30S Chemistry Final Exam Problem Review Sheet

Mr. Storie 30S Chemistry Final Exam Review

30S CHEMISTRY FINAL EXAM PROBLEM REVIEW SHEET:

COMPLETE AS MUCH OF THIS REVIEW AS YOU CAN FOR THE FINAL EXAM.

**THIS IS NOT A COMPLETE REVIEW. CONTINUE TO READ ALL COURSE NOTES, GO OVER ALL WORKSHEETS, HANDOUTS, AND THE MID-TERM EXAM TO BE BETTER PREPARED.

PROPERTIES OF MATTER PROBLEMS

1. List each of the following in order of increasing melting points. Explain your reasons for the order. C2H4, NaCl, C2H5OH, C2H6, C2H5F

2. Use temperature to explain that all molecules in a container of liquid have different amounts of energy?

3. Create a concept map showing the relationship between the following terms.  Gas  Solid  Liquid  Sublimation  Deposition  Condensation  Vaporization  Melting  Freezing

4. Why does evaporation lower the temperature of a liquid?

5. Why does the temperature remain constant at the boiling point until all the liquid is gone, no matter how long the liquid is boiled? Use a graph to illustrate your point.

6. Explain how intermolecular forces affect the boiling point of a substance.

CHEMICAL REACTIONS PROBLEMS

23 1. Find the mass of 9.27 x 10 molecules of AlCl3?

2. What is the volume of 8.67 moles of oxygen gas

3. Write a balance equation and identify the category of each of these reactions: a. Calcium carbonate  calcium oxide and carbon dioxide

b. Tin and oxygen  tin (IV) oxide

c. Zinc nitrate and hydrogen sulfide  zinc sulfide and nitric acid

4. What mass of water is produced from 20.0 g of methane (CH4) in the combustion reaction?

5. What mass of propane (C3H8) is required to react with 35 L of oxygen gas (at STP) in a combustion reaction?

6. 7.5 g of potassium chloride is mixed with 11.7 g of calcium hydroxide. Which is the limiting reagent, and what mass of calcium chloride can be produced? Mr. Storie 30S Chemistry Final Exam Review

7. Give the formula for each of the following and state whether each compound is ionic or covalently bonded: a. Nitrogen monoxide b. Dihydrogen monosulfide c. Strontium nitrate d. Dinitrogen pentoxide e. Carbon tetrachloride f. Iron (III) sulfite g. Zinc phosphate h. Potassium carbonate i. Copper (II) sulfate

8. Give the name for each of the following and state whether each compound is ionic or covalently bonded: a. SiF4 b. Cs2SO4 c. MgSO3 d. (NH4)2CO3 e. Ba(OH)2 f. Ca3N2 g. CuClO3 h. NaHSO4 i. Ni3(PO4)2

9. Given the following reaction at STP: 2 C2H6 + 7 O2  4 CO2 + 6 H2O a. What mass of oxygen is needed to react with 68.25 g of ethane?

b. How many molecules of CO2 will form when 3.24 g of ethane reacts with oxygen?

c. How many moles of water can be made from 35.00 g of ethane?

d. What volume of CO2 at STP will be produced from 45.0 g of ethane?

SOLUTIONS PROBLEMS

1. You require 1.00 L of dilute ammonia solution with a concentration of 0.150 M. Ammonia stock solution is 15.0 M. Give instructions to your assistant to make the dilute solution?

2. What would be the concentration of a hydrochloric acid solution prepared by diluting 25.0 mL of concentrated hydrochloric acid (12.0 M) to a volume of 2.00 L?

3. What mass of solute is needed to prepare 1.00 L of each of the following solutions: a. Sodium hydroxide with a concentration of 0.100 M.

b. Calcium nitrate with a concentration of 0.40 M. Mr. Storie 30S Chemistry Final Exam Review

4. Using your solubility rules, complete the following double displacement reactions, also explain why each product is insoluble or soluble. a. sodium sulfate reacts with barium chloride b. potassium phosphate reacts with strontium nitrate c. silver nitrate reacts with sodium sulfide

5. Explain which of the following C2H4, NaCl, C2H5OH, C2H6, C2H5F will dissolve in water and why.

ORGANIC CHEMISTRY PROBLEMS

1. Draw the structural formula for the following: a. 2-heptyne b. 3-ethyl-2-iodo-2-hexene c. 2- methyl-bromobenzene d. 1-propanol e. cyclobutene f. butanoic acid g. 2,4-diphenylhexane h. Ethylpropanoate i. benzoic acid j. 3-methylphenol

2. Name the following structural formulas:

3. List the general formulas for alkane, alkene, alkynes.

4. List all organic functional groups and list whether they are polar or non-polar.

5. Why does a long chain alcohol not dissolve in water?

6. Use an example to show cis/trans isomerization.

7. Use an example to show structural isomerization.

8. Draw a hydrogenation equation for butene.

9. Draw a dehydration equation for 2-butanol. Mr. Storie 30S Chemistry Final Exam Review

GASES PROBLEMS

1. Briefly explain Boyle’s, Charles, and G-L’s laws.

2. What does Absolute zero mean?

3. A gas collected on a day when the pressure was 104 kPa and the temperature was 18°C has a volume of 642 mL. If the volume on another day changed to 937 mL when the temperature was 33°C, what was the pressure on that day?

4. Calculate the volume of 500.0 mL gas if its temperature is doubled from 25.0°C to 45.0°C.

5. You get a balloon at the circus with a volume of 4.50 L at room temperature (20.0°C). You then step outside on a cold winter day (–20.0°C). If the pressure remains constant, what is the balloon’s new volume?

6. Change the following from the initial conditions to the new conditions: a) 150.0 mL oxygen gas at 10.50 kPa is changed to 19.91 kPa b) 250.0 mL nitrogen at 0.990 atm is changed to 0.05 atm

7. You fill your tires on a cool morning (5.0°C) to a pressure of 35 kPa. If you take a long driving trip where the tire temperature reaches 45.0°C, what is the pressure in the tire while you are driving?

8. If the pressure exerted by nitrogen gas at 22.0°C in a volume of 0.45 L is 785.5 kPa, how many grams of gas is present? Mr. Storie 30S Chemistry Final Exam Review

30S CHEMISTRY FINAL EXAM REVIEW KEY:

PROPERTIES OF MATTER PROBLEMS

1. List each of the following in order of increasing melting points. Explain your reasons for the order. C2H4, NaCl, C2H5OH, C2H6, C2H5F C2H4 – lower melting points than alkane of size, only weak dispersion IMFs. C2H6 – higher than alkene, but only dispersion IMF. C2H5F – polar covalent compound with have dipole-diplole IMFs. C2H5OH – polar covalent compound with hydrogen-bonding IMFs (stronger) NaCl – ionic compound with very strong electrostatic attraction IMF.

2. Do all particles in a container of a liquid have the same amount of energy? Explain. NO, temperature is a measure of the average kinetic energy of the population of particles. Every particle can have a differing amount of energy as seen in the graph:

3. Create a concept map showing the relationship between the following terms.  Gas  Solid  Liquid  Sublimation  Deposition  Condensation  Vaporization  Melting  Freezing

4. Why does evaporation lower the temperature of a liquid? Only those particles with enough kinetic energy (the highest amount) can escape the IMFs and become gas particles. When they do, they leave behind only those particles with less energy – Mr. Storie 30S Chemistry Final Exam Review

temperature is a measure of average kinetic energy, which goes down as high energy particles evaporate.

5. Why does the temperature remain constant at the boiling point until all the liquid is gone, no matter how long the liquid is boiled? Use a graph to illustrate your point. As temperature increases, solid particles begin to absorb the heat and convert it to kinetic energy. When the particles have enough energy they begin to overcome the IMFs holding them together in a crystal, at this point the continued heat energy is used to break up the IMFs and not used as kinetic energy (raising the temperature). Once all solid particles have broken the forces to become liquid, the heat energy is once again used to increase particle kinetic energy.

6. Giving examples, explain how intermolecular forces affect the boiling point of a substance. Stronger IMFs require more energy from each particle to break free, which requires a higher temperature. A molecule like methane (CH4) is non-polar and only has weak dispersion forces. Thus its particles require little energy to break the forces – a gas at room temperature. Water (H2O) is polar-covalent had has strong hydrogen-bonding IMFs holding particles together – higher temperature required to reach needed energy, thus liquid at room temperature (bp – 100). Table salt (NaCl) is an ionic compound held together by the strongest IMFs – electrostatic attraction. This requires the highest boiling point for the particles to receive enough energy which is why it is still solid at room temperature (bp > 700)

CHEMICAL REACTIONS PROBLEMS

23 1. Find the mass of 9.27 x 10 molecules of AlCl3? 9.27 x 1023 molcs x 1 mole/6.02 x 10 23 molcs x 133.33 g/1 mole = 205.318 g = 205 g of AlCl3

2. What is the volume of 8.67 moles of oxygen gas 8.67 moles x 22.4 L/1 mole = 194.2 L Mr. Storie 30S Chemistry Final Exam Review

= 194 L O2 gas

3. Write a balance equation and identify the category of each of these reactions: a. Calcium carbonate  calcium oxide and carbon dioxide CaCO3  CaO + CO2 - decomposition

b. Tin and oxygen  tin (IV) oxide Sn + O2  SnO2 - synthesis

c. Zinc nitrate and hydrogen sulfide  zinc sulfide and nitric acid Zn(NO3)2 + H2S  ZnS + 2 HNO3 - double displacement

4. What mass of water is produced from 20.0 g of methane (CH4) in the combustion reaction? CH4 + 2 O2  2 H2O + CO2 20.0 g x 1 mole/16.05 g x 2 H2O/1 CH4 x 18.02 g /1 mole = 44.91 g =44.9 g H2O

5. What mass of propane (C3H8) is required to react with 35.0 L of oxygen gas (at STP) in a combustion reaction? C3H8 + 5 O2  4 H2O + 3 CO2 35.0 L x 1 mole/22.4 L x 1 C3H8/5 O2 x 44.11 g /1 mole = 13.78 g =13.8 g C3H8

6. 7.5 g of potassium chloride is mixed with 11.7 g of calcium hydroxide. Which is the limiting reagent, and what mass of calcium chloride can be produced? 2 KCl + Ca(OH)2  CaCl2 + 2 KOH 7.5 g x 1 mole/74.55 g x 1 Ca(OH)2/2 KCl x 74.1 g /1 mole = 3.72 g Ca(OH)2 =KCl is the limiting reactant

7.5 g x 1 mole/74.55 g x 1 CaCl2/2 KCl x 110.95 g /1 mole = 5.582 g = 5.6 g CaCl2

7. Give the formula for each of the following and state whether each compound is ionic or covalently bonded:

a. Nitrogen monoxide NO - covalent b. Dihydrogen monosulfide H2S - covalent c. Strontium nitrate Sr(NO3)2 - ionic d. Dinitrogen pentoxide N2O5 - covalent Mr. Storie 30S Chemistry Final Exam Review

e. Carbon tetrachloride CCl4 - covalent f. Iron (III) sulfite Fe2(SO3)3 - ionic g. Zinc phosphate Zn3(PO4)2 - ionic h. Potassium carbonate K2CO3 - ionic i. Copper (II) sulfate CuSO4 - ionic

8. Give the name for each of the following and state whether each compound is ionic or covalently bonded: a. SiF4 silicon tetrafluoride - covalent b. Cs2SO4 cesium sulfate - ionic c. MgSO3 magnesium sulfite - ionic d. (NH4)2CO3 ammonium carbonate - ionic e. Ba(OH)2 barium hydroxide - ionic f. Ca3N2 calcium nitride - ionic g. CuClO3 copper (I) chlorate - ionic h. NaHSO4 sodium bisulfate - ionic i. Ni3(PO4)2 nickel (II) phosphate- ionic

9. Given the following reaction at STP: 2 C2H6 + 7 O2  4 CO2 + 6 H2O a. What mass of oxygen is needed to react with 68.25 g of ethane? 68.25 g x 1 mole/30.06 g x 7 O2/2 C2H6 x 32.00 g/1 mole = 254.29 g = 254.3 g O2 b. How many molecules of CO2 will form when 3.24 g of ethane reacts with oxygen? 23 3.24 g x 1 mole/30.06 g x 4 CO2/2 C2H6 x 6.02 x 10 /1 mole = 1.297 x 1023 23 = 1.30 x 10 molcs of CO2

c. How many moles of water can be made from 35.00 g of ethane? 35.00 g x 1 mole/30.06 g x 6 H2O/2 C2H6 = 3.493 = 3.493 moles of H2O

d. What volume of CO2 at STP will be produced from 45.0 g of ethane? 45.0 g x 1 mole/30.06 g x 4 CO2/2 C2H6 x 22.4 L/1 mole = 67.065 L = 67.1 L CO2

SOLUTIONS PROBLEMS

1. You require 1.00 L of dilute ammonia solution with a concentration of 0.150 M. Ammonia stock solution is 15.0 M. Give instructions to your assistant to make the dilute solution? C1V1=C2V2 1. add 500ml of water to empty beaker 15.0(V1)=0.15(1.0) 2. add 10 mL (0.01 L) of stock to the beaker = 0.01 L 3. mix 4. fill volume up to 1 L with water 5. mix again Mr. Storie 30S Chemistry Final Exam Review

2. What would be the concentration of a hydrochloric acid solution prepared by diluting 25.0 mL of concentrated hydrochloric acid (12.0 M) to a volume of 2.00 L? C1V1=C2V2 C1(2.0 L) = 0.025 L(12.0 M) = 0.15 M

3. What mass of solute is needed to prepare 1.00 L of each of the following solutions: a. Sodium hydroxide with a concentration of 0.100 M. 0.100 mole/1 L x 40.0 g/1 mole = 4.00 g of NaOH

b. Calcium nitrate with a concentration of 0.40 M. 0.40 moles/1 L x 164.1 g/1 mole = 65.64 g =65.6 g Ca(NO3)2 4. Using your solubility rules, complete the following double displacement reactions, also explain why each product is insoluble or soluble. a. sodium sulfate reacts with barium chloride Na2SO4 + BaCl2  2 NaCl + BaSO4 Sol insol

b. potassium phosphate reacts with strontium nitrate 2 K3PO4 + 3 Sr(NO3)2  6 KNO3 + Sr3(PO4)2 Sol insol

c. silver nitrate reacts with sodium sulfide 2 AgNO3 + Na2S  Ag2S + 2 NaNO3 Insol sol

5. Explain which of the following C2H4, NaCl, C2H5OH, C2H6, C2H5F will dissolve in water and why. C2H4, C2H6 – non-polar molecules are insoluble in water because there are no forces of attraction between solute and solvent, the molecule is neutral charged. NaCl – ionic compound contains + and – charged ions. Forces of attraction between solute and solvent are stronger than between solvent (cohesion) C2H5OH, C2H5F – polar covalent compounds contain + and – charged poles that are attracted to the poles of solvent. Attraction between solute-solvent is stronger.

ORGANIC CHEMISTRY PROBLEMS

Draw the structural formula for the following: 1. 2-heptyne 2. 3-ethyl-2-iodo-2-hexene 3. 2- methyl-bromobenzene

CH3 - CΞC-CH2-CH2-CH2-CH3 Mr. Storie 30S Chemistry Final Exam Review

4. 1-propanol 5. cyclobutene 6. butanoic acid

7. 2,4-diphenylhexane 8. ethylpropanoate 9. benzoic acid

CH3CH2C=O

Name the following structural formulas:

Mr. Storie 30S Chemistry Final Exam Review

propyl butanoate 2-methylbutane

3-ethyltoluene trichloromethane cyclohexane phenol 2-butanol butyne

propanoic acid hexene

GASES PROBLEMS

1. Briefly explain Boyle’s, Charles, and G-L’s laws. B = volume is inversely proportional to any change in pressure (at constant T). C = volume is directly proportional to any changes in temperature (at constant P). G/L: Pressure is directly proportional to any temperature changes (at constant V).

2. What does Absolute zero mean? Temperature where particles of an ideal gas have zero kinetic energy – motion stops and volume is reduced to theoretical zero.

3. A gas collected on a day when the pressure was 104 kPa and the temperature was 18°C has a volume of 642 mL. If the volume on another day changed to 937 mL when the temperature was 33°C, what was the pressure on that day? PV/T = P2V2/T2 P2 = PVT2 / TV2

104 (0.642) / (18 + 273) = P(0.937) / (33 + 273)

P = 74.9 kPa

4. Calculate the volume of 500.0 mL gas if its temperature is increased from 25.0°C to 45.0°C. V/T = V2/T2

V2 = VT2 / T = (0.5)(45+273) / (25+273) = 0.53 L

5. You get a balloon at the circus with a volume of 4.50 L at room temperature (20.0°C). You then step outside on a cold winter day (–20.0°C). If the pressure remains constant, what is the balloon’s new volume? V/T = V2/T2

V2 = VT2 / T = (4.5)(-20+273) / (20+273) = 3.89 L Mr. Storie 30S Chemistry Final Exam Review

6. Change the following from the initial conditions to the new conditions: a) 150.0 mL oxygen gas at 10.50 kPa is changed to 19.91 kPa b) 250.0 mL nitrogen at 0.990 atm is changed to 0.05 atm PV = P2V2 V2 = (10.5)(0.150) / (19.91) = 0.079 L

PV = P2V2 V2 = (0.99 x 101.3/1)(0.25) / (0.05 x 101.3/1) = 5 L

7. You fill your tires on a cool morning (5.0°C) to a pressure of 35 kPa. If you take a long driving trip where the tire temperature reaches 45.0°C, what is the pressure in the tire while you are driving? P/T = P2/T2

P2 = PT2 / T = (35)(45+273) / (5+273) = 40 kPa

8. If the pressure exerted by nitrogen gas at 22.0°C in a volume of 0.45 L is 785.5 kPa, how many grams of gas is present? PV = nRT n = PV/RT = (785.5)(0.45)/(8.314)(22+273) n = 0.14 mol

0.14mol x 28g / 1 mol = 3.9 g of nitrogen