total number of sodium atoms in 46.0 grams is
a)
3.01 x 1023
b)
6.02 x 1023
c)
12 x 1023
d)
24 x 1023
61.
Which sample of O2 contains a total of 3 x 1023 molecules?
a)
1.0 moles
b)
2.0 moles
c)
16.0 grams
d)
32.0 grams

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