Name: ______________________
Date: _______________________
Period: ______________________
Honors Chemistry Final Review Packet
Directions: Solve the following problems, showing all work and units
1) Calculate each of the following quantities
a. The volume of a gas, in liters, if 1.75 moles has a pressure of 748.6 mmHg at a temperature
of -6 0C.
b. The absolute temperature of the gas at which 3.33 x 10-3 mol occupies 255 mL at 720 torr.
c. The pressure, in kPa of 19.6 grams of Nitrogen in a 6.41 liter flask at 0 0C
d. The pressure in atmospheres if .0467 mol occupies 413 mL at 122 0C
e. The quantity of gas, in moles, if 67.5 L at 54 0C has a pressure of 11.25 kPa.
2) An unknown vapor has a mass of .846 grams, a volume of 3540 mL, a pressure of 100.23 kPa and
a temperature of 100 0C.
a. What is the molar mass of the unknown vapor?
b. The pressure of the vapor is increased to 104.57 kPa, the volume is decreased to 2789 mL
and the mass remains constant. What is the new temperature?
3) Calcium hydride, CaH2, reacts with water to form hydrogen gas and calcium hydroxide
CaH2 + H2O  Ca(OH)2 + H2
a. How many grams of CaH2 are needed to generate hydrogen gas with a volume of 53.5 liters
and a total pressure of 814 mmHg at 21 0C. Vapor pressure of water at 21 0C is 18.62 mmHg.
4) A 3500 mL flask at 17 0C contains a mixture of .31 mol Nitrogen, .25 mol Helium, and .42 mol
Neon.
a. What is the total pressure of the gases
b. What is the partial pressure of each gas?
c. Calculate the new volume at 735 Torr and 12 0C if all the helium was removed
5) A fixed quantity of gas at 45 0C exhibits a pressure of 735 mmHg and occupies a volume of 5220
mL.
a. Calculate the volume the gas will occupy if the pressure is increased to 1.88 atm, while the
temperature is held constant
b. Calculate the pressure the gas will occupy if the temperature is increased to 75 0C while the
volume is held constant.
c. Calculate the volume the gas will occupy if the temperature is increased to 165 0C while the
pressure is held constant.
6) The work done when a gas is compressed in a cylinder is 426 J. During this process there is a
heat transfer of 128 J from the gas to the surroundings.
a. Calculate the energy change for this process
b. Does the system gain or lose heat?
c. Is work being done on or by the system
d. Is there an overall net gain or net loss of energy by the system
7) Suppose a 50.0 g block of silver (specific heat = 0.2350 J/g· C) at 100 C is placed in contact with
a 50.0 g block of iron (specific heat = 0.4494 J/g· C) at 0 C, and the two blocks are insulated
from the rest of the universe. The final temperature of the two blocks.
8) Answer the following questions for the reaction below:
ZnS + O2  ZnO + SO2
∆H = ?
Calculate ∆H for the following reaction
a. Is the overall reaction endothermic or exothermic?
b. Calculate the amount of heat transferred when 25 grams of Zinc Sulfide reacts at a
constant pressure
c. For a given sample of Zinc Sulfide the enthalpy of reaction is 88.8 kJ, how many grams of
Sulfur Dioxide can be produced?
Directions: Show the following problem. Make sure to show ALL work for each step including units.
For the Following Reaction:
CH3OH(g) à CO(g) + H2(g)
ΔH = +90.7 kJ
a)Is this reaction endothermic or exothermic?
b)Calculate the amount of heat transferred when 45.0g of CH3OH(g) is decomposed by this reaction at a
constant pressure
c)For a given sample of CH3OH, the enthalpy change on the reaction is 18.5 kJ. How many grams of
hydrogen are produced?
d)How many kilojoules of heat are released when 27.0g of CO(g) reacts completely with H2(g) to form
CH3OH(g) at a constant pressure.
A gas expands from 267 L to 893 L at a pressure of 3.7 atm. The amount of heat required in this reaction
from the surroundings is 127 J.
1)Does the system gain or lose heat?
2)Is the reaction endothermic or exothermic
3)Is work being done on the system or by the system
4)Is there a net gain or net loss of energy
5)What is the change in energy for the system?
Directions: Write the complete reaction with solubility. Balance the equation. Write the overall net ionic
equation.
1) Elemental Manganese(IV) is reacted with nitrogen gas
2) A solution of magnesium nitrate is combined with a solution of sodium carbonate
3) Fluorine gas is combined with a solution of sodium bromide
4) A solution of copper(II) sulfide is combined with a solution of acetic acid
5) A strip of aluminum metal is immersed in a solution of silver nitrate
6) A solution of nitric acid is combined with a solution barium hydroxide
7) A solution of Tin(IV) nitrate is combined with solid calcium sulfite
Directions:
For the following compounds:
I.
Draw the structure with the proper molecular geometry
II.
List the Bond Angle/s
III.
What is the Electron Domain
IV.
List the proper notation
V.
Identify the hybridization of the central atom
VI.
Identify type of molecular geometry
VII.
Identify if the overall molecule is Polar or Non-Polar
1) PF5
2) OF2
3) BrF44) XeF3+
5) NF3
Identify the intermolecular forces for the following
9) CH2O
10) HCl
11) CF4
12) SF6
13) SF4
14) CHCl3
15) C2H6
16) He
17) SO2
18) KI
19) CH3CHCH2
20) CH3CH2CH2OH
21) C2H6
22) CH3OCH3
23) CH3NH2
Directions: Answer the following questions:
1)
2)
3)
4)
5)
6)
7)
8)
9)
10)
11)
12)
13)
14)
15)
16)
17)
18)
19)
20)
21)
What elements are involved in hydrogen bonding
What determines if a compound has a high vapor pressure?
What is vapor pressure?
Solids have what type of intermolecular forces (strong, moderate, weak)
Liquids have what type of intermolecular forces (strong, moderate, weak)
Gases have what type of intermolecular forces (strong, moderate, weak)
What is the difference between a state function and a non-state function? Give an example of
each.
What is internal energy? How can you change the internal energy of an object?
If you release 100 J of heat from the system to the surroundings, how much heat will be
absorbed by the surroundings (more, less, or same)
Heat is equal to enthalpy at a constant____?
All elements have a standard formation value of _____?
What does the first law of thermodynamics state?
What does enthalpy of reaction mean?
What does Hess’s Law State?
If ∆H is positive the reaction is _____ and if ∆H is negative the reaction is ______?
If ∆E is positive the reaction is _____ and if ∆E is negative the reaction is _______?
Explain the following processes:
a. sublimation
b. evaporation
c. condensation
d. melting
e. freezing
f. vaporization
What is Boyle’s Law? What is the relationship between the variables? What condition is held
constant?
What is Charles’ Law? What is the relationship between the variables? What condition is held
constant?
What is Gay-Lussac’s Law? What is the relationship between the variables? What condition is
held constant?
What is the combined gas law? Why would we use this law? *Hint – what condition is held
constant?*
22) Which of the following statements is correct?
The greater the molecular weight, the lower the b.p
The greater the molecular attraction, the higher the b.p
The greater the molecular attraction, the lower the HV
The smaller the molecular weight, the higher the b.p
23) The hydrocarbon having the lowest boiling point is _____.
C4H10
CH4
C6H6
C2H6
24) The ion not having Octet configuration in the outermost shell is _____.
A)
Sr2+
B)
Fe2+
C)
Mg2+
D)
S2–
25) In an ionic compound, _____.
A) the cation is a metal and the anion is the non-metal
B) the anion is the metal and the cation is the non-metal
C) the negative ion is a metal and the positive ion is the non-metal
D) both elements can be metals.
26)
According to Lewis's theory, a covalent bond is formed by the _____.
A)
transfer of electrons
B)
sharing of electrons
C)
overlap of electrons
D)
donation of electrons
27)
The molecule containing no lone pairs of electrons is _____.
A)
CH4
B)
H2O
C)
HI
D)
PH3
28)
The least electronegative element of the following is _____.
A)
Cs
B)
Ca
C)
F
D)
C
29)
An example of a polar covalent molecule is _____.
A)
CH4
B)
HCl
C)
Br2
D)
N2
30)
The molecule, which is non-polar of the following, is _____.
A)
HCl
B)
H2
C)
CO
D)
NO2
31) The electronegativities of the elements D, E, F and G are 3.8, 3.3, 2.8 and 1.3. The order
decreasing covalent bond character is
A)
EG > DF > DG > DE
B)
DG > EG > DF > DE
C)
DE > DF > EG > DG
D)
DE > DG > DF > EG
of
32)
A)
B)
C)
D)
33)
A)
B)
C)
D)
34)
A)
B)
C)
D)
35)
A)
B)
C)
D)
36)
A)
B)
C)
37)
A)
B)
C)
D)
38)
A)
B)
C)
D)
39)
A)
B)
C)
D)
40)
A)
B)
C)
D
The ionic bond of the following is _____.
Cs–F
N–H
Si–Cl
N–B
The Octet rule is applicable mainly to _____.
16th group elements
first period elements
transition elements
second period elements
Which of the following bonds is not possible?
C=C
C=H
CºC
C=O
Which of the following compounds does not exhibit resonance?
C6H5OH
CO2
H2O
NO2
NNO bond is present in _____.
N2O5
NH4NO3
N2O
In the Lewis structure of XeO2F2, how many lone pairs surround the xenon?
0
1
2
3
The molecule not obeying the octet rule of the following is _____.
SbCl5
PCl3
SiH4
Cl2
A triple bond is present in _____.
NO2
N2
N2H4
N2O4
Which of the following species is trigonal planar?
AlCl3
ZnCl2
Zn
NH3
41)
Which of the following molecules is not linear?
A)
HgBr2
B)
H2O
C)
N2O
D)
SCN42)
Which of the following has the greatest dipole moment?
A)
H2O
B)
H2S
C)
H2Te
D)
H2Se
43)
Which of the following has the smallest dipole moment?
A)
HBr
B)
HCl
C)
HI
D)
HF
44)
Which of the following molecules does not contain an sp2 hybridized carbon atom?
A)
H3C-CH3
B)
H3C-CH=CH2
C)
CH3-CH=CH-CH2OH
D)
CH3CH=O
45)
In which of the following species is C not sp hybridized?
A)
CO
B)
HCOOH
C)
CO2
D)
CN46) How many sigma bonds and pi bonds are there in the molecule below?
A)
B)
C)
D)
4 sigma, 1 pi
5 sigma, 1 pi
4 sigma, 2 pi
1 sigma, 4 pi
47) Both ethylene (C2H4) and benzene (C6H6) contain the C=C bond. The reactivity of ethylene is greater
than that of benzene. For example, ethylene readily reacts with molecular bromine, whereas benzene is
normally quite inert toward molecular bromine and many other compounds. Explain this difference in
reactivity.
A)
Benzene is a liquid and is therefore less reactive than ethylene, which is a gas.
B)
Molecules of greater molecular weight are less reactive than molecules of lower molecular
weight.
C)
The double bonds in benzene are delocalized and thus less reactive than an isolated double
bond such as in ethylene.
D)
Molecules with larger numbers of double bonds are less reactive than molecules with fewer
double bonds.
48)
Which of the following species is not likely to have a tetrahedral shape?
A)
SiBr4
B)
NF4+
C)
SF4
D)
BeCl4249)
Which of the following has a dipole moment?
A)
PCl3
B)
XeF4
C)
PCl5
D)
SF6
50)
What is the hybridization state of arsenic in arsenic pentafluoride (AsF5).
A)
sp
B)
sp2
C)
sp3
D)
sp3d
51)
Which of the following species is nonpolar?
A)
SO3
B)
PF3
C)
F3SiH
D)
Br2CH2
52) The molecule shown below has a dipole moment.
A)
True
B)
False
53) Dipole–dipole interactions are present in _____.
A)
HCl
B)
C6H6
C)
CH4
D)
NaCl
54)
Non-polar atoms and molecules condense due to _____.
A)
ion–dipole interaction
B)
van der Waals forces
C)
polarizability dispersion forces
D)
dipole–dipole attraction
55)
A)
B)
C)
D)
56)
A)
B)
C)
D)
57)
A)
B)
C)
D)
58)
A)
B)
C)
D)
59)
A)
B)
C)
D)
60)
A)
B)
C)
D)
61)
A)
B)
C)
D)
62)
A)
B)
C)
D)
63)
A)
B)
C)
D)
A compound having a permanent dipole moment is _____.
CO2
H2
CH4
CO
Which element can take part in hydrogen bonding?
F
O
N
all of them
An element which does not take part in hydrogen bonding is _____.
F
C
O
N
The hydride having the highest boiling point is _____.
SiH4
GeH4
CH4
SnH4
Only dispersion forces are present in _____.
HF
C6H6
CO
C2H5OH
Ion–ion attractive forces are present in _____.
CS2
CO2
NaCl
CO
A compound which hydrogen bonds is _____.
BeH2
CH4
CH3COOH
C2H6
The correct order of boiling points is _____.
Ne > Xe
CS2 > CO2
PH3 > NH3
H2S >H2O
Define the following term: system.
The part of the universe that is of interest to us.
Heat transfer.
The part of the universe surrounding a reaction.
The universe
64)
Define the following term: surroundings.
A)
The part of the universe that is of interest to us.
B)
Heat transfer.
C)
The part of the universe surrounding the system.
D)
The universe.
65)
Define the following term: thermochemistry.
A)
The study of heat change in chemical reactions
B)
The process of transferring thermal energy from a system to the surroundings.
C)
The process of transferring thermal energy from the surroundings to a system.
D)
The transfer of thermal energy between two bodies that are at different temperatures.
66)
Define the following term: exothermic process.
A)
The study of heat change in chemical reactions
B)
The process of transferring thermal energy from a system to the surroundings.
C)
The process of transferring thermal energy from the surroundings to a system.
D)
The transfer of thermal energy between two bodies that are at different temperatures.
Use the following to answer questions 67-69:
The internal energy of an ideal gas depends only on its temperature. Do a first-law analysis of the
following process. A sample of an ideal gas is allowed to expand at constant temperature against
atmospheric pressure.
67.
Does the gas do work on its surroundings?
A)
Yes
B)
No
C)
Cannot be determined.
68.
Is there heat exchange between the system and the surroundings? If so, in which direction?
A)
No
B)
Yes, heat is absorbed by the system.
C)
Yes, heat is given off by the system.
69.
What is DE for the gas in this process?
A)
Negative
B)
Zero
C)
Positive
70)
The following reaction takes place:
CuSO4 × 5H2O(s) ® CuSO4(s) + 5H2O(g)
Describe the work involved in this reaction. (No calculations are necessary.)
A)
Work is done by the system on the surroundings.
B)
Work is done by the surroundings on the system.
C)
No work is done.
71)
Define the following term: enthalpy.
A)
Heat transfer at constant temperature.
B)
E + PV
C)
Heat flow under all conditions.
D)
Heat transfer at constant volume.
72)
Define the following term: enthalpy of reaction.
A)
The heat transfer from a system to a reaction.
B)
The transfer from a reaction to the surroundings.
C)
The difference between the enthalpies of the products and the enthalpies of the reactants.
D)
The endothermic process of breaking chemical bonds
73) Consider the following data:
Metal
Al
Cu
Mass (g)
10
30
Specific Heat (J/g°C)
0.900
0.285
Temperature (°C)
40
60
these two metals are placed in contact, which of the following will take place?
A)
Heat will flow from Al to Cu because Al has a larger specific heat.
B)
Heat will flow from Cu to Al because Cu has a larger mass.
C)
Heat will flow fro Cu to Al because Cu has a larger heat capacity.
D)
Heat will flow from Cu to Al because Cu is at a higher temperature.
E)
No heat will flow in either direction.
74)
Which of these processes is endothermic?
A.
O2(g) + 2H2(g) —> 2H2O(g)
B.
H2O(g) —> H2O(l)
C.
3O2(g) + 2CH3OH(g) —> 2CO2(g) + 2H2O(g)
D.
H2O(s) —> H2O(l)
75)
ΔH for an endothermic process is __________ while ΔH for an exothermic process is
__________.
A) zero, positive
B) zero, negative
C) positive, zero
D) negative, positive
E) positive, negative
76)
77)
A)
B)
C)
D)
What is the difference between an ionic equation and a molecular equation?
b. An ionic equation is not balanced, while a molecular equation is balanced.
c. A molecular equation represents only molecular compounds, while an ionic
equation represents only ionic compounds.
d. A molecular equation shows spectator ions while an ionic equation does not.
e. An ionic equation shows all compounds dissociated as ions, while a molecular
equation represents all compounds as associated.
Which of the following processes will likely result in a precipitation reaction?
Mixing a NaNO3 solution with a CuSO4 solution.
Mixing a BaCl2 solution with a K2SO4 solution.
Mixing a NaCl solution with a K2SO4 solution.
Mixing a KF solution with a KCl solution.