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BALANCING EQUATIONS - COMBUSTION OF ORGANIC COMPOUNDS -- Quiz

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3-1.198151

3

Question 1.
Balance the following equation. What is the sum of the coefficients of the
reactants?
C7H10O3 + ____ O2
a)

10

b)

12

c)

9

d)

8

e)

11

____ CO2 + ____ H2O

Question 2.
Balance the following equation. What is the sum of the coefficients of the
reactants?
C12H22O11 + ____ O2
a)

10

b)

7

c)

13

____ CO2 + ____ H2O

d)

12

e)

9

Question 3.
Balance the following equation and choose the quantity which is the sum of the
coefficients of the reactants.
C8H8O2 + ____ O2
a)

9

b)

7

c)

10

d)

11

e)

8

____ CO2 + ____ H2O

BALANCING EQUATIONS - MISC. -- Quiz

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3-4.198227

3

Question 1.
Balance the following equation. What is the sum of the coefficients of the
reactants?
____ Pb + ____ H2O + ____ O2
____ Pb(OH)2

a)

6

b)

4

c)

5

d)

8

e)

10

Question 2.
Balance the following equation and choose the quantity which is the sum of the
coefficients of the reactants?
____ Mg3(PO4)2 + ____ C
____ Mg3P2 + ____ CO
a)

7

b)

8

c)

9

d)

6

e)

5

Question 3.
Balance the following equation for the oxidation of table sugar. What is the
coefficient of oxygen in the balanced equation?
____ C12H22O11 + ____ O2
____ CO2 + ____ H2O
a)

13

b)

18

c)

12

d)

11

e)

7

MASS-MASS STOICHIOMETRY PROBLEMS -- Quiz

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3-11.198285

3

Question 1.
How many grams of HCl are produced from 1.23 g TiCl 4 according to the following
reaction?
(Atomic weights: Ti = 47.90, Cl = 35.45, H = 1.008).
TiCl4 + 2 H2O
a)

0.946

b)

0.624

c)

0.388

d)

0.812

e)

0.472

TiO2 + 4 HCl

Question 2.
Aspirin (C9H8O4), which many students take after a chemistry exam, is prepared by
the reaction of salicylic acid (C7H6O3) with acetic anhydride (C4H6O3) according to
the following equation. How many grams of salicylic acid must be used to prepare
two 5 grain aspirin tablets? (1 gram = 15.4 grains)
(Atomic weights: C = 12.01, O = 16.00, H = 1.008).
C7H6O3 + C4H6O3

C9H8O4 + C2H4O2

a)

0.498

b)

0.214

c)

0.999

d)

0.766

e)

0.649

Question 3.
What mass of K3AsO4 can be prepared by the reaction of 7.10 g of H 3AsO4 with an
excess of KOH?
(Atomic weights: K = 39.10; As = 74.92; O = 16.00; H = 1.008).
H3AsO4 + 3 KOH
a)

12.8

b)

10.1

c)

11.9

d)

11.4

e)

10.8

K3AsO4 + 3 H2O

LIMITING REAGENT -- Quiz

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3-12.198331

Question 1.

3

What mass of PbI2 will precipitate when 2.57 g Pb(NO3)2 reacts with 2.28 g of KI?
(Atomic weights: Pb = 207.2, I = 126.90, N = 14.01, O = 16.00, K = 39.10).
Pb(NO3)2 + 2 KI
a)

3.97

b)

2.14

c)

4.19

d)

3.17

e)

2.58

PbI2 + 2 KNO3

Question 2.
How many grams of ClF3 can be produced from 12.4 g of chlorine and 14.0 g of
fluorine?
(Atomic weights: Cl = 35.45, F = 19.0).
Cl2 + 3 F2
a)

19.3

b)

26.4

c)

21.3

d)

22.7

e)

20.1

2 ClF3

Question 3.
Silver tarnishes in the presence of hydrogen sulfide according to the following
equation. How much Ag2S is produced from a mixture of 0.950 g Ag, 0.140 g H2S
and 0.0800 g O2?
(Atomic weights: Ag = 107.89, O = 16.00, H = 1.008, S = 32.06).
4 Ag + 2 H2S + O2

2 Ag2S + 2 H2O

a)

1.32

b)

1.07

c)

1.45

d)

1.02

e)

1.21

PERCENT YIELD WITH LIMITING REAGENTS -- Quiz

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3-14.198384

3

Question 1.
The mass of S2Cl2 formed when 6.00 g of sulfur reacts with 6.00 g of chlorine is
9.5 g. What is the percent yield?
(Atomic weights: S = 32.06, Cl = 35.45).
S8 + 4 Cl2

Question 2.

a)

83.1

b)

84.8

c)

81.3

d)

82.4

e)

80.5

4 S2Cl2

The mass of Li2O formed when 2.00 g of lithium reacts with 2.00 g of oxygen is
3.02 g. What is the percent yield?
(Atomic weights: Li = 6.94, O = 16.00).
4 Li + O2
a)

80.7

b)

83.8

c)

81.3

d)

82.0

e)

78.2

2 Li2O

Question 3.
The mass of H2 produced by reaction of 1.60 g Fe and 2.00 g HCl is 0.0505 g. What
is the percent yield?
(Atomic weights: Fe = 55.85, Cl = 35.45, H = 1.008).
Fe + 2 HCl
a)

91.3

b)

92.4

c)

89.8

d)

90.4

e)

88.9

FeCl2 + H2

DETERMINE MOLES FROM VOLUME AND MOLARITY -- Quiz

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3-16.198430

3

Question 1.
Determine the number of moles of solute present in 416 mL of 3.75 M HBr
solution.
(Atomic weights: Br = 79.9, H = 1.008).

a)

1.98

b)

1.89

c)

1.56

d)

1.71

e)

1.23

Question 2.
Determine the number of moles of solute present in 152 mL of 1.24 M NaClO 3.
(Atomic weights: Cl = 35.45, O = 16.00, Na = 22.99).

Question 3.

a)

0.212

b)

0.112

c)

0.188

d)

0.142

e)

0.0922

Determine the number of moles of solute present in 2.50 mL of 0.1812 M KMnO 4
solution.
(Atomic weights: K = 39.10, Mn = 54.94, O = 16.00).

a)

5.24 x 10-4

b)

2.42 x 10-4

c)

4.53 x 10-4

d)

1.83 x 10-4

e)

3.12 x 10-4

DETERMINE MASS FROM MOLARITY AND VOLUME -- Quiz

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3-17.198547

3

Question 1.
Determine the mass (g) of solute required to form 275 mL of a 0.4230 M KClO 3
solution.
(Atomic weights: K = 39.10, O = 16.00, Cl = 35.45).

a)

12.2

b)

14.3

c)

19.6

d)

1.97

e)

4.21

Question 2.
Determine the mass (g) of solute required to form 450.0 mL of a 1.00 M HCl
solution.
(Atomic weights: H = 1.008, Cl = 35.45).

a)

29.5

b)

16.4

c)

24.2

d)

18.6

e)

22.2

Question 3.
Determine the mass (g) of solute required to form 250.0 mL of a 0.250 M NaCN
solution.
(Atomic weights: Na = 22.99, C = 12.01, N = 14.01).

a)

2.72

b)

3.06

c)

2.91

d)

3.21

e)

2.51

DILUTION OF SOLUTIONS -- Quiz

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3-20.198620

3

Question 1.
A solution is prepared by dissolving 516.5 mg of oxalic acid (C 2H2O4) to make
100.0 mL of solution. A 10.00 mL portion is then diluted to 250.0 mL. What is the
molarity of the final solution?
(Atomic weights: C = 12.01, H = 1.008, O = 16.00).

a)

5.737 x 10-2

b)

5.738 x 10-2

c)

5.737

d)

2.295 x 10-3

e)

2.295

Question 2.
Fluoxymesterone, C20H29FO3, is an anabolic steroid. A solution is prepared by
dissolving 10.0 mg of the steroid in 500.0 mL of water. A 1.00 mL portion of this
solution is diluted to a final volume of 1.00 L. What is the resulting molarity?
(Atomic weights: C = 12.01, O = 16.00, F = 19.00, H = 1.008).

Question 3.

a)

2.38 x 10-11

b)

1.19 x 10-7

c)

1.19 x 19-10

d)

5.94 x 10-8

e)

5.94 x 10-11

A solution containing Ni2+ is prepared by dissolving 1.485 g of pure nickel in nitric
acid and diluting to 1.00 L. A 10.00 mL aliquot is then diluted to 500.0 mL. What is
the molarity of the final solution?
(Atomic weight: Ni = 58.70).

a)

5.06 x 10-3

b)

0.0253

c)

2.53 x 10-4

d)

5.06 x 10-4

e)

0.0506

SOLUTION STOICHIOMETRY - CALCULATE MOLES OR MASS -- Quiz

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3-21.198693

3

Question 1.
How many moles of calcium carbonate, CaCO3, are required to react with the
sulfuric acid in 375.4 mL of a 0.9734 M solution of H 2SO4?
(Atomic weights: Ca = 40.08, C = 12.01, O = 16.00).
CaCO3(s) + H2SO4(aq)
CaSO4(s) + H2O + CO2
a)

0.1256

b)

0.1829

c)

0.3654

d)

0.8238

e)

0.7132

Question 2.
How many moles of silver nitrate, AgNO3, are required to react with the calcium
chloride in 14.96 mL of a 2.244 M solution of CaCl2?
2 AgNO3(aq) + CaCl2(aq)
2 AgCl(s) + Ca(NO3)2(aq)
a)

1.343 x 10-1

b)

3.357 x 10-2

c)

6.715 x 10-2

d)

3.357 x 10-3

e)

1.343 x 10-2

Question 3.
How many moles of sodium hydroxide, NaOH, are required to react with the
hydrochloric acid in 225 mL of a 0.100 M HCl solution?
(Atomic weights: O = 16.00, H = 1.008, Cl = 35.45, Na = 22.99).
NaOH(aq) + HCl(aq)
a)

2.25 x 10-1

b)

2.25 x 10-3

c)

2.25 x 10-2

NaCl(aq) + H2O(l)

d)

4.44 x 10-2

e)

4.44 x 10-1

SOLUTION STOICHIOMETRY - DETERMINE VOLUME -- Quiz

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3-22.198748

3

Question 1.
What volume, in L, of 0.0385 M ScCl3 is required to react with 22.0 mL of 0.130 M
AgNO3?
(Atomic weights: Sc = 44.96, Cl = 35.45, Ag = 107.87, N = 14.01, O = 16.00).
ScCl3 + 3 AgNO3
a)

0.0690

b)

0.0315

c)

0.454

d)

0.0742

e)

0.0248

3 AgCl + Sc(NO3)3

Question 2.
What volume of 0.0916 M BaCl2 will react completely with 0.475 g of Na2SO4?
(Atomic weights: Ba = 137.33, S = 32.01, Cl = 35.45, Na = 22.99, O = 16.00).
BaCl2 + Na2SO4

BaSO4 + 2 NaCl

a)

33.4

b)

31.2

c)

41.6

d)

28.8

e)

36.5

Question 3.
What volume, in mL, of 0.1130 M AgNO3 is required to react with 10.00 mL of
0.09410 M K2CrO4 to form Ag2CrO4?
(Atomic weights: Ag = 107.87, Cr = 52.00, K = 39.10, N = 14.01, O = 16.00).
2 AgNO3 + K2CrO4
a)

23.25

b)

8.33

c)

14.22

d)

11.62

e)

16.65

Ag2CrO4 + 2 KNO3

STOICHIOMETRY - DETERMINE MOLARITY -- Quiz

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3-23.198820

Question 1.

3

The titration of 25.0 mL of potassium dichromate solution with 0.0350 M Fe 2+
solution requires 27.5 mL of the iron solution. What is the molarity of the
potassium dichromate?
(Atomic weights: Fe = 55.85, Cr = 52.00, O = 16.000, H = 1.008).
14 H+ + 6 Fe2+ + Cr2O726 Fe3+ + 2 Cr3+ + 7 H2O
a)

0.0642

b)

0.0385

c)

0.0231

d)

0.231

e)

0.00642

Question 2.
A 5.00 mL solution of battery acid (H2SO4) requires 16.25 mL of 2.19 M sodium
hydroxide solution. What is the molarity of the sulfuric acid?
2 NaOH + H2SO4
a)

5.25

b)

7.12

c)

0.356

d)

0.712

e)

3.56

Na2SO4 + 2 H2O

Question 3.
What is the molar concentration Sn2+ ions in a solution if 500 mL are titrated with
21.35 mL of 0.1065 M Ce4+ solution?
(Atomic weights: Ce = 140.12, Sn = 118.68).
2 Ce4+ + Sn2+

2 Ce3+ + Sn4+

a)

4.55 x 10-2

b)

9.10 x 10-3

c)

1.13 x 10-3

d)

4.55 x 10-3

e)

2.27 x 10-3

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