WorksheetsFinal Exam Review
Total questions: 32
Worksheet time: 2hrs 4mins
Name
Class
Date
1.
In which of the following molecules will hydrogen bonding NOT occur?
a)
H2O
b)
HF
c)
NH3
d)
HCl
2.
In order for the reaction
2Al (s) + 6HCl(aq) --> 2AlCl3(aq) + 3H2(g) to occur, which of the following must be true ?
2Al (s) + 6HCl(aq) --> 2AlCl3(aq) + 3H2(g) to occur, which of the following must be true ?
a)
Al must be above Cl on the activity series.
b)
Al must be above H on the activity series.
c)
Heat must be supplied for the reaction.
d)
Al must be an acid.
3.
Double bonds are _________ and ___________ than single bonds.
a)
longer and stronger
b)
longer and weaker
c)
shorter and weaker
d)
shorter and stronger
4.
If you want to produce 35.4 g of zinc chloride, what mass of zinc do you need to react according to the equation
Zn + 2 HCl --> ZnCl2 + H2?
Zn + 2 HCl --> ZnCl2 + H2?
a)
17.0 g Zn
b)
4.00 g Zn
c)
35.4 g Zn
d)
54.3 g Zn
5.
What intermolecular forces (IMFs) would occur in the following molecule
a)
London Dispersion Forces only.
b)
LDF and dipole-dipole interactions.
c)
LDF, dipole-dipole, and hydrogen bonding.
d)
dipole-dipole only
6.
Given the equation
2Mg(s) + O2(g) --> 2MgO(s) + 72.3 kJ, if the reaction began with 20.0 g of Mg, how many kJ of heat would be produced?
2Mg(s) + O2(g) --> 2MgO(s) + 72.3 kJ, if the reaction began with 20.0 g of Mg, how many kJ of heat would be produced?
a)
72.3 kJ
b)
36.2 kJ
c)
144.6 kJ
d)
29.7 kJ
7.
A chemical reaction in the laboratory that absorbs heat from its surroundings into the system and feels cold to the touch is considered to be _________________.
a)
exothermic
b)
endothermic
c)
hyperthermic
d)
ectothermic
8.
Which molecule would have the lowest melting point?
a)
H2O
b)
HCl
c)
CCl4
d)
They are all the same.
9.
The melting point and boiling point of water is significantly higher than other small molecules of comparable mass (ex. Ammonia and methane) because of the__________________.
a)
small size of water molecules.
b)
covalent bonds in water molecules.
c)
low mass of water molecules.
d)
hydrogen bonding between water molecules.
10.
Which statement correctly describes why the freezing of water is an exothermic reaction?
a)
Water molecules (the system) lose energy to its surroundings.
b)
Water molecules (the system) absorb energy from the surroundings.
c)
Water molecules (the system) speed up and lose kinetic energy.
d)
Water molecule (the system) slow down and gain kinetic energy.
11.
In a voltaic cell, ______________ occurs at the anode and ________________ occurs at the cathode.
a)
reduction; oxidation
b)
everything;nothing
c)
oxidation;reduction
d)
none of these
12.
Given the equation 2Mg(s) + O2(g) --> 2MgO(s) + 72.3 kJ, which of the following is true?
a)
The reaction is endothermic because heat is a product.
b)
ΔH = -72.3 kJ
c)
ΔH = +72.3 kJ
d)
The reaction absorbs heat.
13.
What is the percentage of aluminum in Al2(SO4)3?
a)
28.1%
b)
54.0%
c)
15.8%
d)
56.7%
14.
Predict the products of the following single replacement reaction:
Ag + CuCl2 --> ?????
Ag + CuCl2 --> ?????
a)
Cu + AgCl
b)
Cu + AgCl3
c)
Ag + Cu + Cl
d)
no reaction
15.
How many grams of SO2 are in a 0.65 mole sample of SO2?
a)
32 g
b)
16 g
c)
42 g
d)
64 g
16.
A heating curve gives information on:
a)
plasma and gases.
b)
Termperature at which a substance exists at a solid, liquid and gas.
c)
Volumes of liquids and solids.
d)
Mass changes of solids, liquids and gases.
17.
According to the diagram above, the boiling point of this substance is at:
a)
30 degrees Celsius
b)
100 degrees Celsius
c)
70 degrees Celsius
d)
125 degrees Celsius
18.
On line segment R, the substance exists in which state of matter?
a)
solid
b)
solid and liquid
c)
liquid
d)
liquid and gas
19.
On line segment U, the substance exists in which state of matter?
a)
solid
b)
liquid
c)
gas
d)
liquid and gas
20.
1.00 grams of water (specific heat is 4.18 J/g ̊C) and 1.00 grams of aluminum (specific heat 0is 0.902 J/g ̊C) are heated at the same time. Which of the following is true:
a)
The water will heat up faster because it has a higher specific heat.
b)
The aluminum will heat up faster because it has a lower specific heat.
c)
The water and the aluminum are heat up at the same time.
d)
You cannot tell from the information given.
21.
Which of the following molecules are polar?
a)
Cl2
b)
CH4
c)
CO2
d)
NH3
22.
Which state of matter has the strongest IMFs (intermolecular forces) at room temperature?
a)
solids
b)
liquids
c)
gases
d)
They are all the same.
23.
According to Le Châtelier’s Principle, removing O2 to the following reaction, 2Mg(s) + O2(g) <--> 2MgO(s) + 72.3 kJ, will push the reaction towards the:
a)
products
b)
reactants
c)
catalyst
d)
It will have no effect.
24.
According to Le Châtelier’s Principle, adding heat to the following reaction, 2Mg(s) + O2(g) <--> 2MgO(s) + 72.3 kJ, will push the reaction towards the:
a)
reactants
b)
products
c)
catalyst
d)
it will have no effect.
25.
An increase in intermolecular forces causes increases in which of the following:
a)
Boiling point
b)
Surface Tension
c)
Viscosity
d)
All of the above
26.
2 Fe(NO3)3 + 3 Ba(OH)2 -->
2 Fe(OH)3 + 3 Ba(NO3)2 If you want to produce 86.5 g of iron (III) hydroxide, what mass of barium hydroxide do you need to react?
2 Fe(OH)3 + 3 Ba(NO3)2 If you want to produce 86.5 g of iron (III) hydroxide, what mass of barium hydroxide do you need to react?
a)
208 g Ba(OH)2
b)
171 g Ba(OH)2
c)
107 g Ba(OH)2
d)
307 Ba(OH)2
27.
Which statement best explains why chlorine is a gas at room temperature and iodine is a solid at room temperature?
a)
Chlorine has stronger London Disperson Forces than iodine.
b)
Chlorine has stronger covalent bonds than iodine.
c)
Iodine has stronger London Dispersion Forces than chlorine.
d)
Iodine has stronger ionic bonds than chlorine.
28.
In a sample with 17.0 grams of water, how many molecules of water are present?
a)
6.0 molecules
b)
5.68 x 1023 molecules
c)
5.68 molecules
d)
6.02 x 1023 molecules
29.
Fill in the blanks. When bonds are broken, energy is ______. When bonds are formed, energy is _______.
a)
released; absorbed
b)
absorbed;released
c)
absorbed;absorbed
d)
released;released
30.
Is the following reaction exothermic or endothermic?
N2 + 2O2 + 34kJ --> 2NO2
N2 + 2O2 + 34kJ --> 2NO2
a)
Exothermic
b)
Endothermic
31.
Does this potential energy diagram represent an exothermic or endothermic reaction?
a)
Exothermic
b)
Endothermic
32.
What compounds are responsible for acid rain?
a)
sulfuric acid and nitric acid
b)
sulfur and nitrogen
c)
sulfur dioxide and nitrogen oxides
d)
Ms. Soloman
100 %
