CHEM_FINAL_EXAM_PRACTICE_TEST.docx.pdf

Practice Exam questions:

1. What is 89.5 lbs in grams ( 454 g = 1.00 lbs)?

a. 197g

b. 507g

c. 4.06x104 g

d. 41.0 g

e. 1.97x106g

2. If the appropriate dose for a medication is 2.6 mg per kg body weight, what is the correct

dose for 177lb man? (0.454 kg = 1.00 lb)

a. 210 mg

b. 460 mg

c. 1.0x103 mg

d. 6.7 mg

e. 150 mg

3. What is the height in meters of a person who is 68 inches tall? (1.00 inch = 2.54 cm)

a. 16 m

b. 0.17 m

c. 4.3 m

d. 1.7 m

e. 2.6 m

4. A metal cube having a mass of 100.0 grams and a density of 11.1 g/ml is placed in a

graduated cylinder that contains 30.00 ml of water. What is the final water level?

a. 9.01ml

b. 41.10 ml

c. 32.70 ml

d. 133 ml

e. 39.01ml

5. What is the value of (167.62/12.05) + 13.5 rounded to the correct number of significant

figures?

a. 27.410

b. 27.41

c. 27.4

d. 27.

e. 3 x101

6. Which of the following numbers has 4 significant figures?

a. 0.004309

b. 0.0430

c. 0.0431

d. 0.43980

e. 0.43090

7. Which of the following represents a chemical change?

a. Steam condenses to water droplets.

b. Sea water is desalinated.

c. Sodium bicarbonate and HCl forms salt, carbon dioxide and water.

d. Sugar crystals form.

e. Lead melting at 327.5 oC

8. The ion 52Cr+3 contains:

a. 24 protons 52 neutrons 27 electrons

b. 24 protons 28 neutrons 27 electrons

c. 24 protons 28 neutrons 21 electrons

d. 28 protons 24 neutrons 21 electrons

e. 28 protons 24 neutrons 27 electrons

9. How many neutrons does the sulfur isotope 33S contain?

a. 8

b. 16

c. 15

d. 17

e. 33

10. What is the charge on the stable ion formed by the fluorine (F) atom?

a. +2

b. +1

c. 0

d. -1

e. -2

11. What is the charge on the stable ion formed by the Arsenic (As) atom?

a. +3

b. +2

c. +1

d. -2

e. -3

12. What is the charge on the stable ion formed by the iodine (I) atom?

a. +2

b. +1

c. 0

d. -1

e. -2

13. The element Li is best classified as a

a. alkali metal

b. alkaline earth metal

c. transition metal

d. halogens

e. noble gas

14. The element Ba is best classified as a

a. alkali metal

b. alkaline earth metal

c. transition metal

d. halogens

e. noble gas

15. The element Ne is best classified as a

a. alkali metal

b. alkaline earth metal

c. transition metal

d. halogens

e. noble gas

16. The formula for the simplest ionic compound of B and F is:

a. B2F3

b. BF

c. BF3

d. BF2

e. B2F

17. The formula for the simplest ionic compound of Be and S is:

a. Be2S3

b. Be3S2

c. BeS2

d. BeS

e. Be2S

Match the Name With the Formula:

18. sulfide a. S-2

19. sulfate b. SO2-2

20. sulfiite c. SO4-2

21. bisulfate d. SO3-2

e. HSO4-1

22. Choose the formula of sodium carbonate:

a. Na(CO3)2

b. NaHCO4

c. Na2CO2

d. NaHCO3

e. Na2CO3

23. Choose the formula of rubidium sulfate:

a. RbSO4

b. Rb3(SO4)2

c. Rb2SO4

d. Rb3(SO2)2

e. Rb(SO3)2

24. An element with the Lewis dot symbol shown below is most likely to be found in which

column?

a. III

b. IV

c. V

d VI

e. VII

25. Use the electron dot structure of As (column VA) to predict how many H atoms will bond

to it. Choose the correct formula:

a. AsH2

b. AsH3

c. AsH4

d. AsH

e. As2H3

26. Draw the Lewis dot structure for H2S. How many non-bonding valence electrons (= “lone

pair electrons” are on the S atom?

a. one electron

b. two electrons (1 pair)

c. three electrons

d. four electrons (2 pairs)

e. six electrons (3 pairs)

27. Draw the Lewis dot structure for H-N-O. In the molecule HNO, the N will have:

a. one single bond, one double bond, and one lone pair

b. two single bonds and two lone pairs

c. two double bonds and no lone pairs

d. three single bonds and one lone pair

e one double bond and two lone pairs.

28. Given the general shape below, draw the Lewis dot structure for H2CO. The oxygen in

this molecule will have:

a. a double bond and a lone pair

b. a triple bond and a lone pair

c. a single bond and three lone pairs

d. a double bond and two lone pairs

e. a single bond and two lone pairs

29. In H-C-N the bond between the C and the N will be a ____________ bond, and the N

will have ______ lone pairs.

a. single, one

b. double, one

c. triple, one

d. double, two

e. triple, two

30. How much heat is required to raise the temperature of 125g of water from 22.5 oC to

100.0 oC? (specific heat of water is 1.00 cal/goC)

a. 9380 cal

b. 2810 cal

c. 12,500 cal

d. 3330 cal

e. 2250 cal

31. How much heat is required to melt 2.10 lbs of ice at 0 oC? (Heat of melting for ice is

79.7 cal/g, 1.00 lb = 454g)

a. 159 cal

b. 3.62 x 104 cal

c. 7.60 x 104 cal

d 1.72 x 104 cal

e. 125 cal

32. Convert 19 oC to Farenheit.

a. 292 oF

b. 42.6 oF

c. 91.8 oF

d. 41.0 oF

e. 66.2 oF

33. Which of the following corresponds to a 42He nucleus?

a. α particle

b. +β particle

c. - β particle

d. γ radiation

34. The radioactivity with the highest penetrating power is:

a. α particle

b. +β particle

c. - β particle

d. γ radiation

35. What is the missing product of the following nuclear reaction:

239

231

235

36. A certain radioactive element that has a half-life of 15.0 s. How much of a 100. mg

sample will remain after 40.0 s?

a. 15.7 mg

b. 2.67 mg

c. 37.5 mg

d. 14.1 mg

e. 2.50 mg

37. What is the formula of Tin(II)perchlorate?

a. Sn(ClO4)2

b. Sn(ClO3)2

c. Sn(ClO2)2

d. SnClO4

e. SnClO2

38. What is the formula of Cuprous Chloride?

a. CuCl2

b. CuCl3

c. CuCl

d. Cu2Cl

e CuCl4

1. How many phosphorus atoms are there in 0.323 moles of phosphorus?

a. 8.16 x 1023 atoms

b. 6.86 x 1022 atoms

c. 1.94 x 1023 atoms

d. 4.50 x 1022 atoms

e. 1.16 x 1022 atoms

2. Determine the number of moles in 1.70x1023 atoms of aluminum.

a. 0.37 moles

b. 0.28 moles

c. 0.56 moles

d. 0.72 moles

e. 0.88 moles

3. How many moles of C3H8 are there in 150 grams of C3H8?

a. 1.28 moles

b. 0.293 mole

c. 3.41 moles

d. 0.480 mole

e. 4.03 moles

4. What is the mass of 0.216 mole of C8H9O4?

a. 86.9 g

b. 782 g

c. 169 g

d. 56.4 g

e. 36.5 g

Balance the equations with the SMALLEST WHOLE NUMBER COEFFICIENTS possible. In

each case choose the answer that equals the sum of the coefficients in the balanced equation.

5. Ag + H2S + O2 ---> Ag2S + H2O

a. 9

b. 10

c. 11

d. 12

e. 14

6. PtCl4 + XeF2 ---> PtF6 + ClF + Xe

a. 16

b. 22

c. 24

d. 26

e. 32

7. Cr2(SO4)3 + RbOH ---> Cr(OH)3 + Rb2SO4

a. 10

b. 12

c. 13

d. 14

e. 15

8. Classify the reactions as one of the following kinds.

2 HBr + Ba(OH)2------> BaBr2 + 2 H2O

a. combination

b. single replacement

c. decomposition

d. double displacement

9. Classify the reactions as one of the following kinds.

Zn + 2 AgNO3 ------>Zn(NO3)2 + 2 Ag

a. combination

b. single replacement

c. decomposition

d. double displacement

10. Consider the following reaction at equilibrium:

CoCl4-2 (blue) + 6H2O(l)  4Cl- + Co(H2O)6+2(pink) + heat

Which of the following will cause the mixture to turn blue?

1. Add heat (place in a hot water bath).

2. Add HCl or NaCl

3. Add water.

a. 1 and 3

b. 1 and 2

c. 2

d. 2 and 3

e. 1, 2 and 3

11. For the system H2 (g) + CO2 (g)  H2O (g) + CO (g) at equilibrium, the addition of H2 (g)

would cause (according to LeChatelier's principle):

a. only more H2O (g) to form

b. only more CO (g) to form

c. more H2O (g) and CO (g) to form

d. only more CO2 (g) to form

e. no change in amounts of products or reactant

12. Consider the following systems at equilibrium. Which reponse includes all the stresses

listed that would shift the equilibrium to the right (favor the forward reaction?)

Equilibrium Stress

1. CO (g) + Cl2 (g)  COCl2 (g) add Cl2

2. CO (g) + Cl2 (g)  COCl2 (g) remove COCl2

3. PCl3 (g) + Cl2  PCl5 (g) remove PCl3

a. 1

b. 3

c. 1, 2

d. 2, 3

e. another one or another combination

13. What is the mass of 0.216 mole of C8H9O4?

a. 86.9 g

b. 782 g

c. 169 g

d. 56.4 g

e. 36.5 g

Consider the following reaction for the next two questions:

2 KMnO4 + 5 H2SO3 ---> 2 MnSO4 + K2SO4 + 2 H2SO4 + 3 H2O

14. How many moles of MnSO4 can be made from 1.5 moles of H2SO3?

a.. 0.75

b. 3.0

c. 3.75

d. 1.5

e. 0.60

15. How many grams of MnSO4 can be produced from the complete reaction of 10.0 g of

KMnO4?

a. 6.45 g

b. 7.80 g

c. 9.56 g

d. 9.89 g

e. 10.3 g

Refer to the following diagram for the following two questions:

16. The point labeled "C" is the

a. energy content of products

b. energy content of reactants

c. activation energy for the forward reaction

d. activation energy for the reverse reaction

e. net change in energy for the reaction

17. The arrow labeled "D" represents the

a. energy content of products

b. energy content of reactants

c. activation energy for the forward reaction

d. activation energy for the reverse reaction

e. net change in energy for the reaction

18. Which of the following is false for an Endothermic reaction?

a. ΔH = +

b. The reaction absorbs heat

c. The reactants have a higher heat content than the products

d. The reaction can be spontaneous.

19. Which of the following will increase the rate of the forward (left to right) reaction:

A(s) + B(g)  C ?

1. Increase the temperature

2. Add more B

3. Remove C

4. Grind A to a powder

a. 1, 2, 4

b. 1, 2, 3

c. 3, 4

d. 2, 3, 4

e. 1, 4

Important Information:

STP = 273K and 1 atm

1 atm = 760 torr

R = 0.0821 (L)(atm)/(mol)(K)

20. A gas occupies 1.75 liters and exerts a pressure of 730 torr at a certain temperature. If

the temperature remains constant, what volume must it occupy to exert a pressure of

820 torr?

a. 0.641 L

b. 1.56 L

c. 3.44 L

d. 0.291 L

e. 1.08 L

21. A sample of a gas occupies 3.24 liters at 25.0oC and 0.966atm. What volume does it

occupy at 273K and 1.00 atm?

a. 2.87 L

b. 2.96 L

c. 3.07 L

d. 3.42 L

e. 3.66 L

22. Which of the following is an endothermic process?

a. Burning wood.

b. Melting ice.

c. Condensing steam to liquid water.

d. H2 + O2  H2O

e. Both b and c are endothermic.

23. What volume will 12.40 grams of CO2 occupy at STP?

a. 6.31 L

b. 8.46 L

c. 4.42 L

d. 11.7 L

e. 9.68 L

24. What will the partial pressure of oxygen be in a mixture of gasses that is 15% oxygen,

80% nitrogen, 4% carbon dioxide and 1% water vapor, and has a total pressure of 820

torr?

a. 723 torr

b. 15 torr

c. 123 torr

d. 154 torr

e. 145 torr

25. When Ca(NO3)2 dissolves in water it produces the ions:

a. Ca2+ and (NO3)22-

b. Ca1+ and (NO3)21-

c. Ca2+ and 2NO31-

d. CaNO31+ and NO31-

e. CaNO32+ and NO32-

26. Which is the net ionic equation for Zn(s) + CuCl2(aq)  Cu(s) + ZnCl2(aq)

a. Cu2+(aq) + 2Cl-(aq)  Zn2+(aq) + 2Cl-(aq)

b. Zn(s) + 2Cl-(aq) ZnCl2(aq)

c. Zn(s) + CuCl2(aq)  Zn2+(aq)+ 2Cl-(aq)

d. Zn(s) + Cu2+(aq) Zn2+ (aq) + Cu(s)

e. Cu2+(aq) + 2Cl-(aq)  CuCl2(aq)

27. Which of the following is not true?

a. Exothermic reactions have ΔH = negative

b. Exothermic reactions give off heat to the surroundings.

c. Boiling water is an exothermic process.

d. Heat is a product of exothermic processes.

e. Combustion is exothermic process.

28. A sample of gas originally at 25.0 oC and a pressure of 1.00 atm, has its temperature

doubled to 50.0 oC, while the volume is kept constant. What is the new pressure?

a. 2.00 atm

b. 1.08 atm

c. 0.845 atm

d. 0.500 atm

e. 1.74 atm

29. Which is not a part of the Kinetic – Molecular theory?

a. Gas particles are in constant, random motion.

b. Gas particles can exert attractive forces on each other.

c. Gas particles are infinitesimal, so the volume of the gas is mostly empty space.

d. Forces between particles are negligible – collisions are the only interactions.

e. Temperature is a measure of the Kinetic Energy of the gas.

30. The partial pressure of CO2 in alveoli of the lungs is 42.5 torr, what is that pressure in

atm?

a. 17.9

b. 2.25

c. 1.44x10-1

d. 5.59x10-2

e. 7.63x10-3

31. If 5.81g of a gas occupies 1.30L at STP, what is its molar mass?

a. 36.0 g/mol

b. 133 g/mol

c. 217. g/mol

d. 44.0 g/mol

e. 100. g/mol

Match the Structure to the correct molecular shape (some shapes may match more than one

molecule)

32. 33.

34. 35.

a. tetrahedral b. bent

c. trigonal planar d. pyramidal

e. linear

36. Which of the above will be polar?

a. SO2 and H2CO

b. SO2, H2S and H2CO

c. SiH4, SO2

d. H2S and SiH4

e. H2S, H2CO and SiH4

37. Which of the following is polar?

a. H2

b. CH4

c. HF

d. P4

e. Cl2

38. Which of the following will have hydrogen bonds?

H2O, H2S, HCl, CH3OH

a. H2S and HCl

b. H2O and HCl

c. H2O, HCl and CH3OH

d. H2O, CH3OH

e. H2O, H2S and HCl

1. Give the following in order of increasing water solubility (least to most soluble).

1. CH3CH2OH 2. CH3CH33. CH3-O-CH2CH3

a. 1, 2, 3

b. 2, 3, 1

c. 3, 1, 2

d. 3, 2, 1

e. 2, 1, 3

2. Which of the following will be least soluble in the nonpolar solvent hexane (C6H14)?

a. I2

b. C12H26

c. NaCl

d. CH4

e. CH3CH2OCH2CH3

3. What is the percent by mass of ethanol, C2H5OH, of a solution of 47.5 g of C2H5OH in 850 g

of water?

a. 5.29%

b. 5.99%

c. 8.71%

d. 11.2%

e. 12.4%

4. Calculate the molarity of a solution that contains 60 g of sodium hydroxide in 750 ml of

solution. At. Wt. Na = 23, O = 16, H = 1.

a. 1.00 M

b. 2.00 M

c. 3.00 M

d. 1.80 M

e. 2.20 M

5. What is the concentration in ppm of Ca2+ if a solution that contains 12.5mg Ca2+ in

425mL of solution?

a. 53.1 ppm

b. 29.4 ppm

c. 34.0 ppm

d. .0294 ppm

e. 0.0340ppm

6. What is the concentration in Eq/L of Mg2+ in 500. mL or a solution that contains 22.0g of

Mg2+ ions?

a. 0.905 Eq/L

b. 1.81 Eq/L

c. 3.62 Eq/L

d. 7.24 Eq/L

e. 2.71 Eq/L

7. If 5.00 mL of a 1000. ppm solution is diluted to 250. mL, what is the new concentration?

a. 5.00 ppm

b. 50.0 ppm

c. 12.5 ppm

d. 20.0 ppm

e. 80.0 ppm

8. How many grams of NaCl would be dissolved in 2.50L to make a 0.100M solution?

a. 6.80g

b. 0.250g

c. 2.50g

d. 14.6g

e. 5.85g

9. Which one of the following pairs of acids and conjugate bases is incorrectly labeled or

incorrectly matched?

Acid Conjugate Base

a. HF F-

b. HClO ClO-

c. H2O OH-

d. NH4+NH2-

e. H3O+H2O

10. In the following reaction, identify the conjugate acids and bases:

HCN + H2O CN- + H3O+

Acids Bases

a. HCN, H2O CN- , H3O+

b. CN- , H3O+ HCN, H2O

c. H3O+ , HCN H2O, CN-

d. HCN, CN- H2O, H3O+

e. H2O, CN- H3O+ , HCN

11. What is the pH of a solution in which [H3O+] = 3.60 x 10-10 M?

a. 8.56

b. 5.44

c. 9.44

d. 4.56

e. 4.32

12. What is the pOH of the solution in the previous question?

a. 8.56

b. 5.44

c. 9.44

d. 4.56

e. 4.32

13. Which of the following is a strong acid?

a. HF

b. HCOOH

c. CH3CO2H

d. H3PO4

e. HNO3

14. Which of the following could you add to a solution of carbonic acid (H2CO3) to make a

buffer?

a. NaCl

b. NaHCO3

c. HCl

d. CO2

e. CH3CO2H

15. A Bronsted-Lowry base is defined as

a. an H+ acceptor

b. a OH- donor

c. an H+ donor

d. something that lowers pH

e. both a and b

16. A solution of morphine is listed as having a concentration 4mg/mL. If the dosage

required is 0.1mg/(kg body weight), how many mL of the solution should be given to an

84 kg patient?

a. 8.4 mL

b. 1.6 mL

c. 3.4 mL

d. 2.1 mL

e. 0.56 mL

17. Which is true of colloids, but false concerning true solutions?

a. Solute particles are small enough to pass through a filter

b. The solution is transparent.

c. Solute particles are small enough to not settle out of solution

d. Solute particles are small enough to go through a semipermeable membrane

e. Solute particles are large enough to diffract light

18. Choose the correct name for the following compound:

a. 1,2-dimethylethanal

b. dimethylpropanone

c. ethylpropanal

d. 2-methylbutanal

e. 2-methylbutanone

19. Choose the correct name for the following compound:

a. 1-butanol

b. 1-propanol

c. 1-butanal

d. 1-propanol

e. 2-methyl-1-butanol

20. Choose the correct name for the following compound:

a. methylcyclopentanol

b. 5-methylcyclopentanone

c. 2-methylcyclohexanone

d. 2-methylcyclopentanal

e. 3-methylcyclopentanone

21. Choose the correct name for the following compound:

CH3CH2CH CH

CH3

CH3CH2CH CH2

CH3

O CH CH

a. methylisopropyl ether

b. 3-methyl-2-butanol

c. 3-methyl-2-butanone

d. 2-methyl-3-butanol

e. 3-methyl-2-propanol

22. Choose the correct name for the following compound:

a. 2-pentanal

b. 3-pentanone

c. 2-propanone

d. 2-pentanone

e. 3-butanone

23. Choose the correct name for the following compound:

a. 3,3-dimethylbutanoic acid

b. 3,3-dimethylbutanal

c. 3,3-dimethylpropanoate

d. 3,3,3-trimethylpropanal

e. 2,2-dimethylpropanoic acid

H C

CH2C CH3

CH3

For 24 to 27 match the name with the correct structure:

a. b. c. d. e.

24. formaldehyde

25. acetone

26. formic acid

27. acetaldehyde

For 28 to 31 match the name with the correct functional group:

a. aldehyde

b. ketone

c. ether

d. alcohol

e. carboxylic acid

28.

R OH

29.

30.

31.

32. List the following in order of increasing boiling point (low to high):

1. pentanol 2. pentanone 3. hexanoic acid 4. diethyl ether

a. 1, 2, 3, 4

b. 4, 2, 1, 3

c. 2, 1, 4, 3

d. 1, 2, 4, 3

e. 2, 1, 3, 4

33. Which of the following will be the most water soluble?

a. 2-pentanone

b. 2-butanone

c. butanal

d. butane

e. butanoic acid

34. Which of the following alcohols is in alcoholic beverages?

a. methanol

b. ethanol

c. isopropanol

d. glycerol

e. ethylene glycol

35. Which of the following is an important component of many pharmaceuticals?

a. aniline

b. toluene

c. phenol

d. benzene

e. formic acid

ANSWER KEY:

1c, 2a, 3d, 4e, 5c

6a, 7c, 8c, 9d, 10d

11e, 12d, 13a, 14b, 15e

16c, 17d, 18a, 19c, 20d

21e, 22e, 23c, 24d, 25b

26b, 27c, 28d, 29c, 30a

31c, 32e, 33a, 34d, 35c

36a, 37a, 38c,

1c 2b 3c 4e 5c 6a 7b 8d 9b 10b 11c 12c 13e

14e 15c 16a , 17e 18c 19a 20b 21a 22b 23a 24c 25c 26d

27c 28b 29b 30d 31e 32b 33c 34a 35b 36b

1b 2c 3a 4b 5b 6c 7d 8d 9d 10c 11c 12d 13e

14b 15a 16d 17e 18d 19e 20c 21a 22d 23b 24c 25b 26e

27a 28d 29a 30b 31c 32b 33e 34b 35a

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