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Final Review

Total questions: 103

Worksheet time: 3hrs 5mins

Name
Class
Date
1.

Which of the following is a characteristic of a base?

a)

tastes sour

b)

found mostly in foods

c)

feels slippery

d)

turn litmus paper red

2.

A sour taste is a characteristic of:

a)

acids

b)

bases

c)

neutral

d)

pH scale

3.
If the [H+] of a solution is 1 x 10-2 mol/L the pH is
a)
2
b)
12
c)
-2
d)
1
4.

If the pH of a solution is 5, then [H+] is:

a)

1.0 x 105 M

b)

1.0 x 109 M

c)

5.0 x 101 M

d)

1.0 x 10-5 M

5.

If the pH of a solution is 5.6, then the pOH is:

a)

6.5

b)

12.4

c)

8.4

d)

5.6

6.

The pH and a pOH of a solution will always add up to:

a)

0

b)

7

c)

14

d)

1.0 x 10-14

7.

if the [H+] of a solution is 1.0 x 10-2 mol/L, the pH is

a)

2

b)

-2

c)

1

d)

12

8.
A solution with a [H+] of 9.4 x 10-5 mol/L is said to be
a)
Acidic
b)
Basic
c)
Neutral
d)
negative number, no solution.
9.

If the [H+] of a solution is 6.8 x 10-9 mol/L, then the pH of that solution is:

a)

8.17

b)

8.2

c)

9.99

d)

8.62

10.
Bleach is a strong base, what is the pH level of bleach?
a)
13
b)
14
c)
1
d)
2
11.

What name is given to the long graduated cylinder used in titrations?

a)

Pipette

b)

Tube

c)

Burette

d)

Measuring Cylinder

12.

what is the reading on this graduated cylinder?

a)

4.40mL

b)

3.50mL

c)

3.60mL

d)

4.50mL

13.
Which is the stronger acid?
a)
pH 1
b)
pH 4
c)
pH 8
d)
pH 13
14.

30mL of NaOH is neutralized by 12.3mL of 0.2M HCl. What is the concentration of the NaOH.

a)

82 mol/l

b)

0.82 mol/l

c)

0.49 mol/l

d)

0.082 mol/l

15.

If it takes 50 mL of 0.5 M Ca(OH)2 to neutralize 125 mL of hydrochloric acid (HCl), what is the concentration of the acid?

a)

0.2 M

b)

5 M

c)

0.5 M

d)

0.4 M

16.

Electrons always flow from

a)

cathode to anode

b)

anode to cathode

17.

Electrons are gained at the

a)

anode

b)

cathode

18.

Given their standard reduction potentials, which of the following substances will be oxidized?

Cu2+/Cu = 0.34V

Zn2+/Zn = -0.76V

a)

Cu

b)

Zn

c)

CuSO4

d)

ZnSO4

19.

What occurs to the mass of copper electrode in the following reaction?

Zn/Zn2+ // Cu2+/Cu

a)

increases

b)

decreases

c)

remains the same

20.

What half-reaction occurs at the anode?

Ag+/Ag = 0.80V

Ni2+/Ni = -0.25V

a)

Ag+ + e- →Ag

b)

Ag → Ag+ + e-

c)

Ni2+ + 2e- → Ni

d)

Ni → Ni2+ + 2e-

21.

What would be the theoretical cell potential of the previous electrochemical cell?

Ag+/Ag = 0.80V

Ni2+/Ni = -0.25V

a)

1.05V

b)

-1.05V

c)

0.55V

d)

-0.55V

22.

What is a redox reaction?

a)

A reaction where both reactants get reduced.

b)

A reaction where both reactants get oxidized.

c)

A reaction that involves a transfer of electrons between reactants.

d)

A reaction that involves the combustion of at least one reactant.

23.

What is reduction?

a)

It is the gain of electrons.

b)

It is the loss of electrons.

c)

It is the creation of electrons.

d)

It is the destruction of electrons.

24.

What is oxidation?

a)

It is the gain of electrons.

b)

It is the loss of electrons.

c)

It is the creation of electrons.

d)

It is the destruction of electrons.

25.

What is a reducing agent?

a)

It is the species that gets reduced -- gains electrons.

b)

It is the species that gets oxidized -- loses electrons.

c)

It is the species that creates electrons.

d)

It is the species that destroys electrons.

26.

What is an oxidizing agent?

a)

It is the species that gets reduced -- gains electrons.

b)

It is the species that gets oxidized -- loses electrons.

c)

It is the species that creates electrons.

d)

It is the species that loses electrons.

27.

What is an anode?

a)

It is the electrode where oxidation takes place.

b)

It is the electrode where reduction takes place.

c)

It is an aqueous solution containing an electrode.

d)

It is the salt bridge that connects half-cells.

28.

What is a cathode?

a)

It is the electrode where oxidation takes place.

b)

It is the electrode where reduction takes place.

c)

It is an aqueous solution containing an electrode.

d)

It is the salt bridge that connects half-cells.

29.
The amount of energy required to raise the temperature 1ºC for every kilogram is called____?
a)
Thermal Energy
b)
Specific Heat
c)
Temperature
d)
Kinetic Energy
30.
What unit do you use to measure Thermal Energy?
a)
J/Kg ºC
b)
Kg
c)
ºC
d)
J
31.
What is the symbol for Thermal Energy?
a)
Q
b)
t
c)
m
d)
C
32.
What is the equation to measure change in Thermal Energy?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ∆mct
d)
m=QC
33.
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
34.
Copper, Stainless Steel, Carbon Steel, and Zinc were all heated using the same thermal energy.  What material would be the coolest after being heated?
a)
Copper
b)
Carbon Steel
c)
Zinc
d)
Stainless Steel
35.
A material was cooled from 100ºC to 40ºC.  What is the temperature change?
a)
60ºC
b)
40ºC
c)
-60ºC
d)
-40ºC
36.

20 grams of water are placed in a jar and left standing. Since the water temperature changes from 25°C to 20°C, how much heat energy moves from the water to the surroundings?

a)

418 J

b)

209 J

c)

83 J

d)

4.18 J

37.

The specific heat of copper is 0.39 J/g °C. What is the temperature change when 128 Joules of heat are added to 78 grams?

a)

128°C

b)

0.24°C

c)

30.4 °C

d)

4.21°C

38.

A pot of 2400g of water at a temperature of 25˚C is heated on a stove until the water boils at 100˚C. How much heat energy is needed to boil the water.

a)

133.76 J

b)

43,062.2 J

c)

753,120 J

d)

1,003,200 J

39.
What is the molar mass of sodium?
a)
11
b)
23
c)
45.98
d)
3
40.

What is the molar mass of fluorine gas, F2?

a)

18.998 g/mol

b)

38 g/mol

c)

9 g/mol

d)

18 g/mol

41.
What is the molar mass of table salt (NaCl)?
a)
116.886 g/mol
b)
35.453 g/mol
c)
22.990 g/mol
d)
58.443 g/mol
42.
What is the molar mass of CO2?
a)
12
b)
16
c)
32
d)
44
43.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
44.

Calculate the molar mass of Ba(C2H3O2)2

a)

255.3 g/mol

b)

237.3 g/mol

c)

228.3 g/mol

d)

196.3 g/mol

45.
What is the percent by mass of magnesium in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
46.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
47.

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

48.

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

49.

What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?

a)

C3H8

b)

CH4

c)

C2H2

d)

C4H10

50.
Molarity is measured in
a)
moles per kg
b)
mols per L
c)
moles per kJ
d)
moles per mL
51.
What is the molarity of a solution which contains 22.41 grams of NaCl in 50.0 mL of solution?
a)
0.488 M
b)
7.67 mol
c)
7.67 M
d)
0.00767 M
52.

What is the molarity of a solution made from 325.4g of AlCl3 with enough water to make 500.0 mL?

a)

4.88 g

b)

4.88 M

c)

2.440 M

d)

2.44 M

53.

What is the mass in grams of 5.90 mol C8H18?

a)

.0516 g

b)

19.4 g

c)

674 g

d)

114.232 g/mole

54.

How many moles are in 19.82 g Mg?

a)

1.226 mol Mg

b)

481.7 mol Mg

c)

1.000 mol Mg

d)

0.8155 mol Mg

55.

Determine the molar mass of carbon tetrachloride CCl4?

a)

153.81 g/mole

b)

118.37 g/mole

c)

189.26 g/mole

d)

47.46 g/mole

56.

What is the mass of 2.3456 g moles of W?

a)

431.22 grams

b)

0.012759 grams

c)

78.376 grams

d)

486.01 grams

57.

How many grams are in 0.523 mol of AlPO4?

a)

63.8 g

b)

0.00429 g

c)

233 g

d)

55.4 g

58.

PCl5 + ___ H2O → ___ HCl + H3PO4

a)

4, 5

b)

1, 6

c)

3, 8

d)

2,2

59.

__ Al + __ FeO → Al2O2 + __ Fe

a)

1, 1, 2

b)

2,1,2

c)

2, 2, 2

d)

2,4,2

60.
 Mg  +  ___ HCl  →   MgCl2  +   H2
a)
1
b)
2
c)
3
d)
4
61.
Which side of a chemical equation is the reactant side?
a)
Left (before the yields sign)
b)
Right (after the yields sign)
62.
Which side of a chemical equation os the product side?
a)
Left (before the yields sign)
b)
Right (after the yields sign)
63.

Determine the temperature in Celsius of 2.49 moles of gas contained in a 1.00-L vessel at a pressure of 14.3 atm.

PV =nRT

a)

-266 oC

b)

-203 oC

c)

70.0 oC

d)

343 oC

64.

In the ideal gas law, which variable represents the universal gas constant?

a)

n

b)

R

c)

T

d)

V

65.
Determine the number of moles in a container of gas at STP with a volume of 99.2 L. 
a)
2222.08 moles
b)
4.43 moles
c)
22.4 moles 
d)
76.8 moles
66.

If the pressure exerted by a gas at 25 oC in a volume of 0.044 L is 3.81 atm, how many moles of gas are present? Remember to convert from Celsius to Kelvin

a)

.002766 mole

b)

.0069 mol

c)

2.766 mol

d)

9.887 mol

67.
In order to solve gas law calculations, temperature must be measured in:
a)
Fahrenheit
b)
Celsius
c)
Kelvin
d)
It doesn't matter 
68.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
69.

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)

310 K

70.
Which of the following is described as the basic unit of matter?
a)
Element
b)
Atom
c)
Molecule
d)
Compound
71.
In the atom diagram shown, E is pointing to
a)
An electron
b)
a proton
c)
a neutron
d)
the nucleus
72.

In the atom diagram shown, A is pointing to the darker particles, these are known as

a)

electrons

b)

protons

c)

neutrons

d)

the nucleus

73.

In this chemical equation, the elements in red are the_______.

a)

Products

b)

Reactants

c)

Subscripts

d)

Coefficients

74.

What is the atomic mass of this atom?

a)

1

b)

3

c)

4

d)

7

75.
What is the atomic number of this atom?
a)
4
b)
5
c)
9
d)
none of the above
76.

An ionic bond forms when

a)

valence electrons are shared back and forth (move between) two atoms.

b)

a sea of mobile electrons surround the cations and they then become negativly charged

c)

valence electrons are transferred from one atom to another, forming charged ions that are then pulled together by attraction between opposite charges

d)

none of the above

77.

Covalent bonds form when

a)

the electronegativity difference between two atoms is very large.

b)

electrons are completely transferred between two atoms.

c)

pairs of electrons are shared between two atoms.

d)

ions are held together by opposite charges.

78.
Why type of bond is forming between the atoms in the diagram?
a)
Ionic
b)
Covalent
79.

Using the information provided, determine how many electrons the a Boron atom contains.

a)

2.5

b)

5

c)

6

d)

10.81

80.
What type of bond is forming between oxygen and hydrogen?
a)
Ionic 
b)
Covalent
81.
How many atoms of iodine are in a mole of iodine?
a)
53
b)
63.55g
c)
126.9
d)
6.02 x 1023
82.
What would be the mass of 1.5mol H2O
a)
20
b)
27
c)
32
d)
40
83.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
84.
What can be determined from a balanced chemical equation?
a)
Mole ratio of any two substances in the reaction
b)
Energy released in the reaction.
c)
Electron configuration of all elements in the reaction. 
d)
Mechanism involved in the reaction. 
85.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__CO + __Fe2O3--> __Fe + __CO2
a)
3,1 --> 2,3
b)
3,2 --> 1,1
c)
3,2 --> 2,4
d)
3,2 --> 2,1
86.
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
87.
In an exothermic process the surrounding looses heat. 
a)
True
b)
False
88.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
89.
H2 + Cl2 --> 2 HCl + 1845 kJ
Is this reaction endothermic or exothermic?
a)
Endothermic 
b)
Exothermic
90.
Do the reactants in an exothermic reaction have a higher or lower energy than the products?
a)
Higher
b)
Lower
91.
If the enthalpy ter (ΔH) is negative the reaction is ____.
a)
Endothermic
b)
Exothermic
c)
Neutral
92.
If ΔH is positive, heat would be shown on the _____ side of the thermochemical equation.
a)
Reactant
b)
Product
93.
The diagram represents which type of reaction
a)
endothermic
b)
exothermic
94.
Energy can not be created or destroyed, it can only be transferred refers to the....
a)
law of conservation of energy
b)
law of conservation of mass
c)
life facts
d)
law of conservation of chemistry
95.

The pH of a solution is 2.0. What is the [OH-] concentration?

a)

1x10-12M

b)

12 M

c)

1x10-2M

d)

2 M

96.

What is the [H+] if the pH is 4.0?

a)

1.0 x 10-10 M

b)

1.0 x 10-4 M

c)

1.0 x 10-14 M

d)

1.0 x 10-7 M

97.
What is the oxidation number of Fe in FeO?
a)
+1
b)
-1
c)
+2
d)
-2
98.
What is the oxidation number of O in CO2?
a)
+2
b)
-1
c)
+4
d)
-2
99.
What is the oxidation number of N in NO21- ?
a)
-3
b)
+4
c)
-2
d)
+3
100.
What is oxidation number of Mn in MnO2 ?
a)
0
b)
+2
c)
-2
d)
+4
101.
The sum of all oxidation numbers in a neutral compound is ___.
a)
0
b)
1
c)
-1
d)
depends on the compound
102.
What is the oxidation of C in CH4?
a)
-4
b)
-1
c)
+4
d)
+1
103.
What is the oxidation number of Ca in Ca3N2?
a)
+3
b)
+2
c)
-3
d)
-2

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