Name: _____________________________ Date: ______________________________
Chem…is….TRY!!!!!!!
Final Exam includes the following:
1. Unit 5, 7 – Moles and Stoichiometry and Analytical Techniques
2. Unit 10 – Organic Chemistry and Applications
NEXT STEP:
(100% not actually guaranteed. However, it is good practice. So work hard and enjoy the math!!!!!!!!!!!!!!!!!!!!!!!!!!!!!! Also did you actually read this? How did you do it? Was it a waste of your time? Why aren’t you working on the package now? You probably just wasted 10 minutes of your time that you could have spent on the calculations!!!!!!!!!!!!!!!! Get to
work!!!!!!!!!!!!!!!!!!)
(Special instructions written above)
Chemistry 11 – Final Exam – Rough Outline
Unit 5/7: Moles and Stoichiometry
Knowledge and Understanding:
 Preform stoichiometric calculations in non-aqueous environments between two
different compounds using molar ratios from the balanced chemical equations as a
bridge:
o Grams to atoms, or vice versa
o Grams to liters, or vice versa
o Liters to atoms, or vice vera
 Preform stoichiometric calculations in aqueous environments between two different
compounds using molar ratios from the balanced chemical equations as a bridge:
o Concentration to volume or vice versa
o Density and volume to concentration or vice versa
o Ion calculations (i.e: NiCl3 = 3 moles of Cl- produced in water)
o Dilution Calculations (c1v1=c2v2)
 Identify limiting reagent by preforming stoichiometric calculations to determine
amount of product produced from each reactant
 Calculate amount of excess reagent leftover after a chemical reaction
 Calculate percentage yield given experimental information
 Given titration data, preform:
o Calculations including:
 Average volume used
 Initial Concentration of solution
o Evaluation of sources of error for a titration
Questioning and Predicting:
 Predict the products or reactants, balance the chemical equation, and identify the
type of chemical reaction
 Show enthusiasm for chemistry by:
o Giving a question that is interesting to you related to chemical reactions
o Proposing an experiment to answer this question
 Use provided metal activity series to predict the results of mixing different
chemicals.
Planning and conducting:
 Design a titration experiment to determine whether a claim is true or false involving
acids and base using equipment names (Erlenmeyer flask, burette with stand and
clamps, pipette & bulb, beaker, etc.)
 Apply the concepts of accuracy, precision, significant figures, and uncertainty to
experimental procedures involving titrations and determine which set of data is
more accurate, precise, less uncertainty, etc.
Processing and analyzing data and information:
 Describe the relationship between variables involving dilutions questions,
stoichiometric calculations, molar ratios, etc.
 Interpret and analyze your local environment by giving an example of an acid or
base from your daily life.
Evaluation:
 Identify and explain limitations and assumptions with stoichiometric calculations
(i.e: percent yield, incomplete reactions, etc.)
 Exercise healthy informed skepticism to form an investigation to evaluate whether a
claim is true or false.
Unit 10: Organic Chemistry
Processing and analyzing data and information:
 Identify the following functional groups from general formula (i.e: R- COOH) or from
skeletal drawing:
o Alcohol
o Alkanes, Alkenes, Alkynes
o Amides
o Amines
o Benzenes/Aromatics
o Carboxylic Acid
o Ester
o Ether
 Identify the parent chain of a given molecule
 Count the number of carbon and hydrogen when provided a skeletal structure
 Name or draw an organic compound for the following:
o Branches (methyl, ethyl, etc.)
o Multiple branches (di, tri, tetra, etc.)
o Alkyl Halide substitution (bromo, chloro, fluoro, iodo, etc)
o Cis-trans isomers and alkenes
o Alkynes
Evaluation:
 Identify errors involving the naming or drawing of organic compounds
 Use knowledge of dehydration synthesis/esterification to identify experimental
error/confounding errors when trying to produce esters.
 Identify bias given primary or secondary source and then design an experiment to
test any claims given
 Relate organic chemistry to a career (not a teacher!)
Communicate:
 Formulate a mental model and show the reaction path for an alkyl halide
substitution reaction using dipoles, high/low EN, positive & negative charges, curly
arrows to show the movement of electrons, reactants and products.
Stoichiometry Review
1) Calculate the Molar mass of:
a. H
b. HCO3
c. NaCl
2) What are the units for concentration? How many moles in one liter if [HCl] = 1.5 M?
________________
________________
3) Methane (CH4) is a common gas use in camp fire stoves. When it burns with excess
oxygen gas it produces carbon dioxide and water. The equation for this reaction is listed
below:
CH4 (g) + 2 O2 (g) --------------------> CO2 (g) + 2 H2O (g)
A) If 25.0 L of O2(g) reacts with 58.0 g of CH4 at STP, what is the limiting reagent? Support
your answer by calculating the mass produced of CO2.
B) Calculate the leftover mass of excess reactant based on the results from part A).
C) If only 0.01 grams of water were produced from the reaction in part A). What is the percent
yield?
4) Methyl ethanoate has pleasant smell like nail polish. It is produced by the following
equation:
CH3OH
+
+
CH3COOH
→
→
+
CH3OCOCH3 +
H2 O
A) When 65.4 g of methanol (CH3OH) is added to excess ethanoic acid, how many
grams of methyl ethanoate (CH3OCOCH3) will be produced?
B) If 25.0 mL of 1.5 M of CH3COOH is added to excess CH3OH, how many molecules
of H2O will be produced?
C) When 1.58 * 107 molecules of water is produced, how many grams of CH3OH will be
needed to react (assuming ethanoic acid is excess)?
5) When 58.5 g of N2 is added to 1.5 L of H2, what volume of gaseous NH3 will be
produced at STP? Calculate limiting reagent first.
1 N2(g) + 3 H2(g)  2 NH3(g)
Calculations:
1) If 45.8 g of Na2CO3 is dissolved in 150 mL of water, what is the [Na+] and [CO32-]?
Dissociation reaction: Na2CO3(s) -> ___ Na++ 1 CO32
b) If 1.50 mL of this solution was taken and diluted to 1.0 L, what would the new
concentration of CO32- be (i.e: [CO32-])? Remember c1v1 = _______
Organic Chemistry
1. Name the following: (1)
Name: ___________________________
Name: ___________________________
Name: ___________________________
2. Draw the following:
Name: ___________________________
8‐ethyl‐3,4,6‐trimethyl‐7‐
phenyldecane
1‐bromo‐3‐ethyl‐2,4‐diiodo‐5‐
methylcyclopentane
3. See the exemplar and complete the following mechanism on Alkyl Halide Substitution:
A) Name the reactants and complete the following mechanisms below:
Reactant #1
Reactant #2:
Name:
_________________________________
EN: C: _____________________ Cl:____________________ ∆EN: __________________
Mechanism: Show the movement of electrons using curly arrows and label the positive
and negative dipoles
B)
Reactant #1
Reactant #2
Name: _________________________________
Mechanism: Show the movement of electrons using curly arrows
C)
Reactant #1
Reactant
#2
Name: _________________________________
Mechanism: Show the movement of electrons using curly arrows
Chemistry 11: OLD test review
Multiple Choice
Identify the choice that best completes the statement or answers the question.
Unit 7: Stoichiometry
____
1. How many moles of chlorine gas would be needed to produce 10 moles of AlCl3 based on the equation
below?
2Al + 3Cl2 à 2AlCl3
A.
B.
C.
D.
____
15 moles
7 moles
10 moles
3 moles
2. When a reaction occurs between 56.8g of FeCl2, 14.0g of KNO3, and 40.0g of HCl as shown in the
equation below, which of the reactants is the limiting reactant.
3FeCl2 + KNO3
A.
B.
C.
D.
____
+ 4HCl
3FeCl3 + 2H2O + NO + KCl
FeCl2
H2O
KNO3
HCl
3. Based on the chemical equation below, which of the following would be an example of a mole ratio?
5C + 2SO2
A.
B.
C.
D.
____
à
à
CS2
+ 4CO
2CO : 4SO2
5C : 5CS2
4CO : 5C
5C : 1SO2
4. Use the equation below to calculate the volume of carbon dioxide gas produced if 63.25g of water was
produced at the same time.
C3H8(g) + 5O2(g) à 3CO2(g) + 4H2O(l)
A.
B.
C.
D.
____
58.97 L
235.9 L
19.66 L
1.585 x 1024 L
5. When 17.5g of carbon reacts with 39.5g of sulfur dioxide as shown in the equation below, the limiting
reactant is carbon. Based on the equation below, calculate how much the sulfur dioxide will be in excess.
5C + 2SO2
à
CS2
+ 4CO
A.
B.
C.
D.
____
194 g in excess
22.0 g in excess
2.16 g in excess
37.3g in excess
6. In a titration, the equivalence point has been reached when:
A. the base solution changes colour
B. the acid solution changes colour
C. the ratio of the moles of each chemical reactant in the reaction is equal to the coefficients
in the chemical equation
D. the neutralization reaction has begun
____
7. Which of the following best describes the excess reactant?
A.
B.
C.
D.
____
8. The equipment in which the standard solution with the known concentration is held (stored) in for a
titration is called the....
A.
B.
C.
D.
____
The reactant that is used up first in a reaction
The reactant that you will use to calculate the amount of product produced
The reactant you will use to calculate the percentage yield
The reactant that is left over after the reaction finishes
volumetric pipette
test tube
burette
bulb
9. In the following equation, the X in the equation would represent which of the following?
A.
B.
C.
D.
percent error
percent purity
percent yeild
percent reacted
____ 10. The theoretical yield of a product NH3 was 231.6g, while the actual yield when doing the reaction was
104.04g. Based on the theoretical and actual yield of the reaction, calculate the percentage yield for the
reaction.
A.
B.
C.
D.
222.6% yield
44.93% yield
55.08% yield
1.276% yield
____ 11. Based on the equation below, how many moles of Fe(s) would be produced if you mixed 17.4L of carbon
monoxide gas with excess Fe2O3(s)?
Fe2O3(s) + 3CO(g)
à
2Fe(s) + 3CO2(g)
A.
B.
C.
D.
1.93 x 10-23 mol Fe
0.777 mol Fe
28.9 mol Fe
0.518 mol Fe
Unit 9: Organic Chemistry
____ 12. Carbon is the foundation of organic chemistry. Based on its chemical reactivity and ability to form bonds,
which other element could possibly form the basis for life on another planet? (hint: Consider other
chemicals with similar characteristics to carbon)
A.
B.
C.
D.
F
Xe
Si
S
____ 13. How many carbons in the organic molecule pictured below?
A.
B.
C.
D.
11
12
10
13
____ 14. Which of the following could be isomers for heptane (C7H16)?
A.
B.
C.
D.
3-methylhexane
2,3-dimethylhexane
heptyne
heptene
____ 15. Which of the molecules below would contain a section of the backbone that would have a LINEAR
geometry/structure?
A.
B.
C.
D.
octane
cis-oct-2-ene
3-octyne
trans-oct-2-ene
____ 16. Which of the following types of organic molecules would be considered as saturated?
I.
II.
III.
Alkanes
Alkenes
Alkynes
A.
B.
C.
D.
I and II only
II and III only
I only
All of the above
____ 17. Aromatic molecules are a specific catagory of organic compounds that are commonely found in
many products like chlothing. Which of the following molecules must be present in an aromatic
molecule?
A.
C.
B.
D.
Short Answer
Unit 7: Stoichiometry
18. Nitric acid can be neutralized with iron (III) hydroxide as shown in the equation below.
___HNO3(aq) + ___Fe(OH)3(aq) à ___Fe(NO3)3(aq) + ___H2O(l)
a) Balance the equation above with ALL blanks filled in. (1 mark)
b) Determine the concentration of the HNO3 if 42.5 mL of 2.6M Fe(OH)3 is used to titrate 25.00
mL HNO3 ? (3 marks)
Answer:__________________
c)If 92.83 g of HNO3 reacts with excess Fe(OH)3, how many molecules of water would be
produced? (2 marks)
Answer:_________________
Unit 9: Organic Chemistry
19. Complete the following table by either naming the molecules based on the picture provided or
drawing the molecule based on the provided names. (2 marks each)
Name
1-fluoro-2,2,3-trimethylbutane
7-ethyl-2-iodo-6,6-dimethyl-5-propylnon3-yne
Drawing
Chemistry 11 – Final Exam Review Package
Chemistry 11: OLD test review
Answer Section
MULTIPLE CHOICE
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A
C
C
A
C
C
D
C
C
B
D
C
B
A
C
C
D
SHORT ANSWER
18. ANS:
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PTS: 1
19. ANS:
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