Chemistry 1045

Name:ffabnev\aExam 1 Fall 2012

Lab Instructor

ID Number:

1. These tests are machine grades; therefore, be sure to use a No. 1 or 2 pencil for marking the answer sheets.Completely blacken the answer circle. If you change an answer, erase the previous mark completely.2. Write your last name (family name) in the first box of the section marked "NAME". Skip one box and then inthe next box write your first name. Example: if a student's name is John L. Doe then his answer sheet would looklike this:

NAME (LAST FIRST, M.I.D O E J O H N

If your whole name does not fit, put as much as will fit. Then blacken the corresponding letters below each space onthe answer sheet.3. Fill in your ID number in the space provided, beginning with 00 followed by your panther ID# in space "A".Column J will remain blank. Then blacken the circles corresponding to the numbers below each space.4. In the "Grade or Educ" section, indicate the color of the test form you were given:

Mark in Grade or Educ. Test Color Stripe Color123456

VIV2V3V4V5V6

BlueGoldGrayIvoryPinkTan

BlueYellowGreenOrangePinkBrown

Make sure that you mark in "Grade or Educ" your test color, AND that the color mark above your name on theanswer sheet is the same as your test color. It is your responsibility to make sure that colors match. You also needto fill in the test color number in the vertical strip next to the name field.

GRADE

OREDUC

5. In special Code column P, bubble in your section number,MWF 9:30 AM bubble 1MWF 11:00 AM bubble 2MWF 12:30 PM bubble 3MWF 2:00 PM bubble 5MW 6:25 PM bubble 6

6. The time limit on this test is about 1 hr 35 min. 2 hours less the administration time.8. READ THE TEST CAREFULLY. You should find 21 questions on the exam.

CHM 1045

EQUATIONS1km = 0.6214 mi l f t = 30.48 cm

1 atm = 760 mm Hg

1 m = 39.37 in = 1.094yds

1 mm Hg-= 1 torr

1 in = 2.54 cms

1 kg = 2.205 Ibs l l b = 453.59 g

1 oz = 28.35 g

KE = l/2 mv2

NA 6.022x1023

-34h = 6.626*10-MJs

RH =1.097xl(T2

= 3*108m/s

Cwa,er=4.184J/g°C

E« = - 2 . 1 8 x l O ~ 1 8 J ( l / n 2 )

1 L.atm = 101.325 J

1 cal = 4.184 J

R = 0.0821 L.atm/mol.K

q = C x AT

R = 8.314J/molK

lL=1.057qt 1 gallon = 3.785 L

Pressure(P) = F/A = m*a/A

PV=nRT

AE = q+ w

w = - PAY

q = AE+ PAY

Formulaand Constant Sheet

= Av E = hv

E = b 1 1nf n.

ftl

= nAH

1—«*'

MW = •dRT i _ P2V2

P

= XSr

V°l,phere = f

PM

RT

R

where£0= 8.85 xlO-12C2/J.m

IAPeriodic Table

8A

1H

1.01

3

Li6.94

11

Na22.99

19

K39.10

37

Rb85.47

55

Cs132.91

87

Fr(223)

2A 3A 4A

4

Be9.01

12

Mg24.31

20

Ca

, 3B 4B SB B 7B SB SB SB IB 2B

21

Sc40.08 44.96

38 39

Sr Y87.62 j 88.91

56

Ba137.33 \8

Ra(226)

57

La138.91

89

Ac(227)

22

Ti47.87

40

Zr91.22

72

Hf178.49

104

Rf(261)

(atomic mass) In parenthesesrefers to the atomic mass of

the most stable Isotope

23

V50.94

41

Nb92.91

73

Ta180.95

105

Db(262)

24

Cr52.00

42

Mo95.94

74

w183.84

106

Sg(266)

25

Mn54.94

43

Tc(98)

75

Re186.21

107

Bh(264)

26

Fe55.85

44

Ru101.07

76

Os190.23

108

Hs(269)

27

Co58.93

45

Rh102.91

77

Ir192.22

109

Mt(268)

28

Nl58.69

46

Pd106.42

78

Pt195.08

29

Cu63.55

47

Ag107.87

79

Au196.97

30

Zn65.39 ;

48

5

B10.81

13

Al26.98

31

Ga69.72

49

Cd In112.41 ' 114.82

80 81

Hg TI200.59 204.38

6

c12.01

14

Si28.09

32

Ge72.61

50

Sn118.71

82

Pb207.2

5A 6A 7A

7

N14.01

15

P30.97

33

As74.92

51

Sb121.76

83

Bi208.98

8

o16.00

16

s32.06

34

Se78.96

52

Te127.60

84

Po(209)

9

F19.00

17

Cl35.45

35

Br79.90

S3

I126.90

85

At(210)

2

He4.00

10

Ne20.18

18

Ar39.95

36

Kr83.80

54

Xe131.29

86

Rn(222)

58

Ce140.12

90

Th232.04

59

Pr140.91

91

Pa231.04

60

Nd144.24

92

u238.03

61

Pm(145)

93

Np(237)

62

Sm150.36

94

Pu(244)

63

Eu151.96

95

Am(243)

64

Gd157.25

96

Cm(247)

65

Tb158.93

97

Bk(247)

66

Dy162.50

98

Cf(251)

67

Ho164.93

99

Es(252)

68

Er167.26

100

Fm(257)

69

Tm168.93

101

Md(258)

7 0

Yb173.04

102

No(259)

71

Lu174.97

103

Lr(262)

CHM 1045-All Sections Exam IB Fall 2012 ^\t 1 Basic Concepts of Chemistry

Chapters 1 - 3 £

1. Find the mass of carbon in 1.350 L of acetone (CH^COCH^) given the density of acetone is0.791 g/mL . i?£OL x ( 000ml v

f —^—^ .i—iiraim "t '«•• -l.pnlil-l~ •̂

( N 669 ̂ ^ ^^ ^ ^^ «O^\ fY\ I 1 «AO\

V. 220.8 gD. 73.59 g ^ Q?E. 1068 g / (

1} lOO'Cs^ . l^2. An unknown element E is found to have two isotopes. The atomic mass of E is 57.15 amu.

The mass of the first isotope E - 56 is 56.482 amu, and its natural abundance is 69.19%.Calculate the mass of the second isotope of E?

E. 56:82amu 6*30'*l* - \ g - G H b | GUI X^Sg,C/>

3. Which of the following lists contain only transition metals?

A. Mg,Ca,BB. Cu,Fe,CoC. Gd,Tb,Bk,.̂ Li,Fr,Rb

E. I,F,C1

4. Which of the following symbols represent isotopes of nitrogen?

;.> «. ?N

A. ionlyB. iionly

,€L iii only\~D\i and ii^E^i and iii

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UJ

O

\. Which of the following statements is/are correct? .

i. Hg, Pb, and Na are the symbols for mercury, lead, and sodiumii. K, S, and Mn are the symbols for potassium, sulfur, and manganese

, and Ti are the symbols for antimony, silver, and tin

A. ionly^.^.ii onlyQc. i and ii

D. ii and iiiE. i and iii

6. What is the name of the following compound Cr(CO3)3

A. ''Chromium ( III ) carbonateChromium carbonate

C. Chromium ( H ) carbonateD. Chromium ( VI ) carbonateE. Chromium ( EX ) carbonate

7. Sulfurous acid is:

E. HSO3

8. A student in CHM1045L is asked to measure out the area of the classroom and report theanswer in m^. Using a measuring tape, the student found that the room is 18.8 by 15.5 ft inarea. What should the student report for the area in m^? (1 in. = 2.54 cm)

I <? Q- t t- v ^Oi U K <T-T2 /\ I , . \ ^ O^ ',2 » «> • *

cr-r-%

9. The radius of a helium atom 3 1 .4 pm. What is the thickness in Gm?

C. 3.14xlO-17

3.14xl04

E. .14X10-20 A

X 10

Page 2, v5

10. How many significant figures will the final answer to this calculation have?

( 935.30/2.195)+ 50

/2)i T^2 U a t / > \ 3 vSa H3AD. 4 ,E. 5

11 ̂ Which of the following statements is fr-«e:i. Lithium and Oxygen will form an ionic bond

.uorine and Phosphorus will form an ionic bond. Iodine and Calcium will form a covalent bond

. )i onlyiionly

C. iii onlyD. i and iiE. i,:

12. What is the correct formula for manganese(ni) sulfite?

A. Mn3(SC>4)2B.C^Mn2(S04)3

/D)/E.

13. Which of the following statements describe a physical change?

</j. Condensation of water vapor to form a liquidSn. Freezing of liquid water into solid water\J iii. Conversion of ammonia to hydrogen and nitrogen gases

A. ii onlyB. i,ii,&iiiC. ii & iii

( D.)i and iiE. i and iii

14. The correct name for BrO2~ ig and the correct name for CC^- is

tA. Bromate; PercarbonateB. Perbromate; CarbonateC^Hypobromite, Carbonite

(upBromite, Carbonatei. Bromite, Hypocarbonite

Page3,v5

15. Which one of the following samples will have the greatest mass

A. 6 mol of Neon gasB. 4 mol of solid siliconC. 2 mol of Chlorine gasD. 3 mol of solid potassiumE. 1 mol of Xenon gas

16. The compound dibromobis(ethylenediamine)cobalt(III) chloride has a formula of[Co(C2N2H8)2Br2]Cl< What is the mass percent hydrogen in the compound?

;

A. 0.27 %B. 4.32 %C. 2.16%D. 8.63 %E. 0.54 %

17. When the follwoing equation is balanced properly, the coefficient indicating the number ofoxygen molecules being reacted is:

02 (g) — > 12 C02 (g) + i H20 (g)

C \(p C / (0 '

H £> (0

0 5018. A sample is found to contain 42.613 g of atomic oxygen and 170.665 g of atomic sulfur.

According to the Law of Definite Proportions, which of the following would be identified asthe same compound as the sample?

A. a compound containing 18.232 g oxygen and 12.179 g sulfurB. a compound containing 22.562 g oxygen and 30.120 g sulfur

a compound containing 16.995 g oxygen and 8.514 g sulfura compound containing 10.448 g oxygen and 41.844 g sulfur

compound containing 12.823 g oxygen and 25.684 g sulfur

M9i'W2> <H

A flask can hold 85.66 g of water at 43.00 °C. At this temperature the density of water is0.99107 g/cm^. Calculatelhe mass of methanol that the same container would hold at 20.00°C. The density of methanol is 0.7913 g/mL at 20.00°C.

gB. 67.18gC. 86.43 g

-D. 60.87 gE. 68.39g

o\

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