Download CHEMISTRY SEMESTER 2 FINAL EXAM STUDY GUIDE Acid/Base

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CHEMISTRY SEMESTER 2 FINAL EXAM STUDY GUIDE
Acid/Base, Gases, Thermo, Kinetics, Equilibrium, & Organic
Acids & Bases
o Know how acids and bases react with water.
o Know how to complete reactions involving the
neutralization of an acid and a base.
o Know the general ranges on the pH scale and
how to identify acidic, basic, and neutral
solutions.
Gases
o Know the definition and mathematical formula
for calculating pressure.
o Know the units that air pressure is measured in
(atm, psi, mm Hg, torr, kPa)
o Know that atmospheric pressure at sea level
equals 1 atm, 760 torr (mm Hg), or 14.7 psi.
o Know the five ideal gas assumptions of KMT
and why they explain the behavior of most
gases is terms of expansion, fluidity,
compressibility, and diffusion.
o Know the difference between directly and
inversely proportional.
o Know that the pressure and volume of a gas
are inversely proportional.
o Know how to use Boyle’s Law to solve for the
initial or final pressure or volume of a gas
undergoing change.
o Know how to convert from Celsius to Kelvin
and vice versa.
o Know what absolute zero is.
o Know what STP is.
o Know that the volume and temperature of a
gas are directly proportional.
o Know how to use Charles’ Law to solve for the
initial or final temperature or volume of a gas
undergoing change.
o
Know the Ideal Gas Law equation and know
the correct units needed for each variable.
Know how to use it to solve for pressure,
volume, moles, or temperature.
Thermodynamics
o Know the difference between heat and
temperature. Know the correct units of each.
o Know what enthalpy is and how to use it to
calculate the heat gained or lost in a chemical
reaction.
o Know the difference between an exothermic and
endothermic reaction and how to recognize each
in an energy diagram.
o Know what is meant by specific heat. Know that
its units are J/g°C.
Know how to solve problems of changing
temperature using the heat equation, Q =
mCΔT.
o Know how to solve problems of water cooling
a metal using the modified heat equation.
o
Know how to read a phase change diagram for
water.
Know how to calculate the heat involved in
vaporization/condensation, melting/freezing, and
in heating up solid, liquid, and gas forms of water.
Kinetics
o Know what is meant by the term ratedetermining step.
o Know what activation energy is. Know what a
catalyst is.
o Know the 4 things that affect reaction rates.
o Know how to label an energy diagram.
Equilibrium
o
Know how equilibrium shifts due to changes in
the 4 things that affect reaction rates.
o
Know how to write and use an equilibrium
constant expression.
o
Know how to solve problems involving Ksp
and solubility.
Organic Chemistry
o Know the characteristics, structural
arrangements, and uses of the 3 allotropes of
carbon: graphite, diamond, and fullerenes.
o Know what an isomer is. Know the difference
between structural and geometric isomers.
Know how to identify examples of each.
o
Know how to identify, name, and draw the
following functional groups of organic
molecules:
o alkanes
o alkenes
o alkynes
o aromatic hydrocarbons
o alkyl halides
o amines
o alcohols
o ethers
o aldehydes
o ketones
o carboxylic acids
o esters
Other
o
There may be some questions on some other
topics, like nuclear reactions, and
oxidation/reduction. (Hint hint)
o
Name:______________________________________
Date:______________________ Per. #:_______
o
Know how the specific heat of water compares
to that of most metals.
1. Stoichiometry
Consider the following balanced equation:
Molar Masses:
18.02 g/mol
C3H8(g) + 5 O2(g)  3 CO2(g) + 4 H2O(g)
44.09
32.00
44.01
a) What mass of CO2 is formed when 100. grams of C3H8 react?
b) What volume (at STP) of O2(g) is needed to completely react with 7.55 grams of C3H8?
2. Nomenclature
Identify whether each compound is an Ionic Compound (I), Covalent Compound (C), or Acid (A) and complete
the table.
Name
I/C/A
Cation
Anion
Formula
Cl–
Mg2+
Fe2S3
hydrobromic acid
NH4+
SO42-
aluminum carbonate
HClO3
3. Redox
Consider the following reaction:
2 Mg + O2  2 MgO
Write the half reactions:
The charge is becoming more:
The element is:
So this element is being:
[ positive | negative ]
[ positive | negative ]
[ gaining | losing ] electrons
[ gaining | losing ] electrons
[ oxidized | reduced ]
[ oxidized | reduced ]
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4. Molarity and Dilution
a) What is the volume of a 0.20 M solution with 0.60 mol HCl dissolved?
b) How many grams of NaOH are required to prepare 800 mL of a 1.50 M solution? (MM of NaOH = 40.0
g/mol)
c) A 50 mL sample of 6 M HCl is diluted to a volume of 250 mL. What is the new concentration?
d) What volume of 18.0 M H2SO4 is needed to make 100 mL of a 1.5 M H2SO4 solution?
Gases
5. The Five Assumptions of Kinetic Molecular Theory – For each sentence, choose the correct phrase that
completes it.
a) Gases consist of large numbers of tiny particles that…
 are far apart.
 are close together.
b) Collisions between gas particles and other particles or the walls of a container are…
 inelastic (sticky).
 elastic (bouncy).
c) Gases consist of large numbers of tiny particles that…
 do not move.
 start and stop moving.
 constantly move at high speed.
d) Ideal gas particles…
 are attracted to each other.
 are repulsed by each other.
 have no attractive or repulsive forces between them.
e) The average kinetic energy of gas molecules causes the gas to have
 volume.
 temperature.

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mass.
6. What causes a gas to have a measureable pressure when inside a container?
7. If someone sprays perfume in one corner of a room, why can it be smelled in the far corner within a few
minutes? Discuss the tiny perfume gas particles to explain your answer.
8. The units of temperature in gas law problems must be in Kelvin. Convert the following temperatures to
Kelvin.
a) 0°C
b) 25°C
c) 100°C
d) -273°C
e) -57°C
f) 44°C
9. What does STP mean? What are the values and units for STP?
10. What is meant by the term “absolute zero”? What is the value of absolute zero in °C and in K?
11. Boyle’s Law
a)
If a gas has a pressure of 450 torr when enclosed
in a 4 liter container, what will the new pressure
be if the volume of the container is decreased to 2
liters?
12. Charles’ Law
a)
A sample of argon gas occupies a volume of 950
mL at 25°C. What volume will the gas occupy at
50°C if the pressure remains constant?
b)
What would have to be the new volume of a gas in a
3 liter container with a pressure of 500 torr, if the
pressure changes so that it has a pressure of 750 torr?
b)
An unknown gas fills a balloon to 2 liters at STP.
What will the temperature have to be, in Kelvin, to
drop the balloon to 0.5 liters if pressure remains
constant?
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Date:______________________ Per. #:_______
13. Ideal Gas Law
a)
How many moles of carbon dioxide would
occupy a 10 L container at 303 K and 1.5 atm?
Thermochemistry
14. Using Enthalpy (ΔH)
a)
Using the reaction below, determine the mass of
carbon that must react to produce 700 kJ of heat.
C(s) + O2(g)  CO2(g) + 393.51 kJ
b)
A large cylinder of He gas, such as that used to
inflate balloons, has a volume of 25.0 L at 295K and
5.8 mol. How many atmospheres of pressure are in
such a cylinder?
b)
Using the reaction below, determine the amount of
heat released by the complete reaction of 50 grams of
methane (CH4).
CH4(g) + 2 O2(g)  CO2(g) + 2 H2O(l) + 890.31 kJ
15. The Heat Equation, Q = mCΔT
a)
How much heat is lost by 50 grams of iron if it
cools from 250°C to 25°C? The specific heat of
iron is 0.449 J/gK.
b)
How much heat must be absorbed by a 15 g piece of
calcium metal to raise the temperature from 0°C to
100°C? Use the back of the Heat of Formation
handout to find the specific heat of calcium.
16. The Modified Heat Equation, mCΔT = –mcΔT
a)
b)
If silver has a specific heat of 0.057 Cal/g°C,
What will be the final temperature if 45 g of iron at
what will be the final temperature if 20 g of silver 250°C is placed in 200 g of water at 25°C?
at 300°C is placed in 120 g of water at 15°C?
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17. Heating Curve
Label the diagram below with all of the following terms:
 0°C
 100°C
 liquid water
 solid ice
 water vapor
 ΔHvap = 41 kJ/mol
 ΔHfus = 6 kJ/mol
 C = 4.18 J/g°C
 C = 2.06 J/g°C
 C = 1.87 J/g°C
18. Heat of Phase Changes
a)
How many kilojoules of energy would it take for
25 grams of ice at 260 K to heat up, melt, heat
up, boil, and heat up of steam at 400 K?
b)
How many kilojoules of energy are released when
100 grams of water vapor at 120°C condenses into
liquid water at 30°C?
19. Nuclear Chemistry
a) Consider the isotope 40K+. Find the following:
Number of protons:
Number of neutrons:
Atomic number:
Mass number:
Number of electrons:
Net Charge:
b) 40K can undergo beta decay, electron capture, and positron decay. Write the equations for each of these
nuclear reactions.
Beta decay:
Electron capture:
Positron decay:
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c) After 3.75 × 109 years, only 12.5% of a sample of 40K remains. What is the half-life of 40K?
20. Heat
For water, Cp,ice = 2.06 J/ g·°C, Cp,water = 4.18 J/ g·°C, Cp,steam = 1.87 J/g·°C, ∆Hfus = 6 kJ/mol, ∆Hvap = 41 kJ/mol
50.0 g of water at 0°C is heated to 50°C.
50.0 g of water at 0°C is completely frozen to ice.
This process is [ endothermic | exothermic ] because
This process is [ endothermic | exothermic ] because
energy is [ absorbed by | released from ] the system.
energy is [ absorbed by | released from ] the system.
The temperature [ increases | remains unchanged |
The temperature [ increases | remains unchanged |
decreases]
decreases]
& molecular attractions are
& molecular attractions are
[ strengthened | about the same | weakened ].
[ strengthened | about the same | weakened ].
The value of Q is [ negative | positive ].
The value of Q is [ negative | positive ].
Calculate Q for this process.
Highlight the portion that corresponds to this process:
Highlight the portion that corresponds to this process:
Temp
Temp
Calculate Q for this process.
Heat
21. pH and pOH
Complete the table.
[H+]
[OH–]
Heat
pH
pOH
1.0 × 10-5 M
1.0 × 10–7 M
10
2
1.0 × 10-3 M
6
1
22. Equilibrium
Consider the following equilibrium equation:
H2(g) + I2(g) + 26.5 kJ  2 HI(g)
At equilibrium, which reaction will be favored (forward, reverse, or neither) when
______________________________________ a. extra I2 gas is introduced?
______________________________________ b. a catalyst is introduced?
Acidic/Basic/Neutral
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______________________________________ c. the temperature of the system is lowered?
______________________________________ d. the pressure on the system is increased?
23. Equilibrium Constant, Keq
a)
b)
At equilibrium a 1.0 L vessel contains 20.0 mol
At equilibrium at 2500 K, [HCl] = 0.0625 M and [H2]
of H2, 18.0 mol of CO2, 12.0 mol of H2O, and 5.9 = [Cl2] = 0.0045 M. What is the equilibrium constant
mol of CO at 427°C. What is the equilibrium
at this temp?
constant at this temperature ?
CO2(g) + H2(g)  CO(g) + H2O(g)
H2(g) + Cl2(g)  2 HCl(g)
Will you expect more products or reactants at
equilibrium?
24. Equilibrium Constants
Write the expression for the equilibrium constant for the reactions:
a) Fe3+(aq) + SCN–(aq) FeSCN2+(aq)
b) Fe3O4(s) + 4 H2(g)  3 Fe(s) + 4 H2O(g)
c) Ca(OH)2(s)  Ca2+(aq) + 2 OH– (aq)
25. Le Châtelier’s Principle
a) Given the equilibrium reaction below, indicate the direction of
the shift and the change in concentration of each substance when
each of the following stresses is placed on the system.
2 NO(g) + O2(g) ↔ 2 NO2(g)
Add NO2(g)
_______ _______ _______
Remove NO(g) _______ _______ _______
Add O2(g)
_______ _______ _______
Add Ne(g)
_______ _______ _______
Decrease volume_______ _______ _______
When the temperature of the system is lowered, more NO(g) is
produced. Is the reaction endothermic or exothermic? Why?
b) Given the equilibrium reaction
below, list three stresses that would
produce more SF6(g).
heat + S4(s) + 12 F2(g) ↔ 4 SF6(g)
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Organic Chemistry
26. Complete the following table.
Name
General Formula
Suffix
Example
Alkane
Used as fuels, to make
plastics. Ethene helps fruit
ripen.
Alkene
Used to make plastics,
formerly used as refrigerants
and aerosol propellants
(CFCs).
Able to form H-bonds,
soluble in water, used as
fuel, disinfectant and
cleaning, cosmetics.
Reactive compounds formed
by oxidizing alcohols,
preserving dead tissue, food
flavors.
Polar solvents used in paint
and textile manufacturing,
dissolve polymers, food
flavors.
Alkyl
Halide
Alcohol
Aldehyde
Ketone
Carboxylic
Acids
Esters
27. Name the following organic molecules.
a)
Properties and Uses
Boiling point increases with
# of carbons. Uses as fuels,
waxes, lubricants.
b)
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c)
d)
e)
f)
28. Draw a picture of the following organic compounds.
a) 2-methyl pentane
b) 3-hexene
c) 2,3,3-trichloro butane
d)1-butanol
e) propanal
f) 3-pentanone
29. What is an allotrope? What are the differences between diamond, graphite, and fullerenes? What do they all
have in common?
30. Lewis Structures and Intermolecular Forces
a) Draw the electron dot structures for the following species, and write the number of valence electrons:
C
S2–
P
Mg2+
# Val e–:
# Val e–:
# Val e–:
# Val e–:
b) Draw the Lewis dot structures for the following compounds. Indicate the type of bond between atoms,
whether the molecule is polar or non-polar, and what kind of Inter-molecular Forces are found.
Compound
CO2
NH3
CH4
Lewis Structure
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Non-Polar Covalent or
Polar Covalent Bonds
Non-polar or
Polar Molecules
Inter-Molecular Forces