Chemistry 30 - SharpSchool



Name |Structure | |

|1. | |

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|2. | |

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|hex-3-yne | |

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|3. | |

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|4. | |

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|hexane | |

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|5. | |

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|6. | |

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|3-butyl-4-propylcyclopentene | |

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|7. | |

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|8. | |

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|tetrachloroethene | |

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|Name |Structure |

|9. | |

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|heptanoic acid | |

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|10. | |

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|11. | |

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|3-methylpentan-2-ol | |

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|12. | |

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|13. | |

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|1,2-diethyl-3,3-dipropylcyclooctane | |

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|14. | |

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|15. | |

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|1-chloro-4-propylcyclopentene | |

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|16. | |

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|Name |Structure |

|17. | |

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|1,2-dichloro-3-fluorocyclobutane | |

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|18. | |

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|19. | |

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|ethyne | |

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|20. | |

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|21. | |

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|1,2-dipropylcyclopentene | |

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|22. | |

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|23. | |

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|3-chlorohexan-1-ol | |

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|24. | |

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25. Give the reaction type, draw and give the names for each of the following reactions:

a)

b) ethene + hydrogen

c) 3-methylhex-1-yne + oxygen

d) n phenylethene

e) benzoic acid + pentan-2-ol

f) + decane + octane

g) choroethane + hydroxide ion

h) pentanoic acid + butan-1-ol

i) heptan-2-ol

j) 1-chloropropane + fluorine

k) + iodobenzene + HI

l) cyclobutane + chlorine

m) ethanol + hexanoic acid

n) pent-1-ene + bromine

o) + 1,1,2,2-tetrafluoropropane

p) chlorobenzene + chlorine

q) butane + bromine

r) oct-2-ene + oxygen

s) propanoic acid + methanol

t) chloroethene

26. In all of your reactions in question 25, circle the saturated organic compounds.

Chemistry 30

Thermochemistry Review

1. What is the difference between kinetic energy and potential energy?

2. Calculate the energy released when 100 g of liquid water cools from 75.0(C to 10.5(C.

3. Calculate the change in enthalpy when 10.62 g of propane burns in a combustion reaction. The molar enthalpy of combustion for propane is (2043.9 kJ/mol.

4. Write out the balanced chemical reactions for photosynthesis and cellular respiration…without looking!!!!

5. For each of the following, re-write the information using the notations not given (shown in brackets after each question):

a) H2O(l) + 285.8 kJ ( H2(g) + ½ O2(g)

((H notation, EP diagram)

b) 2 SO3(g) ( 2 SO2(g) + O2(g) (rH = +197.8 kJ

(inside equation, EP diagram)

c)

((H notation, inside equation)

6. A 2.00 g sample of sucrose was burned in excess oxygen in a bomb calorimeter which contained 2000 mL of water. The temperature of the water increased from 20.0(C to 25.0(C. Determine the molar heat of combustion of sucrose.

7. The combustion of 1.00 g of octane causes the temperature of 200 mL of water in a calorimeter to rise from 15.00(C to 63.00(C. Calculate the molar enthalpy of combustion of octane in kJ/mol. Convert to kJ/g.

8. A student mixed 100.0 mL of 1.50 mol/L sulphuric acid with 200.0 mL of 1.50 mol/L sodium hydroxide. Both solutions were at 21.0(C initially and the highest temperature reached by the reaction mixture was 36.0(C. Calculate the molar enthalpy of neutralization for sulphuric acid.

9. Determine the heat of reaction for:

C(s) + 2 H2(g) ( CH4(g)

10. Determine the heat of reaction for:

2 C(s) + 2 H2(g) + O2(g) ( CH3COOH(l)

11. Carbohydrates, such as sugars and starches, are oxidized in the body to provide needed energy through cellular respiration. Calculate the molar heat of combustion for glucose assuming that the products of combustion are carbon dioxide and liquid water.

12. Calculate the heat produced when 8.22 ( 103 g of sulphur trioxide combines with liquid water to produce sulphuric acid.

13. Calculate the molar heat of formation for nitric acid given the following reaction:

3 NO2(g) + H2O(l) ( 2 HNO3(l) + NO(g) (H = (72.0 kJ

Chemistry 30

Electrochemistry Review

1. For each of the following reactions, write and label the oxidation half reaction, reduction half reaction and net reaction:

a. Solid silver reacts with copper (II) nitrate.

b. Magnesium reacts with aluminium chloride.

c. Iodine reacts with sodium fluoride.

2. Predict the most likely redox reaction and the spontaneity for each of the following:

a. Potassium metal is added to water.

b. Zinc nitrate is stored in an aluminium container.

c. A solution of potassium dichromate is added to an acidified solution of tin (II) chloride.

3. In an experiment, four metals were placed into test tubes containing various ion solutions. Their resulting behaviour is communicated by the equations below. List the reducing agents from strongest to weakest.

Pt(s) + 2 H+(aq) ( Pt2+(aq) + H2(g)

2 Ce(s) + 3 Ni2+(aq) ( 2 Ce3+(aq) + 3 Ni(s)

3 Sr(s) + 2 Ce3+(aq) ( 3 Sr2+(aq) + 2 Ce(s)

Ni(s) + 2 H+(aq) ( Ni2+(aq) + H2(g)

4. Balance each of the following reactions using either the half-reaction method or the oxidation number method:

a. ___H2O(l) + ___Al(s) + ___NO3((aq)( ___AlO2((aq) + ___NH3(aq) + ___H+(aq)

b. ___H+(aq) + ___ClO2((aq) + ___Fe(s) ( ___Fe3+(aq) + ___Cl((aq) + ___H2O(l)

c. ___H+(aq)+ ___MnO4((aq) + ___H2C2O4(aq) ( ___Mn2+(aq) +___CO2(g) +___H2O(l)

5. A 3.52 g piece of aluminum is placed in 350 mL of iron(III) nitrate solution. Assuming that the reaction reaches endpoint, calculate the concentration of the Fe3+(aq) ions.

6. The copper (II) ions in a solution can be converted to copper metal by trickling the solution over iron. The reaction produces iron (II) ions from the scrap iron. If the process produces 10 L of solution containing 0.0035 mol/L of Fe2+(aq) ions, what mass of copper is produced?

7. An experiment was used to analyze the tin in a tin ore sample. The Sn2+(aq) ions in an acidic solution were oxidized to Sn4+(aq) by a 0.200 mol/L KMnO4(aq) solution. Use the following information to calculate the concentration of Sn2+(aq) in the solution. The volume of the tin (II) solution is 25 mL.

Evidence

|Trial |1 |2 |3 |4 |

|Final Volume (mL) |18.40 |35.30 |17.30 |34.10 |

|Initial Volume (mL) |1.00 |18.40 |0.60 |17.30 |

|Volume of KMnO4(aq) (mL) | | | | |

|Endpoint Colour |pink |light pink |light pink |light pink |

8. Draw and completely label the following voltaic cells. Please include the half-reactions, net reaction and calculation of E(net.

a. Zn(s) / Zn2+(aq) // Co2+(aq) / Co(s)

b. Cd(s) / Cd2+(aq) // Cr2O72((aq), Cr3+(aq), H+(aq) / C(s)

9. For each of the following, determine the half-reactions and net reaction and the minimum voltage required.

a. An aqueous solution of lead (II) perchlorate is electrolyzed.

b. A solution of aqueous sodium chloride and aqueous zinc fluoride are mixed in an electrolytic cell using inert electrodes.

c. Electricity is passed through an aqueous solution containing aluminum chloride, magnesium bromide, and sodium iodide.

10. Draw a Venn diagram to show the differences and similarities between voltaic and electrolytic cells.

11. An electrolytic cell containing molten chromium(III) chloride operated for 25.0 minutes. It was found that the mass of molten chromium metal formed was 0.885 g. Calculate the average current of the cell.

12. If a 2.85 A current runs for 5.00 hours through a solution of zinc sulphate, what mass of zinc solid will be produced?

13. An electroplating firm wishes to plate 15.0 g of copper from a Cu(NO3)2(aq) solution onto a pair of baby shoes. If a 2.50 A current is used, calculate the time required. At which electrode would the shoes be attached?

14. If a current plates out 55.6 g of aluminum, what mass of zinc would be plated out in the same time by the same current?

15.

a. Match the correct numbers with the descriptions below:

anode, cathode, electron flow, anion movement, cation movement, anion, cation

b. What type of cell is this and how do you know?

16.

a. Match the correct numbers with the descriptions below:

anode, cathode, electron flow, load (external circuit), electrolyte

b. What type of cell is this and how do you know?

17. Explain how a sacrificial anode works to protect an iron structure. Use specific examples in your explanation.

Chemistry 30

Equilibrium, Acids and Bases Review

1. What is dynamic equilibrium. How does it appear at the macroscopic level?

2. How is % reaction related to the value of Kc?

3. Write the equilibrium expression for:

a) H2(g) + I2(g) ⇌ 2 HI(g)

b) 2 H2(g) + O2(g) ⇌ 2 H2O(l)

4. Given the following reaction:

2 SO2(g) + O2(g) ⇌ 2 SO3(g) + energy

Predict what shifts happens if:

a) [SO2] is increased b) volume is decreased c) system is cooled

5. The following equilibrium can exist in a closed flask:

N2O4(g) ⇌ 2NO2(g)

colorless brown

a) Predict the colour in the flask:

i) upon immediate addition of N2O4 (right at the start)

ii) after 2 seconds

iii) after 1 minute

b) What evidence do you have that the system is at equilibrium?

c) Describe the changes that would occur if NO2 were added into the flask over a one minute time span.

d) What factors could disturb the equilibrium in this system? What would be the corresponding changes in the system?

e) Find Kc if [NO2] = 0.0547 mol/L and [N2O4] = 0.645 mol/L

6. The following reaction is an equilibrium mixture:

CoCl42((al) + 6H2O(() ⇌ Co(H2O)62+(al) + 4Cl((al) + energy

blue pink

Predict the colour change in the mixture when each of the following changes is made:

a) a few drops of water is added to the system

b) heat is added to the system

c) a crystal of NaCl(s) is added to the system

d) a crystal of AgNO3(s) is added to the system

7. Use the following graph to determine what stress has been applied to the system at times A, B, C and D.

N2(g) + 3 H2(g) ⇌ 2 NH3(g) + energy

8. In an experiment, 0.500 mol of H2(g) and 0.500 mol of F2(g) are introduced into a 1.00 L flask at 500(C. After equilibrium was reached, the concentration of HF(g) was 0.0100 mol/L. Calculate the Kc for this reaction at 500(C.

9. Initially, 10.0 g of H2O(g) and 20.0 g of Cl2O(g) are mixed in a sealed 2.00 L flask at 50.0(C. When equilibrium is reached, 5.76 ( 10(3 mol of HOCl(g) is present in the flask. Calculate Kc for this reaction. Are reactants or products being favoured and why?

H2O(g) + Cl2O(g) ⇌ 2 HOCl(g)

10. Complete each of the following reactions, and label all acids/bases and conjugates

a) HNO3(aq) + F((aq) ⇌ +

b) CH3COOH (aq) + HSO4((aq) ⇌ +

c) H2S (aq) + SO42((aq) ⇌ +

d) HCO3((aq) + S2( (l) ⇌ +

11. Calculate the pH for each of the following solutions. Show all work.

a) 0.25 mol/L Ba(OH)2(aq)

b) 3.5 ( 10(4 mol/L NaHSO4(aq) **red with both litmus

c) 1.0 mol/L H2S(aq)

d) 0.750 mol/L K3PO4(aq)

e) 0.150 mol/L HBr(aq)

f) 12.5 mol/L CH3COOH(aq)

12. For each of the following problems:

a) Write a reaction equation.

b) Label reactants as acid or base and products as conjugate acid or conjugate base.

c) Use appropriate arrow notation to indicate reaction predomination (forward or reverse).

a) Solutions of Na2SO4(aq) and H2SO3(aq) are mixed in a beaker.

b) A solution of NH4NO3(aq) and a solution of NaBr(aq) are mixed.

c) Write the equation for NaC6H5COO(s) dissolving in a solution of KHSO4(aq).

d) A household ammonia solution is mixed with a solution of carbonic acid.

e) Hydroiodic acid and potassium hydroxide solutions are mixed.

f) Sodium acetate is dissolved into a solution of hypochlorous acid.

g) Ammonium chloride is dissolved in water.

13. Write out all reaction steps and the net reaction (assuming all reactions are quantitative) for:

a) Sodium hydroxide is continuously added to a solution of phosphoric acid.

b) A potassium carbonate solution is titrated with hydrochloric acid.

14. Define the term buffer.

15. Write the reaction for the addition of small amounts of strong acid to an acetic acid – sodium acetate buffer solution

16.

a) Label the following on the curve:

• buffer region

• overtitration

• endpoint

• equivalence point

b) What is the endpoint pH?

c) What type of titrant is being used (mono, poly, strong or weak)

d) What type of sample is being used (mono, poly, strong or weak).

e) Give one indicator suitable for this titration.

-----------------------

Reaction Progress

(H = (566.0 kJ

(787.0

(221.0

2 CO2(g)

2 CO(g) + O2(g)

EP Diagram for 2 CO(g) + O2(g) ( 2 CO2(g)

EP

(kJ)

H2(g) + [pic] O2(g) ( H2O(l) (H = (285.8 kJ

C(s) + O2(g) ( CO2(g) (H = (393.5 kJ

CH3COOH(l) + 2 O2(g) ( 2 CO2(g) + 2 H2O(l) (H = (874.3 kJ

Organic Chemistry Review

H2(g) + [pic] O2(g) ( H2O(l) (H = (285.8 kJ

C(s) EMBED Equation.3 [pic] O2(g) ( H2O(l) (H = (285.8 kJ

C(s) + O2(g) ( CO2(g) (H = (393.5 kJ

CH4(g) + 2 O2(g) ( CO2(g) + 2 H2O(l) (H = (890.5 kJ

CH3

CH3

CH

CH3

CH

CH

CH2

CH

‗

CH

CH3

CH2

CH3

CH3

CH3

CH2 ( CH2 ( CH3

OH

║

C

CH2

CHBr

CH3

O

CH3

CH

CH2

CH

C2H5

CH2

CH3

CH3

CH3

CH3

C

CH2

C

Br

CH3

Br

Br

Br

Br

CH3

I

OH

CH3

CH

CH

CH3

CH3

CH2

CH3

C

C

CH2

≡

C

CH3

C

CH3

CH

≡

CH

CH3

CH3

OH

║

C

CH2

CH2

CH2

CH3

O

butanoic acid + methanol

(

H2SO4

(

cat

(

(

cat

(

H2SO4

(

cat

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cat

(

H2SO4

(

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H2SO4

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nonspont

spont

spont

spont

Electroplating Cell

A cell capable of lighting a small light bulb can be made by placing copper and zinc strips in a lemon.

D

B

C

A

H2(g)

N2(g)

NH3(g)

Time (min)

Concentration

(mol/L)

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