Sr no3 2 na2so4 net ionic equation

Chem 1010 Name__________________________________ Unit 4-5 Test

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

1) When the following equation is balanced, the coefficient of Al is __________.

Al (s) + H2O (l) → Al(OH)3 (s) + H2 (g)

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

2) When the following equation is balanced, the coefficient of NaOH is __________.

H3PO4 (aq) + NaOH (aq) → Na3PO4 (aq) + H2O (l)

A) 1 B) 4 C) 2 D) 0 E) 3

3) When the following equation is balanced, the coefficient of O2 is __________.

C2H4O (g) + O2 (g) → CO2 (g) + H2O (g) A) 5 B) 3 C) 4 D) 2 E) 1

4) When the following equation is balanced, the coefficient of C3H8O3 is __________.

C3H8O3 (g) + O2 (g) → CO2 (g) + H2O (g)

A) 2 B) 5 C) 7 D) 1 E) 3

1

5) Write a balanced equation to show the reaction of aqueous aluminum acetate with aqueous ammonium phosphate to form solid aluminum phosphate and aqueous ammonium acetate. A) Al(C2H3O2)2(aq) + (NH4)2PO4(aq) → AlPO4(s) + 2 NH4C2H3O2(aq) B) Al(CO2)3(aq) + (NH4)3PO3(aq) → AlPO3(s) + 3 NH4CO2(aq) C) Al(C2H3O2)2(aq) + (NH3)2PO4(aq) → AlPO4(s) + 2 NH3C2H3O2(aq) D) Al(C2H3O2)3(aq) + (NH4)3PO4(aq) → AlPO4(s) + 3 NH4C2H3O2(aq) E) Al(CO3)2(aq) + (NH3)2PO4(aq) → AlPO4(s) + 2 NH3CO3(aq)

6) When the reaction shown is correctly balanced, the coefficients are:

C6H6 (l) + O2 (g) → CO2 (g) + H2O (g)

A) 1, 3.5, 6, 7 B) 2, 16.5, 12, 7 C) 2, 15, 12, 6 D) 1, 9.5, 6, 7 E) 1, 6, 6, 7

7) The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is ________. A) 2HNO3 (aq) + Sr(OH)2 (aq) → 2H2O (l) + Sr(NO3)2 (aq) B) 2HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2(aq) + 2H2 (g) C) HNO3 (aq) + Sr(OH)2 (aq) → H2O (l) + Sr(NO3)2 (aq) D) HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2 (aq) + H2 (g) E) HNO3 (aq) + SrOH (aq) → H2O (l) + SrNO3 (aq)

8) What are the spectator ions in the reaction between Mg(OH)2 (aq) and HCl (aq)? A) H+ and OH-

B) Mg2+ and H+ C) H+ and Cl- D) OH- only E) Mg2+ and Cl-

9) When aqueous solutions of AgNO3 and KI are mixed, AgI precipitates. The balanced net ionic equation is ________. A) Ag+ (aq) + NO3- (aq) → AgNO3 (aq)

B) Ag+ (aq) + I- (aq) → AgI (s) C) AgNO3 (aq) + KI (aq) → AgI (s) + KNO3 (aq) D) AgNO3 (aq) + KI (aq) → AgI (aq) + KNO3 (s) E) Ag+ (aq) + NO3- (aq) → AgNO3 (s)

10) A neutralization reaction between an acid and a metal hydroxide produces ________. A) oxygen gas B) sodium hydroxide C) ammonia D) water and a salt E) hydrogen gas

2

11) When H2SO4 is neutralized by NaOH in aqueous solution, the net ionic equation is ________.

A) SO42- (aq) + 2Na+ (aq) → Na2SO4 (s) B) 2H+ (aq) + 2NaOH (aq) → 2H2O (l) + 2Na+ (aq)

C) SO42- (aq) + 2Na+ (aq) → Na2SO4 (aq)

D) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq) E) H+ (aq) + OH- (aq) → H2O (l)

12) Which of the following is an oxidation-reduction reaction? A) Pb(C2H3O2)2(aq) + 2 NaCl(aq) → PbCl2(s) + 2 NaC2H3O2(aq) B) HCl(aq) + LiOH(aq) → LiCl(aq) + H2O(l) C) Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) D) NaI(aq) + AgNO3(aq) → AgI(s) + NaNO3(aq) E) All of the above are oxidation-reduction reactions.

13) What reactant (if any) is gaining electrons in the following reaction?

Zn(s) + 2 AgNO3(aq) → Zn(NO3)2(aq) + 2 Ag(s)

A) N B) Ag C) Zn D) O E) There is no transfer of electrons in this reaction.

14) What reactabt (if any) is losing electrons in the following reaction?

Zn(s) + 2 AgNO3(aq) → Zn(NO3)2(aq) + 2 Ag(s)

A) O B) N C) Ag D) Zn E) There is no transfer of electrons in this reaction.

15) A compound that is composed of only carbon and hydrogen contains 80.0% C and 20.0% H by mass. What is the empirical formula of the compound? A) C7H20 B) C20H60 C) CH4 D) C2H6 E) CH3

3

16) What is the empirical formula of a compound that contains 27.0% S, 13.4% O, and 59.6% Cl by mass? A) SO2Cl B) SOCl C) S2OCl D) ClSO4 E) SOCl2

17) An oxide of aluminum contains 0.545 g of Al and 0.485 g of O. Find the empirical formula for the oxide. A) Al2O3 B) Al3O2 C) AlO D) Al6O2

18) A compound that is composed of carbon, hydrogen, and oxygen contains 70.6% C, 5.9% H, and 23.5% O by mass. The molecular weight of the compound is 136 amu. What is the molecular formula? A) C8H4O B) C8H8O2 C) C9H12O D) C5H6O2 E) C4H4O

19) A compound contains 40.0% C, 6.71% H, and 53.29% O by mass. The molecular weight of the compound is 90.09 amu. The molecular formula of this compound is ________. A) CHO2 B) C2H4O2 C) C3H6O3 D) C2H3O4 E) CH2O

20) A certain metal sulfide, MS2, is determined to be 40.064% sulfur by mass. What is the identity of the metal M? A) Molybdenum B) Tungsten C) Chromium D) Iron E) Cobalt

21) Which of the following statements about gases is false? A) Gas mixtures are homogeneous. B) All gases are colorless and odorless at room temperature. C) Distances between molecules of gas are very large compared to bond distances within molecules. D) Gases expand spontaneously to fill the container they are placed in. E) Gases are highly compressible.

4

22) Gaseous mixtures ________. A) are all heterogeneous B) are all homogeneous C) can only contain molecules D) can only contain isolated atoms E) must contain both isolated atoms and molecules

23) When the pressure is 1.00 atm, he volume of an ideal gas is 22.4L at ________. A) -273 K B) -45 °F C) -273 °C D) 0 °C E) -363 K

24) A sample 0.100 moles of a gas is collected at at STP. What is the volume of the gas in liters? A) 2.24 L B) 0.205 L C) 22.4 L D) 2.44 L E) 0.0205 L

25) A sample a gas is collected is maintained at a temperature of 25°C and has a volume of 1.30 L at 0.987 atm of pressure. How many moles of gas are present in the sample? A) 0..981 moles B) 0.205 L C) 0.00209 moles D) 0.0525 moles E) 0..469 moles

26) A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10 L to 15 L. The final pressure is ________ atm. A) 0.67 B) 1.5 C) 3.3 D) 15 E) 7.5

27) A sample of a gas originally at 25 °C and 1.00 atm pressure in a 2.5 L container is subject to a pressure of 0.85 atm and a temperature of 15 °C. The final volume of the gas is ________ L. A) 0.38 B) 3.0 C) 2.8 D) 2.6 E) 2.1

5

28) A 0.250. L sample of gas at 1.00 atm and 20.0°C has the temperature increased to 40.0°C and the volume increased to 0.500 L. What is the new pressure? A) 2.14 atm B) 0.374 atm C) 0.468 atm D) 1.87 atm E) 0.534 atm

29) What volume of carbon dioxide gas in liters is produced at STP by the decomposition of 0.150 g CaCO3 via the equation:

CaCO3 (s) → CaO (s) + CO2 (g)

A) 2.24 L B) 6.31 L C) 0.0196 L D) 0.0336 L E) 1.31 L

30) What quantity of sodium azide in grams is required to fill a 56.0 liters air bag with nitrogen gas at 1.00 atm and exactly 0 °C :

2 NaN3 (s) → 2Na (s) + 3N2 (g)

A) 12.3 g B) 6.31 g C) 108 g D) 162 g E) 25.2 g

6

1 2

H A

bo ut

C he

m is

try H

e

3 4

5 6

7 8

9 10

Li B

e B

C N

O F

N e

11 12

13 14

15 16

17 18

N a

M g

Al Si

P S

C l

Ar

19 20

21 22

23 24

25 26

27 28

29 30

31 32

33 34

35 36

K C

a Sc

Ti V

C r

M n

Fe C

o N

i C

u Zn

G a

G e

As Se

B r

K r

37 38

39 40

41 42

43 44

45 46

47 48

49 50

51 52

53 54

R b

Sr Y

Zr N

b M

o Tc

R u

R h

Pd Ag

C d

In Sn

Sb Te

I Xe

55 56

57 -7

1 72

73 74

75 76

77 78

79 80

81 82

83 84

85 86

C s

B a

H f

Ta W

R e

O s

Ir Pt

Au H

g Tl

Pb B

i Po

At R

n

87 88

89 -1

03 10

4 10

5 10

6 10

7 10

8 10

9 11

0 11

1 11

2 11

3 11

4 11

5 11

6 11

7 11

8

Fr R

a R

f D

b Sg

B h

H s

M t

D s

R g

C n

U ut

Fl U

up Lv

U us

U uo

57 58

59 60

61 62

63 64

65 66

67 68

69 70

71

La nt

ha ni

de s

La C

e Pr

N d

Pm Sm

Eu G

d Tb

D y

H o

Er Tm

Yb Lu

89 90

91 92

93 94

95 96

97 98

99 10

0 10

1 10

2 10

3

Ac tin

id es

Ac Th

Pa U

N p

Pu Am

C m

B k

C f

Es Fm

M d

N o

Lr8A

Pe rio

di c

Ta bl

e of

th e

El em

en ts

1A ©

20 12

T od

d H

el m

en st

in e

1. 00

79 4

2A 3A

4A 5A

6A

ht tp

:// ch

em is

try .a

bo ut

.c om

7A 4.

00 26

02

6. 94

1 9.

01 21

82 10

.8 11

12 .0

10 7

14 .0

06 7

15 .9

99 4

18 .9

98 40

32 20

.1 79

7

30 .9

73 76

2 32

.0 65

35 .4

53 39

.9 48

39 .0

98 3

40 .0

78 44

.9 55

91 2

47 .8

67 50

.9 41

5 51

.9 96

1

7B ┌

─ ─

─ ─

─ 8

B ─

─ ─

─ ─

┐ 1B

2B 26

.9 81

53 86

28 .0

85 5

22 .9

89 76

9 24

.3 05

0 3B

4B 5B

6B

78 .9

6 79

.9 04

83 .7

98 54

.9 38

04 5

55 .8

45 58

.9 33

19 5

58 .6

93 4

63 .5

46 65

.3 8

85 .4

67 8

87 .6

2 88

.9 05

85 91

.2 24

92 .9

06 38

95 .9

6

69 .7

23 72

.6 4

74 .9

21 60

11 4.

81 8

11 8.

71 0

12 1.

76 0

12 7.

60 12

6. 90

44 7

13 1.

29 3

[9 8]

10 1.

07 10

2. 90

55 0

10 6.

42 10

7. 86

82 11

2. 41

1

[2 09

] [2

10 ]

[2 22

] 18

6. 20

7 19

0. 23

19 2.

21 7

19 5.

08 4

19 6.

96 65

69 20

0. 59

[2 23

] [2

26 ]

Ac tin

id es

[2 67

] [2

68 ]

[2 71

]

20 4.

38 33

20 7.

2 20

8. 98

04 0

13 2.

90 54

51 9

13 7.

32 7

La nt

ha ni

de s

17 8.

49 18

0. 94

78 8

18 3.

84

[2 84

] [2

89 ]

[2 88

] [2

93 ]

[2 94

] [2

94 ]

[2 72

] [2

70 ]

[2 76

] [2

81 ]

[2 80

] [2

85 ]

[2 27

] 23

2. 03

80 6

23 1.

03 58

8 23

8. 02

89 1

[2 37

] [2

44 ]

[2 43

]

15 1.

96 4

15 7.

25 13

8. 90

54 7

14 0.

11 6

14 0.

90 76

5 14

4. 24

2 [1

45 ]

15 0.

36

[2 59

] [2

62 ]

[2 47

] [2

47 ]

[2 51

] [2

52 ]

[2 57

] [2

58 ]

16 8.

93 42

1 17

3. 05

4 17

4. 96

68 15

8. 92

53 5

16 2.

50 0

16 4.

93 03

2 16

7. 25

9

Ryan Holcomb
R = 0.08206 L•atm/mol•K
Soluble Ionic Compounds (aq) Insoluble Ionic Compounds (s)

Contain these ions: Exceptions: Contain these ions Exceptions

Cations: Anions:

Group I Cations and ammonia Li+ Na+ K+ Rb+ Cs+

NH4+

Compounds with Group I and ammonia cations are always soluble

CO32- CrO42- PO43- S2-

compounds with Group 1 cations and NH4+

Anions: OH- compounds with Group 1 cations, NH4+

C2H3O2- HCO3- NO3- ClO3-

Compounds with these anions are always soluble

Cl- Br- I-

compounds with Ag+, Hg22+, and Pb2+

F-

compounds with Group II metal cations (Be2+, Mg2+, Ca2+, Sr2+, Ba2+) as well as Pb2+ and Fe3+

SO42- compounds with Ag+, Ba2+, Ca2+, Hg22+, Pb2+ and Sr2+