CHemistry Students: the Chem site is www.acchemistry.blogspot.com

if you are here for your sample exam, it's at http://www.acchemistry.blogspot.com

Great Link for Chemistry--Bonus

for the bonus, you must print out the page and staple it in your notebook.

http://misterguch.brinkster.net/explains2.html

Topics for Exam Ep 4

Ch 11--types of reactions

ch 12--Stoichemistry
limiting reagents
excess
percent yield
mole-gram
mole-volume
stp


ch 13
kinetic theory of gases, liquids, and solids
melting, boiling, and evaporation
conversion of kpascals to atms
crystal structure--cubics

exam covers ch 8-13

read through topics on ch 8-11.

Sample exam final ep 4 BONU

sample exam ep 4

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.

____ 1. According to the kinetic theory, collisions between molecules in a gas ____.
a. are perfectly elastic c. never occur
b. are inelastic d. cause a loss of total kinetic energy


____ 2. The average speed of oxygen molecules in air is about ____.
a. 0 km/h c. 1700 km/h
b. 170 km/h d. 17,000 km/h


____ 3. Standard conditions when working with gases are defined as ____.
a. 0 K and 101.3 kPa c. 0 C and 101.3 kPa
b. 0 K and 1 kPa d. 0 C and 1 kPa


____ 4. How does the atmospheric pressure at altitudes below sea level compare with atmospheric pressure at sea level?
a. The atmospheric pressure below sea level is higher.
b. The atmospheric pressure below sea level is lower.
c. The pressures are the same.
d. Differences in pressures cannot be determined.


____ 5. The temperature at which the motion of particles theoretically ceases is ____.
a. –273 K c. 0 C
b. 0 K d. 273 C


____ 6. Consider an iron cube and an aluminum cube. If the two cubes were at the same temperature, how would the average kinetic energy of the particles in iron compare with the average kinetic energy of the particles in aluminum?
a. The average kinetic energy of the iron particles would be greater.
b. The average kinetic energy of the aluminum particles would be greater.
c. There would be no difference in the average kinetic energies.
d. No determination can be made based on the information given.


____ 7. The average kinetic energy of water molecules is greatest in ____.
a. steam at 100 C c. liquid water at 373 K
b. liquid water at 90 C d. ice at 0 C


____ 8. What is the key difference between a liquid and a gas?
a. intermolecular attractions c. average kinetic energy
b. the ability to flow d. the motion of their particles


____ 9. If a liquid is sealed in a container and kept at constant temperature, how does its vapor pressure change over time?
a. It continues to steadily increase.
b. It increases at first, then remains constant.
c. It increases at first, then decreases.
d. It continues to steadily decrease.


____ 10. An increase in the temperature of a contained liquid ____.
a. has no effect on the kinetic energy of the liquid
b. causes the vapor pressure above the liquid to decrease
c. causes fewer particles to escape from the surface of the liquid
d. causes the vapor pressure above the liquid to increase


____ 11. When the vapor pressure of a liquid is equal to the atmospheric pressure, the liquid ____.
a. has no observable changes. c. evaporates.
b. boils vigorously. d. begins to boil.


____ 12. Compared to the melting points of ionic compounds, the melting points of molecular solids tend to be ____.
a. similar c. lower
b. unpredictable d. higher


____ 13. Most solids ____.
a. are dense and difficult to compress c. are amorphous
b. are able to flow d. have a disorderly structure


____ 14. Crystals are classified into how many different crystal systems?
a. 4 c. 6
b. 5 d. 7


____ 15. The smallest group of particles in a crystal that retains the shape of the crystal is called the ____.
a. cube c. cage
b. unit cell d. crystal lattice


____ 16. The escape of molecules from the surface of a liquid is known as ____.
a. condensation c. evaporation
b. boiling d. sublimation


____ 17. The direct change of a substance from a solid to a gas is called ____.
a. evaporation c. condensation
b. sublimation d. solidification

Compilation of Chemistry Powerpoint Video

Ch 1-4 Conversions


Ch 1-4 Significant Figures


Ch 1-4 Scientific Notation


Ch 5 Quantum Mechanics


Ch 7 Covalent Bonds pt 2


Ch 7 Covalent Bonds pt 3


Ch 12 Stoichemistry


Ch 14 Aqueous Solutions pt 1


Ch 14 Aqueous Solutions pt 2




Ch 16 Solutions


Ch 16.3 Colligative Properties


Ch 21 ElectroChemistry

AC Chemistry Bonus 4: EP 4-6

Page 382. # 81-86

write the question in your notebook. enjoy

AC Chemistry Quiz Make-up

Watch the latest videos on YouTube.com

1. find me a video of a chemistry experiment that is up to date with our class.

hint: ep 5 rate law, free energy--exothermic or endothermic, or equilibrium

ep 4 kinetic theory of gases, liquids, and solids.

Ep 6 sample exam Matching answers

Watch the latest videos on YouTube.com

review ep 6 final
Answer Section

MATCHING

1. ANS: C DIF: L1 REF: p. 101, p. 102
OBJ: 4.1.1, 4.1.2

2. ANS: A DIF: L1 REF: p. 106 OBJ: 4.2.1

3. ANS: D DIF: L1 REF: p. 104 OBJ: 4.2.1

4. ANS: E DIF: L1 REF: p. 106 OBJ: 4.2.1

5. ANS: B DIF: L1 REF: p. 106, p. 107
OBJ: 4.2.1, 4.2.2

6. ANS: E DIF: L1 REF: p. 112 OBJ: 4.3.1

7. ANS: A DIF: L1 REF: p. 111 OBJ: 4.3.1

8. ANS: C DIF: L1 REF: p. 110 OBJ: 4.3.1

9. ANS: D DIF: L1 REF: p. 114 OBJ: 4.3.3

10. ANS: B DIF: L1 REF: p. 114 OBJ: 4.3.3

11. ANS: A DIF: L1 REF: p. 130, p. 131
OBJ: 5.1.2

12. ANS: F DIF: L1 REF: p. 145 OBJ: 5.1.3

13. ANS: D DIF: L1 REF: p. 142 OBJ: 5.1.3

14. ANS: B DIF: L1 REF: p. 133 OBJ: 5.1.3, 5.2.1

15. ANS: C DIF: L1 REF: p. 133 OBJ: 5.2.1

16. ANS: E DIF: L1 REF: p. 134 OBJ: 5.2.1

17. ANS: D DIF: L1 REF: p. 128 OBJ: 5.1.3

18. ANS: E DIF: L1 REF: p. 128 OBJ: 5.1.3

19. ANS: B DIF: L1 REF: p. 138 OBJ: 5.3.1

20. ANS: C DIF: L1 REF: p. 138 OBJ: 5.3.1

21. ANS: F DIF: L1 REF: p. 139 OBJ: 5.3.1

22. ANS: A DIF: L1 REF: p. 141 OBJ: 5.3.2

23. ANS: H DIF: L1 REF: p. 157 OBJ: 6.1.1

24. ANS: I DIF: L1 REF: p. 157 OBJ: 6.1.1

25. ANS: F DIF: L1 REF: p. 157 OBJ: 6.1.1

26. ANS: D DIF: L1 REF: p. 158 OBJ: 6.1.3

27. ANS: E DIF: L1 REF: p. 166 OBJ: 6.2.2

28. ANS: C DIF: L1 REF: p. 170 OBJ: 6.3.1

29. ANS: G DIF: L1 REF: p. 172 OBJ: 6.3.2

30. ANS: J DIF: L1 REF: p. 172 OBJ: 6.3.2

31. ANS: A DIF: L1 REF: p. 177 OBJ: 6.3.3

32. ANS: B DIF: L1 REF: p. 173 OBJ: 6.3.3

33. ANS: E DIF: L1 REF: p. 187 OBJ: 7.1.1

34. ANS: B DIF: L1 REF: p. 188 OBJ: 7.1.2

35. ANS: D DIF: L1 REF: p. 188 OBJ: 7.1.4

36. ANS: A DIF: L1 REF: p. 192 OBJ: 7.1.4

37. ANS: C DIF: L1 REF: p. 194 OBJ: 7.2.1

38. ANS: G DIF: L1 REF: p. 201 OBJ: 7.2.1

39. ANS: F DIF: L1 REF: p. 198 OBJ: 7.2.2

Review Ep 6 Final Sample

Watch the latest videos on YouTube.com

Matching

Match each item with the correct statement below.
a. proton d. electron
b. nucleus e. neutron
c. atom


____ 1. the smallest particle of an element that retains the properties of that element

____ 2. a positively charged subatomic particle

____ 3. a negatively charged subatomic particle

____ 4. a subatomic particle with no charge

____ 5. the central part of an atom, containing protons and neutrons

Match each item with the correct statement below.
a. mass number d. atomic mass
b. atomic mass unit e. isotope
c. atomic number


____ 6. atoms with the same number of protons, but different numbers of neutrons in the nucleus of an atom

____ 7. the total number of protons and neutrons in the nucleus of an atom

____ 8. the number of protons in the nucleus of an element

____ 9. the weighted average of the masses of the isotopes of an element

____ 10. one-twelfth the mass of a carbon atom having six protons and six neutrons

Match each item with the correct statement below.
a. atomic orbital d. ground state
b. aufbau principle e. Pauli exclusion principle
c. electron configuration f. Heisenberg uncertainty principle


____ 11. region of high probability of finding an electron

____ 12. states the impossibility of knowing both velocity and position of a moving particle at the same time

____ 13. lowest energy level

____ 14. tendency of electrons to enter orbitals of lowest energy first

____ 15. arrangement of electrons around atomic nucleus

____ 16. each orbital has at most two electrons

Match each item with the correct statement below.
a. atomic emission spectrum d. photon
b. frequency e. quantum
c. wavelength f. spectrum


____ 17. discrete bundle of electromagnetic energy

____ 18. energy needed to move an electron from one energy level to another

____ 19. number of wave cycles passing a point per unit of time

____ 20. distance between wave crests

____ 21. separation of light into different wavelengths

____ 22. frequencies of light emitted by an element

Match each item with the correct statement below.
a. electronegativity f. periodic law
b. ionization energy g. cation
c. atomic radius h. period
d. metal i. group
e. transition metal j. electrons


____ 23. horizontal row in the periodic table

____ 24. vertical column in the periodic table

____ 25. A repetition of properties occurs when elements are arranged in order of increasing atomic number.

____ 26. type of element that is a good conductor of heat and electric current

____ 27. type of element characterized by the presence of electrons in the d orbital

____ 28. one-half the distance between the nuclei of two atoms when the atoms are joined

____ 29. type of ion formed by Group 2A elements

____ 30. subatomic particles that are transferred to form positive and negative ions

____ 31. ability of an atom to attract electrons when the atom is in a compound

____ 32. energy required to remove an electron from an atom

Match each item with the correct statement below.
a. halide ion e. valence electron
b. octet rule f. coordination number
c. ionic bond g. metallic bond
d. electron dot structure


____ 33. an electron in the highest occupied energy level of an atom

____ 34. Atoms react so as to acquire the stable electron structure of a noble gas.

____ 35. a depiction of valence electrons around the symbol of an element

____ 36. an anion of chlorine or other halogen

____ 37. the force of attraction binding oppositely charged ions together

____ 38. the attraction of valence electrons for metal ions

____ 39. the number of ions of opposite charge surrounding each ion in a crystal

Sample Exam Ep 6

review essay

Short Answer

1. For the reaction 2Na(s) + Cl (g) --> 2NaCl(s), how many grams of NaCl could be produced from 103.0 g of Na and 13.0 L of Cl (at STP)?

2. Solid sodium reacts violently with water, producing heat, hydrogen gas, and sodium hydroxide. How many molecules of hydrogen gas are formed when 48.7 g of sodium are added to water?
2Na + 2H O --> 2NaOH + H

Essay

3. When a mixture of sulfur and metallic silver is heated, silver sulfide is produced. What mass of silver sulfide is produced from a mixture of 3.0 g Ag and 3.0 g S ?
16Ag(s) + S (s) --> 8Ag S(s)

4. What is the limiting reagent when 150.0 g of nitrogen react with 32.1 g of hydrogen?
N (g) + 3H (g) --> 2NH (g)

5. A 500-g sample of Al (SO ) is reacted with 450 g of Ca(OH) . A total of 596 g of CaSO is produced. What is the limiting reagent in this reaction, and how many moles of excess reagent are unreacted?
Al (SO ) (aq) + 3Ca(OH) (aq) --> 2Al(OH) (s) + 3CaSO (s)

Extra Credit Assignment #2 Week of Jan 13

page 319 # 1-15 write the question in your notebook.

this is worth quiz points.

Extra Credit Assignment #1 Week of Jan 7 1009

option 1. page 383 standarized test prep--write the question and just the answer.

option 2. attend the debate training on January 16 at Trium Udom Suksa

Make up exams for second semester

All retests must be turned in by January 20th, hand written in your notebooks. copy the question also.

ep 6 test
Essay

1. Explain what occurs in an electrochemical cell.

2. What are the components of a voltaic cell?

3. Describe a common dry cell.

4. Describe the lead storage battery.

5. Describe how a fuel cell works.

6. What is the standard cell potential?

7. Explain what occurs in an electrolytic cell.

8. Give the sign of the electrodes and the reaction that occurs at each for both voltaic and electrolytic cells.

EP 5 test
make up test ep 5

Essay

1. When steam is used to drive a turbine, the kinetic energy of the moving turbine will be less than the energy used initially to heat the water to steam. Explain why this is not a violation of the law of conservation of energy.

2. Explain the difference between temperature and heat. Also, state what determines the direction of heat transfer.

3. Explain the distinction between heat capacity and specific heat. Provide an example to illustrate this distinction.

4. Describe the parts of a calorimeter and the function of each part.

5. Using what you know about phase changes, why does steam at 100 C produce a more harmful burn than boiling water?

6. Explain the effects of reactant concentration and particle size on the rate of a reaction.


ep 4 test
make up test ep 4

Essay

1. In general, how are word equations written to describe chemical reactions?

2. Describe how to write the skeleton equation for the following reaction:

iron + oxygen iron(III) oxide

3. Consider the description: copper(II) oxide reacts with sulfuric acid to produce copper(II) sulfate and water. List the steps required to write its balanced chemical equation. State how to determine which of the five general types of reaction this represents.

4. What determines whether one metal will replace another metal from a compound in a single-replacement reaction?

5. Predict the precipitate that forms when aqueous solutions of silver nitrate and potassium chloride react to form products in a double-replacement reaction. Include a discussion of how to write the complete chemical equation describing this reaction.

6. When a mixture of sulfur and metallic silver is heated, silver sulfide is produced. What mass of silver sulfide is produced from a mixture of 3.0 g Ag and 3.0 g S ?
16Ag(s) + S (s) 8Ag S(s)

7. What is the limiting reagent when 150.0 g of nitrogen react with 32.1 g of hydrogen?
N (g) + 3H (g) 2NH (g)

8. A 500-g sample of Al (SO ) is reacted with 450 g of Ca(OH) . A total of 596 g of CaSO is produced. What is the limiting reagent in this reaction, and how many moles of excess reagent are unreacted?
Al (SO ) (aq) + 3Ca(OH) (aq) 2Al(OH) (s) + 3CaSO (s)

Syllabus for AC Chemistry

http://www.youtube.com/watch?v=-uqKtczj-hA

My syllabus for class

Exam Topix

Watch the latest videos on YouTube.com

EP 6 Exam topics:

What is standard conditions for battery reactions? Know the composition of batteries from galvanic, voltaic, electrolytic, dry, alkaline, fuel cells, and lead car battery? Also some random stoichemistry from ch 12 to separate the boys from the men.

EP 5 exam topic:

Know how to convert cals to joules, ch 17-18--know equilibrium constants and equilibrium, convert one metal's heat into water, calorimetry

EP 4 exam topics:

Know how to do all the problems from mole to atoms, molecules, volume, density, composition, empirical, and molecular. YES, there are limiting reagents along with types of reactions such as single replacement, combustion, etc. And yes, there are some real doozies to separate the boys from the men.

Ep 6 summative review

summative review ep 6

Matching


Match each item with the correct statement below.
a. anode d. half-cell
b. battery e. cathode
c. fuel cell


____ 1. the electrode at which oxidation occurs

____ 2. one part of a voltaic cell in which either oxidation or reduction occurs

____ 3. the electrode at which reduction occurs

____ 4. a group of cells that are connected together

____ 5. a voltaic cell in which a fuel substance undergoes oxidation and from which electrical energy is obtained continuously

Match each item with the correct statement below.
a. electrode d. voltaic cell
b. electrolysis e. dry cell
c. salt bridge


____ 6. a tube containing a conducting solution

____ 7. a conductor in a circuit that carries electrons to or from a substance other than a metal

____ 8. an electrochemical cell that is used to convert chemical energy to electrical energy

____ 9. a voltaic cell in which the electrolyte is a paste

____ 10. a process in which electrical energy is used to bring about a chemical change

Match each item with the correct statement below.
a. actual yield e. limiting reagent
b. percent yield f. mass
c. theoretical yield g. number of molecules
d. excess reagent h. volume


____ 11. This quantity can always be used in the same way as moles when interpreting balanced chemical equations.

____ 12. This is conserved only in reactions where the temperature is constant and the number of moles of gaseous reactants is the same as that of gaseous products.

____ 13. This is conserved in every ordinary chemical reaction.

____ 14. the reactant that determines the amount of product that can be formed in a reaction

____ 15. the maximum amount of product that could be formed from given amounts of reactants

____ 16. the reactant that is not completely used up in a reaction

____ 17. the amount of product formed when a reaction is carried out in the laboratory

____ 18. the ratio of the actual yield to the theoretical yield

Match each item with the correct statement below.
a. product d. balanced equation
b. reactant e. skeleton equation
c. chemical equation


____ 19. a chemical equation that does not indicate relative amounts of reactants and products

____ 20. a new substance formed in a chemical reaction

____ 21. a starting substance in a chemical reaction

____ 22. a concise representation of a chemical reaction

____ 23. an equation in which each side has the same number of atoms of each element

Match each item with the correct statement below.
a. activity series of metals c. combustion reaction
b. single-replacement reaction d. decomposition reaction


____ 24. a reaction in which a single compound is broken down into simpler substances

____ 25. a reaction in which oxygen reacts with another substance, often producing heat or light

____ 26. a reaction in which the atoms of one element replace the atoms of a second element in a compound

____ 27. a list of metals in order of decreasing reactivity

Match each item with the correct statement below.
a. molar volume
b. molar mass
c. atomic mass


____ 28. the number of grams of an element that is numerically equal to the atomic mass of the element in amu

____ 29. the mass of a mole of any element or compound

____ 30. the volume occupied by a mole of any gas at STP

Match each item with the correct statement below.
a. representative particle d. percent composition
b. mole e. standard temperature and pressure
c. Avogadro's number f. empirical formula


____ 31. the number of representative particles of a substance present in 1 mole of that substance

____ 32. an atom, an ion, or a molecule, depending upon the way a substance commonly exists

____ 33. the SI unit used to measure amount of substance

____ 34. 0 C and 1 atm

____ 35. the percent by mass of each element in a compound

____ 36. the smallest whole number ratio of the atoms in a compound

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.

____ 37. In a zinc-copper cell, Zn | Zn (1M) || Cu (1M) | Cu, which electrode is negative?
a. Cu (aq) c. Zn(s)
b. Cu(s) d. Zn (aq)


____ 38. In a dry cell, the electrolyte is a ____.
a. solid c. liquid
b. paste d. gas


____ 39. What is the electrode in the center of the most common dry cell made of?
a. copper c. iron
b. zinc d. graphite


____ 40. What metal is oxidized in the most common dry cell?
a. copper c. iron
b. zinc d. carbon


____ 41. In a fully charged lead storage battery, the cathode grid is packed with ____.
a. spongy lead c. lead(IV) oxide
b. lead sulfate d. sulfuric acid


____ 42. Why can’t a lead storage battery be recharged indefinitely?
a. A direct current must pass through the cells.
b. The electrodes lose lead sulfate.
c. It is difficult to reverse the direction of current flow.
d. The electrolyte is too expensive.


____ 43. What happens in a hydrogen-oxygen fuel cell?
a. Oxygen diffuses through the cathode.
b. Oxygen diffuses through the anode.
c. Hydrogen diffuses through the cathode.
d. Hydrogen and oxygen are mixed before entering the anode.


____ 44. In which direction will the following reaction go if the standard reduction potentials are 0.80 V for Ag/Ag and –0.44 V for Fe/Fe ?
Ag + Fe Ag + Fe
a. forward c. No such reaction can occur.
b. reverse d. Not enough information is given.


____ 45. What is the standard cell potential of a cell made of theoretical metals Ma/Ma and Mb/Mb if the reduction potentials are –0.19 V and –0.85 V, respectively?
a. +0.66 V c. +1.04 V
b. –0.66 V d. –1.04 V


____ 46. What is produced in the electrolysis of brine?
a. chlorine gas, sodium hydroxide, and hydrogen gas
b. chlorine gas and hydrogen gas only
c. chlorine gas and oxygen gas only
d. chlorine gas and sodium only


____ 47. The gas produced at the cathode in the electrolysis of brine is ____.
a. hydroxide c. oxygen
b. chlorines d. hydrogen


summative review ep 6
Answer Section

MATCHING

1. ANS: A DIF: L1 REF: p. 665 OBJ: 21.1.2

2. ANS: D DIF: L1 REF: p. 665 OBJ: 21.1.2

3. ANS: E DIF: L1 REF: p. 665 OBJ: 21.1.2

4. ANS: B DIF: L1 REF: p. 668 OBJ: 21.1.4

5. ANS: C DIF: L1 REF: p. 669 OBJ: 21.1.5

6. ANS: C DIF: L1 REF: p. 665 OBJ: 21.1.2

7. ANS: A DIF: L1 REF: p. 665 OBJ: 21.1.2

8. ANS: D DIF: L1 REF: p. 665 OBJ: 21.1.2

9. ANS: E DIF: L1 REF: p. 667 OBJ: 21.1.3

10. ANS: B DIF: L1 REF: p. 678 OBJ: 21.3.1

11. ANS: G DIF: L1 REF: p. 356 OBJ: 12.1.2

12. ANS: H DIF: L1 REF: p. 357 OBJ: 12.1.2

13. ANS: F DIF: L1 REF: p. 357 OBJ: 12.1.2

14. ANS: E DIF: L1 REF: p. 369 OBJ: 12.3.1

15. ANS: C DIF: L1 REF: p. 369 OBJ: 12.3.1

16. ANS: D DIF: L1 REF: p. 372 OBJ: 12.3.2

17. ANS: A DIF: L1 REF: p. 372 OBJ: 12.3.2

18. ANS: B DIF: L1 REF: p. 372 OBJ: 12.3.2

19. ANS: E DIF: L1 REF: p. 323 OBJ: 11.1.2

20. ANS: A DIF: L1 REF: p. 323 OBJ: 11.1.2

21. ANS: B DIF: L1 REF: p. 323 OBJ: 11.1.2

22. ANS: C DIF: L1 REF: p. 323 OBJ: 11.1.3

23. ANS: D DIF: L1 REF: p. 325 OBJ: 11.1.3

24. ANS: D DIF: L1 REF: p. 332 OBJ: 11.2.1

25. ANS: C DIF: L1 REF: p. 336, p. 337
OBJ: 11.2.1

26. ANS: B DIF: L1 REF: p. 333 OBJ: 11.2.1

27. ANS: A DIF: L1 REF: p. 333 OBJ: 11.2.2

28. ANS: C DIF: L1 REF: p. 294 OBJ: 10.1.3

29. ANS: B DIF: L1 REF: p. 294, p. 295
OBJ: 10.1.3, 10.1.4

30. ANS: A DIF: L1 REF: p. 300 OBJ: 10.2.2

31. ANS: C DIF: L1 REF: p. 290 OBJ: 10.1.2

32. ANS: A DIF: L1 REF: p. 290 OBJ: 10.1.2

33. ANS: B DIF: L1 REF: p. 290 OBJ: 10.2.1

34. ANS: E DIF: L1 REF: p. 300 OBJ: 10.2.2

35. ANS: D DIF: L1 REF: p. 305 OBJ: 10.3.1

36. ANS: F DIF: L1 REF: p. 309 OBJ: 10.3.2

MULTIPLE CHOICE

37. ANS: C DIF: L1 REF: p. 665 OBJ: 21.1.2

38. ANS: B DIF: L1 REF: p. 667 OBJ: 21.1.3

39. ANS: D DIF: L1 REF: p. 667 OBJ: 21.1.3

40. ANS: B DIF: L1 REF: p. 667 OBJ: 21.1.3

41. ANS: C DIF: L1 REF: p. 668 OBJ: 21.1.4

42. ANS: B DIF: L2 REF: p. 668 OBJ: 21.1.4

43. ANS: A DIF: L1 REF: p. 669 OBJ: 21.1.5

44. ANS: A DIF: L2 REF: p. 675 OBJ: 21.2.3

45. ANS: A DIF: L1 REF: p. 675, p. 676
OBJ: 21.2.4

46. ANS: A DIF: L2 REF: p. 681 OBJ: 21.3.3

47. ANS: D DIF: L2 REF: p. 681 OBJ: 21.3.3

Summative Review EP 5

summative review ep 5

Matching

Match each item with the correct statement below.
a. calorimeter d. enthalpy
b. calorie e. specific heat
c. joule f. heat capacity


____ 1. quantity of heat needed to raise the temperature of 1 g of water by 1 C

____ 2. SI unit of energy

____ 3. quantity of heat needed to change the temperature of 1 g of a substance by 1 C

____ 4. quantity of heat needed to change the temperature of an object by 1 C

____ 5. device used to measure the heat absorbed or released during a chemical or physical process

____ 6. heat content of a system at constant pressure

Match each item with the correct statement below.
a. heat of reaction d. heat of fusion
b. heat of formation e. heat of solution
c. Hess's law of heat summation


____ 7. the enthalpy change for a chemical reaction exactly as it is written

____ 8. the enthalpy change caused by dissolving a substance

____ 9. the energy required to melt a solid at its melting point

____ 10. the change in enthalpy that accompanies the formation of a compound from its elements

____ 11. states that if you add two or more thermochemical equations to give a final equation, you can also add the heats of reaction to give the final heat of reaction

Match each item with the correct statement below.
a. activated complex d. activation energy
b. reaction rate e. free energy
c. inhibitor


____ 12. the minimum energy colliding particles must have in order to react

____ 13. arrangement of atoms at the peak of an energy barrier

____ 14. the number of atoms, ions, or molecules that react in a given time to form products

____ 15. a substance that interferes with a catalyst

____ 16. energy available to do work

Match each item with the correct statement below.
a. spontaneous reaction d. reaction mechanism
b. entropy e. elementary reaction
c. chemical equilibrium


____ 17. when the forward and reverse reactions take place at the same rate

____ 18. a reaction that releases free energy

____ 19. the measure of disorder

____ 20. Reactants are converted to products in a single step.

____ 21. includes all elementary reactions of a complex reaction

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.

____ 22. When energy is changed from one form to another, ____.
a. some of the energy is lost entirely
b. all of the energy can be accounted for
c. a physical change occurs
d. all of the energy is changed to a useful form


____ 23. If heat is released by a chemical system, an equal amount of heat will be ____.
a. absorbed by the surroundings c. released by the surroundings
b. absorbed by the universe d. released by the universe


____ 24. A process that absorbs heat is a(n) ____.
a. endothermic process c. exothermic process
b. polythermic process d. ectothermic process


____ 25. The quantity of heat required to change the temperature of 1 g of a substance by 1 C is defined as ____.
a. a joule c. a calorie
b. specific heat d. density


____ 26. A piece of candy has 5 Calories (or 5000 calories). If it could be burned, leaving nothing but carbon dioxide and water, how much heat would it give off?
a. 500 calories c. 5000 joules
b. 5 kilocalories d. Not enough information is given.


____ 27. How many joules are in 148 calories? (1 cal = 4.18 J)
a. 6.61 J c. 148 J
b. 35.4 J d. 619 J


____ 28. What is the specific heat of a substance if 1560 cal are required to raise the temperature of a 312-g sample by 15 C?
a. 0.033 c. 0.99
b. 0.33 d. 1.33


____ 29. When 45 g of an alloy, at 25 C, are dropped into 100.0 g of water, the alloy absorbs 956 J of heat. If the final temperature of the alloy is 37 C, what is its specific heat?
a. 0.423 c. 9.88
b. 1.77 d. 48.8


____ 30. A chunk of ice whose temperature is –20 C is added to an insulated cup filled with water at 0 C. What happens in the cup?
a. The ice melts until it reaches the temperature of the water.
b. The water cools until it reaches the temperature of the ice.
c. Some of the water freezes, so the chunk of ice gets larger.
d. none of the above


____ 31. What is the standard heat of reaction for the following reaction?
Zn(s) + Cu (aq) Zn (aq) + Cu(s)
( H for Cu = +64.4 kJ/mol; H for Zn = –152.4 kJ/mol)
a. 216.8 kJ released per mole c. 88.0 kJ absorbed per mole
b. 88.0 kJ released per mole d. 216.8 kJ absorbed per mole


____ 32. When 1.0 g of solid NaOH ( H = –445.1 kJ/mol) dissolves in 10 L of water, how much heat is released?
a. 445.1 kJ c. 11.1 J
b. 405.1 kJ d. 11.1 kJ


____ 33. If sulfur dioxide and oxygen can be made into sulfur trioxide, what is the reverse reaction?
a. 2SO 2SO + O c. 2SO + O 2SO
b. SO + O SO d. SO + 2SO 3S + 4O


____ 34. What is the equilibrium constant for the following reaction?
C + O CO
a. c.
b. d.


____ 35. If a reaction has an equilibrium constant just greater than 1, what type of reaction is it?
a. irreversible c. reversible, favoring products
b. spontaneous d. reversible, favoring reactants


summative review ep 5
Answer Section

MATCHING

1. ANS: B DIF: L1 REF: p. 507 OBJ: 17.1.3

2. ANS: C DIF: L1 REF: p. 507 OBJ: 17.1.3

3. ANS: E DIF: L1 REF: p. 508 OBJ: 17.1.3

4. ANS: F DIF: L1 REF: p. 508 OBJ: 17.1.3

5. ANS: A DIF: L1 REF: p. 511 OBJ: 17.2.1

6. ANS: D DIF: L1 REF: p. 511 OBJ: 17.2.1

7. ANS: A DIF: L1 REF: p. 514 OBJ: 17.2.2

8. ANS: E DIF: L1 REF: p. 525 OBJ: 17.3.1

9. ANS: D DIF: L1 REF: p. 520 OBJ: 17.3.1

10. ANS: B DIF: L1 REF: p. 530 OBJ: 17.4.1

11. ANS: C DIF: L1 REF: p. 527 OBJ: 17.4.1

12. ANS: D DIF: L1 REF: p. 543 OBJ: 18.1.1

13. ANS: A DIF: L1 REF: p. 544 OBJ: 18.1.1

14. ANS: B DIF: L1 REF: p. 542 OBJ: 18.1.1

15. ANS: C DIF: L1 REF: p. 547 OBJ: 18.1.2

16. ANS: E DIF: L1 REF: p. 566 OBJ: 18.4.1

17. ANS: C DIF: L1 REF: p. 550 OBJ: 18.2.1

18. ANS: A DIF: L1 REF: p. 567 OBJ: 18.4.1

19. ANS: B DIF: L1 REF: p. 569 OBJ: 18.4.2

20. ANS: E DIF: L1 REF: p. 578 OBJ: 18.5.2

21. ANS: D DIF: L1 REF: p. 578 OBJ: 18.5.2

MULTIPLE CHOICE

22. ANS: B DIF: L1 REF: p. 506 OBJ: 17.1.1

23. ANS: A DIF: L1 REF: p. 506 OBJ: 17.1.1

24. ANS: A DIF: L1 REF: p. 506 OBJ: 17.1.2

25. ANS: B DIF: L1 REF: p. 507 OBJ: 17.1.2

26. ANS: B DIF: L2 REF: p. 507 OBJ: 17.1.2

27. ANS: D DIF: L1 REF: p. 507 OBJ: 17.1.3

28. ANS: B DIF: L1 REF: p. 509, p. 510
OBJ: 17.1.3

29. ANS: B DIF: L2 REF: p. 509 OBJ: 17.1.3

30. ANS: C DIF: L2 REF: p. 512 OBJ: 17.2.1

31. ANS: A DIF: L2 REF: p. 516 OBJ: 17.2.2

32. ANS: D DIF: L2 REF: p. 526 OBJ: 17.3.2

33. ANS: A DIF: L2 REF: p. 549 OBJ: 18.2.1

34. ANS: B DIF: L1 REF: p. 556 OBJ: 18.2.3

35. ANS: C DIF: L1 REF: p. 556 OBJ: 18.2.3

sample test ep 4

review sheetep 4

Matching

Match each item with the correct statement below.
a. molar volume
b. molar mass
c. atomic mass


____ 1. the number of grams of an element that is numerically equal to the atomic mass of the element in amu

____ 2. the mass of a mole of any element or compound

____ 3. the volume occupied by a mole of any gas at STP

Match each item with the correct statement below.
a. representative particle d. percent composition
b. mole e. standard temperature and pressure
c. Avogadro's number f. empirical formula


____ 4. the number of representative particles of a substance present in 1 mole of that substance

____ 5. an atom, an ion, or a molecule, depending upon the way a substance commonly exists

____ 6. the SI unit used to measure amount of substance

____ 7. 0 C and 1 atm

____ 8. the percent by mass of each element in a compound

____ 9. the smallest whole number ratio of the atoms in a compound

Match each item with the correct statement below.
a. product d. balanced equation
b. reactant e. skeleton equation
c. chemical equation


____ 10. a chemical equation that does not indicate relative amounts of reactants and products

____ 11. a new substance formed in a chemical reaction

____ 12. a starting substance in a chemical reaction

____ 13. a concise representation of a chemical reaction

____ 14. an equation in which each side has the same number of atoms of each element

Match each item with the correct statement below.
a. activity series of metals c. combustion reaction
b. single-replacement reaction d. decomposition reaction


____ 15. a reaction in which a single compound is broken down into simpler substances

____ 16. a reaction in which oxygen reacts with another substance, often producing heat or light

____ 17. a reaction in which the atoms of one element replace the atoms of a second element in a compound

____ 18. a list of metals in order of decreasing reactivity

Match each item with the correct statement below.
a. actual yield e. limiting reagent
b. percent yield f. mass
c. theoretical yield g. number of molecules
d. excess reagent h. volume


____ 19. This quantity can always be used in the same way as moles when interpreting balanced chemical equations.

____ 20. This is conserved only in reactions where the temperature is constant and the number of moles of gaseous reactants is the same as that of gaseous products.

____ 21. This is conserved in every ordinary chemical reaction.

____ 22. the reactant that determines the amount of product that can be formed in a reaction

____ 23. the maximum amount of product that could be formed from given amounts of reactants

____ 24. the reactant that is not completely used up in a reaction

____ 25. the amount of product formed when a reaction is carried out in the laboratory

____ 26. the ratio of the actual yield to the theoretical yield

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.

____ 27. How many moles of tungsten atoms are in 4.8 10 atoms of tungsten?
a. 8.0 10 moles c. 1.3 10 moles
b. 8.0 10 moles d. 1.3 10 moles


____ 28. How many molecules are in 2.10 mol CO ?
a. 2.53 10 molecules c. 3.49 10 molecules
b. 3.79 10 molecules d. 1.26 10 molecules


____ 29. What is true about the molar mass of chlorine gas?
a. The molar mass is 35.5 g.
b. The molar mass is 71.0 g.
c. The molar mass is equal to the mass of one mole of chlorine atoms.
d. none of the above


____ 30. What is the number of moles in 432 g Ba(NO ) ?
a. 0.237 mol c. 1.65 mol
b. 0.605 mol d. 3.66 mol


____ 31. What is the volume, in liters, of 0.500 mol of C H gas at STP?
a. 0.0335 L c. 16.8 L
b. 11.2 L d. 22.4 L


____ 32. What is the density at STP of the gas sulfur hexafluoride, SF ?
a. 0.153 g/L c. 3270 g/L
b. 6.52 g/L d. 3.93 10 g/L


____ 33. What is the percent composition of chromium in BaCrO ?
a. 4.87% c. 20.5%
b. 9.47% d. 25.2%


____ 34. Which of the following compounds have the same empirical formula?
a. CO and SO c. C H and C H
b. C H and C H d. C H and C H


____ 35. What are the coefficients that will balance the skeleton equation below?
AlCl + NaOH Al(OH) NaCl
a. 1, 3, 1, 3 c. 1, 1, 1, 3
b. 3, 1, 3, 1 d. 1, 3, 3, 1


____ 36. What are the coefficients that will balance the skeleton equation below?
N + H NH
a. 1, 1, 2 c. 3, 1, 2
b. 1, 3, 3 d. 1, 3, 2


____ 37. When the equation KClO (s) KCl(s) + O (g) is balanced, the coefficient of KClO3 is ____.
a. 1 c. 3
b. 2 d. 4


____ 38. How many moles of aluminum are needed to react completely with 1.2 mol of FeO?
2Al(s) + 3FeO(s)  3Fe(s) + Al O (s)
a. 1.2 mol c. 1.6 mol
b. 0.8 mol d. 2.4 mol


____ 39. When iron rusts in air, iron(III) oxide is produced. How many moles of oxygen react with 2.4 mol of iron in the rusting reaction?
4Fe(s) + 3O (g)  2Fe2O (s)
a. 1.2 mol c. 2.4 mol
b. 1.8 mol d. 3.2 mol


____ 40. At STP, how many liters of oxygen are required to react completely with 3.6 liters of hydrogen to form water?
2H (g) + O (g)  2H O(g)
a. 1.8 L c. 2.0 L
b. 3.6 L d. 2.4 L


____ 41. The equation below shows the decomposition of lead nitrate. How many grams of oxygen are produced when 11.5 g NO is formed?

a. 1.00 g c. 2.88 g
b. 2.00 g d. 32.0 g


review sheet
Answer Section

MATCHING

1. ANS: C DIF: L1 REF: p. 294 OBJ: 10.1.3

2. ANS: B DIF: L1 REF: p. 294, p. 295
OBJ: 10.1.3, 10.1.4

3. ANS: A DIF: L1 REF: p. 300 OBJ: 10.2.2

4. ANS: C DIF: L1 REF: p. 290 OBJ: 10.1.2

5. ANS: A DIF: L1 REF: p. 290 OBJ: 10.1.2

6. ANS: B DIF: L1 REF: p. 290 OBJ: 10.2.1

7. ANS: E DIF: L1 REF: p. 300 OBJ: 10.2.2

8. ANS: D DIF: L1 REF: p. 305 OBJ: 10.3.1

9. ANS: F DIF: L1 REF: p. 309 OBJ: 10.3.2

10. ANS: E DIF: L1 REF: p. 323 OBJ: 11.1.2

11. ANS: A DIF: L1 REF: p. 323 OBJ: 11.1.2

12. ANS: B DIF: L1 REF: p. 323 OBJ: 11.1.2

13. ANS: C DIF: L1 REF: p. 323 OBJ: 11.1.3

14. ANS: D DIF: L1 REF: p. 325 OBJ: 11.1.3

15. ANS: D DIF: L1 REF: p. 332 OBJ: 11.2.1

16. ANS: C DIF: L1 REF: p. 336, p. 337
OBJ: 11.2.1

17. ANS: B DIF: L1 REF: p. 333 OBJ: 11.2.1

18. ANS: A DIF: L1 REF: p. 333 OBJ: 11.2.2

19. ANS: G DIF: L1 REF: p. 356 OBJ: 12.1.2

20. ANS: H DIF: L1 REF: p. 357 OBJ: 12.1.2

21. ANS: F DIF: L1 REF: p. 357 OBJ: 12.1.2

22. ANS: E DIF: L1 REF: p. 369 OBJ: 12.3.1

23. ANS: C DIF: L1 REF: p. 369 OBJ: 12.3.1

24. ANS: D DIF: L1 REF: p. 372 OBJ: 12.3.2

25. ANS: A DIF: L1 REF: p. 372 OBJ: 12.3.2

26. ANS: B DIF: L1 REF: p. 372 OBJ: 12.3.2

MULTIPLE CHOICE

27. ANS: B DIF: L2 REF: p. 290, p. 291
OBJ: 10.1.2

28. ANS: D DIF: L2 REF: p. 291, p. 292
OBJ: 10.1.2

29. ANS: B DIF: L2 REF: p. 294 OBJ: 10.1.3

30. ANS: C DIF: L2 REF: p. 299 OBJ: 10.2.1

31. ANS: B DIF: L2 REF: p. 301 OBJ: 10.2.2

32. ANS: B DIF: L2 REF: p. 302 OBJ: 10.2.2

33. ANS: C DIF: L2 REF: p. 307 OBJ: 10.3.1

34. ANS: B DIF: L1 REF: p. 309 OBJ: 10.3.2

35. ANS: A DIF: L1 REF: p. 324, p. 325
OBJ: 11.1.3

36. ANS: D DIF: L1 REF: p. 324, p. 325
OBJ: 11.1.3

37. ANS: B DIF: L1 REF: p. 327 OBJ: 11.1.3

38. ANS: B DIF: L1 REF: p. 359, p. 360
OBJ: 12.2.1

39. ANS: B DIF: L2 REF: p. 359, p. 360
OBJ: 12.2.1

40. ANS: A DIF: L1 REF: p. 363, p. 364, p. 365, p. 366
OBJ: 12.2.2

41. ANS: B DIF: L2 REF: p. 360, p. 361, p. 362
OBJ: 12.2.2

Chemistry Bonus

I need a problem based powerpoint where you do three problems and have three solutions.

ep 4 it can be on chapter 11 or 12

ep 5 it can be on chapter 17 or 18

ep 6 it can be on chapter 21 or 12

deadline december 13

AC Chemistry Assignments Pack 2

EP 4-- problem set 2: Ch 10. write questions, #30, 31, 34-37.
Reading Ch 10.2-10.4 Prelab Ch 10
Notebook Check Wednesday
Quiz 2 on Wednesday on Empirical formulae, percent composition, and mole conversions

EP 5--Problem set 2: Ch 17 write questions
Reading Ch 17.2-17.3 Pre lab Ch 17.3
Notebook Check Tuesday
Quiz 1 on phase change diagrams, enthalpy calculation, heat of vaporization and heat of fusion

ep 6 Problem set 1: Ch 21 write questions. Reading Ch 21.3 on Electrochemical equations
notebook check Friday
quiz 1 on galvanic cells, electrodes, and fuel cells

check Calendar on bottom for more details.

Make-up exams for First Semester Final due Friday November 14