Name:_____________________________Period:_____
Chemistry in the Community Spring Final Review/ 2014
Please do the calculations and answer questions on a separate piece of paper when necessary!
Types of Reactions
1. List the 5 types of reactions and give an example of each.
2. Balance and classify the following chemical reactions:
a. ___AlBr3 + ___K2SO4  ___ KBr + ___Al2(SO4)3
b. ___Ag2O  ___Ag + ___O2
c. ___Fe203 + ___ H20  ___Fe(OH)3
d. ___C2H4 + ___O2  ___CO2 + ___ H2O
e. ___H2SO4 + ___ Mg  ___ MgSO4 + H2
Type
_____________
_____________
_____________
_____________
_____________
Stoichiometry
Matching
1. Reactant
2. Product
3. Limiting Reagent
4. Excess Reagent
5. Subscript
6. Coefficient
7. Theoretical Yield
8. Actual Yield
a. Number placed in front of formula to balance
equation
b. On the right side of equation
c. Reactant left over
d. Small subscript number that indicates the
number of atoms.
e. On the left side of equation
f. Maximum amount of product that can form from
a given amount of reactants
g. the amount of product measured in the lab
9. Practice this Stoichiometric Problem
a. Write the molar mass of each substance above the formula on the reaction above.
b. Write the mole ratio directly underneath each substance.
c. Multiply the coefficients by the molar mass to determine the gram ratio.
Molar Mass
Cu + 2HCl → CuCl2
+
H2
Mole Ratio
Gram Ratio
d.
e.
f.
g.
h.
i.
How many moles of Cu would it take to produce 3.5 moles of CuCl2?
How many moles of HCl would it take to produce 1.3 moles of H2?
How much (g) copper would it take to produce 4.7 moles of CuCl2?
How much H2 (g) is produced when 23.3 g of Cu reacts?
State the law of conservation of mass
Add the gram ratio values of the reactants and compare it to the sum of the gram ratio
values of the product. This calculation “proves” the law of conservation of mass
Petroleum
1. Fractional Distillation.
a. Describe the process- why does it work?
b. Name 5 fractions separated when petroleum is refined.
c. Draw a fractional distillation graph for a mixture containing hexane (Bp=68.7°C)
and Heptane (Bp=98.4°C).
2. What elements compose all hydrocarbons? _____________ and ____________.
3. Write the complete balanced equation for the combustion of propane. Indicate where bonds
are broken and where they are formed.
4. Name the following hydrocarbons
a. C2H6
Write the formulas:
e. Butyne
b. C3H4
c. C5H12
d. C8H16
f. Hexene
g. nonane
h. ethene
5. Draw the structures for e,f,g, and h.
___6. combustion
___7. heat of combustion
___8. saturated
___9. ionic bond
___10. covalent bond
___ 11. unsaturated
___ 12. endothermic
___ 13. exothermic
___14. viscosity
____15. density
a. thermal energy released when a substance burns
b. resistance to flow
c. metal + nonmetal (metal gives up electrons)
e. absorbs energy
f. Nonmetal + nonmetal (share electrons)
g. all Carbon atoms bonded in 4 places
h. releases energy
i. Burning
j. Hydrocarbon that contains a multiple bond
k. mass per volume
16. Use the table below to answer the questions.
Hydrocarbon
Methane
Ethane
Propane
Butane
Hexane
Heptane
Decane
Octane
a.
b.
c.
d.
e.
f.
g.
h.
i.
j.
k.
l.
m.
n.
o.
Boiling point(C)
-161.7
-88.6
-42.1
-0.5
68.7
98.4
174.0
125.7
Hydrocarbon Information
Heat of Combustion
Molar Heat of Combustion
55.6 kJ/g
891 kJ/mol
52.0 kJ/g
1560 kJ/mol
50.0 kJ/g
2200 kJ/mol
49.3 kJ/g
2859 kJ/mol
48.8 kJ/g
3510 kJ/mol
48.2 kJ/g
4141 kJ/mol
48.2 kJ/g
4817 kJ/mol
47.8 kJ/g
5450 kJ/mol
Write the formula of each hydrocarbon next to the name.
What happens to the number of carbons as you look from top to bottom on the table?
What happens to the boiling point as you look from top to bottom on the table?
What happens to the viscosity of the substances as you look from top to bottom?
What substances are gases (have already boiled) at room temperature (22 C)?
What state of matter is hexane at 50C?
What is the molar heat of combustion for propane?
Write the equation for the complete combustion of propane.
Show where the bonds are broken and formed. What kind of energy is stored in the
bonds?
How much energy is produced when 50 moles of propane burns?
How much energy is released when 70g of propane burns?
How much energy is produced when 50 moles of octane burns?
How much energy is released when 70g of octane burns?
Which is a better energy source, propane or octane? Explain your answer.
Determine the molar mass of propane and octane.
17. List 5 examples of products made with petroleum.
18. List the 3 regions (and %) with most oil reserves.
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19. Consider the following reaction: The potential energy of the reactants is 40J. The activation
energy is 10J. The potential energy of the products is 10J. Notes are in the petroleum section of
your CB.
a. Draw the potential energy diagram for the reaction.
b. Label the reactants and products.
c. Label the activation energy
d. Show where the bonds are broken and where they are formed.
e. Calculate the heat of the reaction.
20. Draw potential energy diagrams for endothermic and exothermic reactions. Know how to
calculate the change in heat.
21. Calorimetry is the procedure that measures the amount of thermal energy in petroleum
products. We use the equation q = mtC. Complete the following table.
What does it mean?
q=
m=
▲t =
C=
What are the units?
a. Calculate the amount of heat transferred when the temperature of 50g of water goes
from 50C to 95C. Specific Heat capacity of water = 4.18J/gC. Report your answer in
J and kJ.
b. Determine the amount of water that would absorb 8500J of energy and undergo a
change in temperature from 40C to 100C.
22. Explain the process of fracking.
23. List 3 pros and 3 cons of fracking.
24. What is the greenhouse effect and what does CO2 have to do with this process?
25. List some possible effects that climate change could have on our planet and on us as humans.
26. What is biodiesel?
27. List 3 advantages to the use of biofuels rather than petroleum.
28. What is the future of biofuels? Where is current research taking it?
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