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University of Waterloo

DEPARTMENT OF CHEMISTRY

Chemistry 120 - Term Test #1

Lecture time: 12:30 pm Instructor: XXXXXXXXX 13 October 2000

Name (Print Clearly): _______________________________________________________________

Student Number: Signature:

Aids Allowed: Electronic Calculator

Time Allowed: 50 minutes

Instructions:

1. This test booklet has 10 questions and 7 pages (including this Cover Page and the Data Sheet)

Check now to ensure no pages are missing. If pages are missing, ask for a new test booklet

immediately.

1. There is only one correct answer for each question. Circle your answer on this booklet.

2. Attempt all questions. No marks are deducted for wrong answers.

3. Do all rough work on this test booklet.

4. Use an ordinary HB lead pencil for filling in the computer card.

5. Print your name and other information in top right corner of the front of the computer card.

6. On the computer answer card, fill in your ID number, Section Number (004) and the appropriate

Card Number (001) in the designated fields. Make sure you fill in the appropriate ovals in pencil.

7.

Make sure any erasures are complete and clean.

8. When you have finished, or before time is up, transfer your answers to the computer card by

filling in the appropriate oval (A,B,C,D or E) in the column for that question on the card.

9. At the end of the test, turn in this test booklet and your computer card, and leave immediately.

Note: The last page is a DATA SHEET. You may tear it off.

On your computer answer card: Fill in ovals 004 for the Section Number.

Fill in ovals 001 for the Card Number.

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CHEM 120 (Section 4) Test #1 (Version 1) Page 2 of 8

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1. What volume of O2, measured at 0.00oC and 101 kPa, is required for the complete

combustion of 0.0390 mol C10H8 ?

A. 0.877 L

B. 126 L

C. 0.104 L

D. 0.0731 L

E. 10.5 L

2. What is the density of O2 gas at 55.0oC and 103 kPa?

A. 1.43 g L1

B. 122 g L1

C. 1.21 g L1

D. 7.21 g L1

E. 4.35 g L1

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CHEM 120 (Section 4) Test #1 (Version 1) Page 3 of 8

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3. What mass of AgCl(s) forms when 100.0 mL of 0.400 M BaCl2 solution is mixed with

100.0 mL of 0.500 M AgNO3 solution?

A. 5.73 g

B. 7.17 g

C. 2.87 g

D. 11.5 g

E. 3.58 g

4. An aqueous solution of ethylene glycol, HO-CH2CH2-OH, has a density of 1.046 g mL1

and is 32.22% (by mass) ethylene glycol. What is the molarity of ethylene glycol in this

solution?

A. 5.43 M

B. 16.8 M

C. 0.523 M

D. 1.91 M

E. 0.184 M

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CHEM 120 (Section 4) Test #1 (Version 1) Page 4 of 8

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5. A sample of a compound of iron, Fe, and sulfur, S, was reacted with oxygen, O2. The

products were 0.1688 g Fe2O3 and 0.2708 g SO2. What is the empirical formula of the

compound?

A. FeS

B. Fe2S

C. Fe2S3

D. FeS2

E. FeS4

6. Which of the following statements is true?

A. A 22.4-L sample of O2 gas must contain one mole of O2 molecules.

B. In a gaseous mixture of helium and argon, helium atoms move faster, on average,

than argon atoms.

C. The volume of one mole of O2 is only two-thirds that of one mole of O3 under the

same conditions of temperature and pressure.

D. If a gas mixture contains one mole of H2 and one mole of O2, the pressure exerted

by O2 is about sixteen times greater than that exerted by H2.

E. If the temperature of a sample of ideal gas is increased from 10oC to 20

oC at

constant pressure, the volume will double.

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CHEM 120 (Section 4) Test #1 (Version 1) Page 5 of 8

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7. Complete and balance the equation below using the smallest whole number coefficients.

VO2+

(aq) + Zn(s) V3+

(aq) + Zn2+

(aq) (acidic solution)

In the complete and balanced equation, there are

A. 3 H+ on the left-hand side of the equation.

B. 4 H2O on the right-hand side of the equation

C. 4 H+ on the left-hand side of the equation.

D. one O2 on the right-hand side of the equation

E. 2 H2O on the left-hand side of the equation.

8. Exactly 1.0 L of helium gas at 760 torr and 1.0 L of argon gas at 380 torr are introduced

into a 4.0-L vessel. Assuming a constant temperature, what is the final pressure?

A. 95 torr

B. 190 torr

C. 285 torr

D. 475 torr

E. 570 torr

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CHEM 120 (Section 4) Test #1 (Version 1) Page 6 of 8

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9. When a 1.00-g sample of a mixture of NaCl and AlCl3 is treated with excess AgNO3

solution, 0.02142 moles of solid AgCl are obtained. What is the percentage by mass of

NaCl in the mixture?

Molar masses: NaCl, 58.44 g mol1 AlCl3, 133.33 g mol1

A. less than 10%

B. 20%

C. 25%

D. 31%

E. 42%

10. When solid potassium hydrogen carbonate, KHCO3, is heated, it decomposes:

2 KHCO3(s) K2CO3(s) + CO2(g) + H2O(l).

When a 0.50-g sample of KHCO3 is heated, 0.32 g K2CO3 is obtained. What is the

percent yield for this experiment?

A. 93%

B. 64%

C. 46%

D. 23%

E. none of the above

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CHEM 120 (Section 4) Test #1 (Version 1) Page 7 of 8

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DETACH THIS DATA SHEET FOR EASY REFERENCE

1

H1.008

2

He4.003

3

Li6.941

4

Be9.012

5

B10.81

6

C12.01

7

N14.01

8

O16.00

9

F19.00

10

Ne20.18

11

Na22.99

12

Mg24.31

13

Al26.98

14

Si28.09

15

P30.97

16

S32.07

17

Cl35.45

18

Ar39.95

19

K39.10

20

Ca40.08

21

Sc44.96

22

Ti47.88

23

V50.94

24

Cr52.00

25

Mn54.94

26

Fe55.85

27

Co58.93

28

Ni58.69

29

Cu63.55

30

Zn65.38

31

Ga69.72

32

Ge72.59

33

As74.92

34

Se78.96

35

Br79.90

36

Kr83.80

37Rb85.47

38Sr87.62

39Y88.91

40Zr91.22

41Nb92.91

42Mo95.94

43Tc(98)

44Ru101.1

45Rh102.9

46Pd106.4

47Ag107.9

48Cd112.4

49In114.8

50Sn118.7

51Sb121.8

52Te127.6

53I126.9

54Xe131.3

55

Cs132.9

56

Ba137.3

(57-71)

La-Lu

72

Hf178.5

73

Ta180.9

74

W183.9

75

Re186.2

76

Os190.2

77

Ir192.2

78

Pt195.1

79

Au197.0

80

Hg200.6

81

Tl204.4

82

Pb207.2

83

Bi209.0

84

Po(209)

85

At(210)

86

Rn(222)

87

Fr(223)

88

Ra226

(89-103)

Ac-Lr104

Rf

105

Db

106

Sg

107

Bh

108

Hs

109

Mt

110

Uun

111

Uuu

112

Uub

113

Uut

Constants: Conversion factors:

NA = 6.022 1023 mol1 1 atm = 101.325 kPa = 760 torr

= 760 mmHg

R = 0.082058 atm L K1 mol

1 0oC = 273.15 K

= 8.3145 kPa L K1

mol1

= 8.3145 J K1 mol

1

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CHEM 120 (Section 4) Test #1 (Version 1) Page 8 of 8

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ANSWERS:

1E 3B 5D 7C 9B

2C 4A 6B 8C 10A