Exam 3 Special Code 111111 Name: __________________,________________ Petrovich, Fall 2010 print last print first

Student Number: ___________________(000######)

1. To what temperature must a substance be heated to contain 10 kJ/mol of thermal energy?

A) 1203 K B) 930 K C) 122 K D) -151 K

2. What is the concentration of Ne in a container at 40 C and 3.2 atmospheres of pressure?

A) 0.974 mol/L B) 0.124 mol/L C) 0.00123 mol/L D) 0.0096 mol/L

E) cannot be answered without volume.

3. A balloon is filled with 2.00 liters of gas at 300 K. What is the volume of the balloon at 100K?

A) 0.75 L B) 1.50 L C) 6.00 L D) 0.67 L

4. Choose the correct letter(A-D) to make a true statement. At 25 C, iodine (I2) is a solid and fluorine(F2) is a gas. This is because..

A) the thermal energy of I2 is greater than the thermal energy of F2.

B) the thermal energy of I2 is less than the thermal energy of F2.

C) the interaction energy of I2 is greater than the interaction energy of F2.

D) the interaction energy of I2 is less than the interaction energy of F2.

5. The pressure of the atmosphere is 755 mm Hg. What is the pressure in atmospheres of the Argon gas in the bulb if the height difference is 145 mm Hg?

A) 0.803 atm

B) 900 atm

C) 1.18 atm

D) 610 atm

6. How many moles of atoms are in 51.0 grams of S8?

A) 1.64x103 mol atoms B) 7.66 x 1024 mol atoms C) 1.59 mol atoms D) 12.7 mol atoms

7. In Phoenix, Arizona, a typical summer day is 40o C (104o F) with 10.% humidity. What is the vapor pressure of water in the air. The vapor pressure of water at 40o C is 55.3 mm Hg.

A) 5.5 mm Hg B) 4.0 mm Hg C) 55.3 mm Hg D) 22 mm Hg

Exam 3

Pre

ssure

(atm

)

1.00

0.75

0.50

0.25

10 20 30 40 50 60 70 80

Temperature (C)

90

A

B

C

D EF

G

H I

J

KLP

ress

ure

(atm

)

1.00

0.75

0.50

0.25

10 20 30 40 50 60 70 80

Temperature (C)

90

A

B

C

D EF

G

H I

J

KL

C HN

H

..H

H

C

H

H

C

H

H

H C H

H

NC

H

H

C

H

H

H

H

H

C H

H

CC

H

H

C

H

H

H

H

H

H

C HN

H

..H

H

C

H

H

H

A B

..

C D

Consider the phase diagram below for kryptonite for the next two questions. 8. Under what conditions is kryptonite a solid and gas, but NOT a liquid?

A) 70o C, 0.75 atm

B) 20o C, 0.25 atm

C) 30o C, 1.0 atm

D) 40o C, 0.50 atm

9. What process is occurring along arrow C?

A) freezing B) evaporation C) melting D) sublimation

10. Which compound below would have the LOWEST boiling point?

11. Which numeric combination (A-E) belongs together in the diagrams below?

A) 1,4,5 B) 2,3,6 C) 1,4,6 D) 2,4,6 E) 2,4,5

12. Select that pair in which hydrogen bonding will NOT occur.

A) I with I B) II with II C) I with II D) I with III E) No correct answer

1

2 H-Cl

5

temperature

43

F-F

6

H

H

H

H

CN

C

CC

C

H

H

H

H

H

CN

C

CC

C

H H

..H

..

F

FNF..

I II III

Exam 3

13. Choose the POLAR compounds from the choices below.

A) I & II B) III & IV C) I & III D) II & IV E) II & III

14. The unit cell of an ionic compound is shown below. The X atom occupies the center and edges of the unit cell. The Y atom occupies the faces of the unit cell. Choose the correct formula for the compound below.

A) X13Y6

B) X4Y3

C) X7Y4

D) X3Y4

15. In the band diagram shown below, which letter represents the valence band?

16. A weak, light metal would likely pack in this type of unit cell.

17. Choose the correct set of words to complete the statement below. ZnS is a(n) ____i_____ substance. SO3 is a(n) ____ii_____ substance. A) i=network covalent, ii=ionic B) i=network covalent, ii=molecular

C) i=metallic, ii=ionic D) i=ionic, ii=molecular

Energ

y

A

B

C

D

E

Energ

y C

A B C

Y

X

Exam 3

18. E for a system is 12.0 kJ. If the system is an endothermic reaction with a value of 17.5 kJ, what is the work component?

A) 5.5 kJ done by the system B) 5.5 kJ done on the system

C) 29.5 kJ done by the system D) 29.5 kJ done on the system

19. The reaction for the reaction of nitrogen with chlorine is shown below. Using bond

enthalpies, determine the value of H for the reaction. Be sure to draw Lewis structures of the products and reactants, to assist in determining the bond order.

N2 (g) + 3Cl2 (g) 2NCl3 (g)

Table of Bond Energies (kJ/mol)

A) -17 kJ/mol B) +889 kJ/mol C) -56 kJ/mol D) +467 kJ/mol E) +1067 kJ/mol

20. The reaction below is similar to the thermite reaction, but uses black iron ore instead of

red iron ore. What is the value of Ho when 94.0 grams of Fe is formed?

3Fe3O4 (s) + 8 Al (s) 4Al2O3 (s) + 9Fe (s) Ho = -3347.6 kJ/mol

A) -6.7 kJ B) -5.08x104 kJ C) -5.63x103 kJ D) -59.9 kJ E) -626 kJ

21. Liquid hydrogen peroxide decomposes according to the reaction:

2H2O2 (l) 2H2O (l) + O2 (g) Ho = -196 kJ/mol

What is the value of H for the reaction shown below?

6H2O (l) + 3O2 (g) 6H2O2 (l)

A) + 196 / 3 kJ B) +6 x 196 kJ C) +3 x 196 kJ D) -196 / 3 kJ

C-H 413 N-H 391 O-H 463 H-H 436

C-F 485 N-F 272 O-F 190 H-F 565 F-F 155

C-Cl 328 N-Cl 200 O-Cl 203 H-Cl 431 Cl-Cl 242

C-Br 276 N-Br 243 O-Br 235 H-Br 366 Br-Br 193

C-I 234 O-I 234 H-I 299 I-I 151

C-C 347 N-N 163 C-N 293 C-O 358 O-O 146

C=C 612 N=N 418 C=N 615 C=O 799 O=O 495

C C 820 N N 941 C N 891 C O 1072

C-H 413 N-H 391 O-H 463 H-H 436

C-F 485 N-F 272 O-F 190 H-F 565 F-F 155

C-Cl 328 N-Cl 200 O-Cl 203 H-Cl 431 Cl-Cl 242

C-Br 276 N-Br 243 O-Br 235 H-Br 366 Br-Br 193

C-I 234 O-I 234 H-I 299 I-I 151

C-H 413 N-H 391 O-H 463 H-H 436

C-F 485 N-F 272 O-F 190 H-F 565 F-F 155

C-Cl 328 N-Cl 200 O-Cl 203 H-Cl 431 Cl-Cl 242

C-Br 276 N-Br 243 O-Br 235 H-Br 366 Br-Br 193

C-I 234 O-I 234 H-I 299 I-I 151

C-HC-H 413413 N-HN-H 391391 O-HO-H 463463 H-HH-H 436436

C-FC-F 485485 N-FN-F 272272 O-FO-F 190190 H-FH-F 565565 F-FF-F 155155

C-ClC-Cl 328328 N-ClN-Cl 200200 O-ClO-Cl 203203 H-ClH-Cl 431431 Cl-ClCl-Cl 242242

C-BrC-Br 276276 N-BrN-Br 243243 O-BrO-Br 235235 H-BrH-Br 366366 Br-BrBr-Br 193193

C-IC-I 234234 O-IO-I 234234 H-IH-I 299299 I-II-I 151151

C-C 347 N-N 163 C-N 293 C-O 358 O-O 146

C=C 612 N=N 418 C=N 615 C=O 799 O=O 495

C C 820 N N 941 C N 891 C O 1072

C-C 347 N-N 163 C-N 293 C-O 358 O-O 146

C=C 612 N=N 418 C=N 615 C=O 799 O=O 495

C C 820 N N 941 C N 891 C O 1072

C-C 347 N-N 163 C-N 293 C-O 358 O-O 146

C=C 612 N=N 418 C=N 615 C=O 799 O=O 495

C C 820 N N 941 C N 891 C O 1072

C-CC-C 347347 N-NN-N 163163 C-NC-N 293293 C-OC-O 358358 O-OO-O 146146

C=CC=C 612612 N=NN=N 418418 C=NC=N 615615 C=OC=O 799799 O=OO=O 495495

C CC C 820820 N NN N 941941 C NC N 891891 C OC O 10721072

Exam 3

22. What is the approximate value of S for the reaction below?

Ca2+ (aq) + 2HCO31-

(aq) CaCO3 (s) + CO2 (g) + H2O (l)

A) S < 0 B) S > 0 C) S ~ 0 D) cannot be predicted

23. Choose the correct statement that describes the reaction below.

MgCO3 (s) MgO (s) + CO2 (g) H = +117.3 kJ/mol

A) The reaction is extensive at high temperature.

B) The reaction is extensive at low temperature.

C) The reaction is extensive at any temperature.

D) The reaction is not extensive at any temperature.

24. Mustard gas is prepared according to the reaction below. Given that Keq = 5.48x10-1,

[SCl2] = 0.385 M and [C2H4] = 0.831 M, what is the concentration of S(CH2CH2Cl)2 in the mixture?

SCl2 (g) + 2 C2H4 (g) S(CH2CH2Cl)2 (g)

A) 0.175 B) 0.485 C) 0.351 D) 0.146 E) 0.268

Use the reaction coordinate diagram below to answer the next three questions regarding the

reaction: A-B + C A + B-C .

25. Which reaction above has the largest forward rate constant?

A) I B) II C) III

26. Which reaction above has the smallest value of Kequilibrium?

A) I B) II C) III

27. Which reaction(s) above will increase in the concentration of [B-C] when heated?

A) I only B) II only C) III only D) I & II E) II & III

5 kJ

10 kJ

15 kJ

A-B, C

A, B-C

reaction coordinate

1 kJ2 kJ

5 kJ

A-B, C

A, B-C

reaction coordinate

3 kJ

6 kJ

9 kJ

A-B, C

A, B-C

reaction coordinate

I II III

Exam 3

28. Consider the following reaction at equilibrium.

2 C2H6O (aq) + 2CO2 (g) C6H12O6 (aq) H > 0 ethanol glucose

Which changes would shift the equilibrium to the right?

I) addition of CO2

II) removal of CO2

III) removal of glucose

IV) heating the reaction

V) cooling the reaction

A) I, III, & IV B) II, III, & V C) I & IV D) I & V E) II, III, & IV

I pledge that I have neither given nor received aid on this exam.

Signature:______________________

Exam 3 Special Code 111111 Petrovich, Fall 2010

Directions:

1) Please put away all papers, cell phones and clear the memory on your calculators. 2) On the scantron sheet, fill and bubble in your last name, first name, special code (111111)

and student identification number (000######). 3) On the paper exam, print your last name and first name on page 1 of the exam. 4) Completely bubble in your answers for questions 1-28 on the scantron. 5) Please sign the honor pledge at the end of the exam. 6) Return all exam materials to Dr. Petrovich/TA before leaving DAB222. 7) Failure to follow the exam labeling instructions will result in a loss of 2 points on your

exam score.

Oxidation State Rules

1) The oxidation states of the atoms in an element are all zero.

2) Fluorine is always assigned an oxidation number of -1.

3) Group 1A metals are +1, Group 2A metals are +2, and aluminum is +3.

4) H is +1 when bonded to non-metals. H is 1 when bonded to metals. 5) Oxygen is assigned an oxidation number of 2. 6) Group 7A elements are assigned an oxidation number of -1.

PV = nRT G = H - T S R = 0.0821 L*atm/K*mol or 8.314 J/K*mol 1 atm = 760 mm Hg = 760 torr

K = C + 273.15 H = coeffxDbonds broke coeffxDbonds formed

Exam 3

Key:

1) A 15) E

2) B 16) B

3) D 17) B

4) C 18) A

5) A 19) D

6) C 20) E

7) A 21) C

8) B 22) B

9) C 23) A

10) C 24) D

11) E 25) A

12) B 26) B

13) D 27) E

14) B 28) A