web viewchemistry 11 midterm review questions. 1.an old barometer hanging on the wall of a mountain...

CHEMISTRY 11 ANSWERS TO REVIEW SHEET

Chemistry 11 Midterm Review Questions

1. An old barometer hanging on the wall of a mountain hut has a reading of 25.5 inches of mercury. If 1 inch of mercury equals 0.0334 atm (atmoshperes) and 1 atm = 101.3 kPa and 1 kPa = 7.50 torr. What is the pressure reading of the barometer in torr?

2. If sugar is $9.80 for 10 kg, what is the cost of: (a) 90.0 kg of sugar? (b) 6.00 tonnes of

sugar (recall 1 tonne = 1000 kg)?

QUANTITY WRITTEN UNIT UNIT SYMBOL

length

mass

time

amount of substance

volume

WRITTEN PREFIX AND UNIT PREFIX AND UNIT SYMBOLS EXPONENTIAL EQUIVALENTS

1.3 kilograms

1.25 µmol

7.25 x 106 t

37.5 mmol

38.3 dekametres

93.5 cL

REVIEW FOR FINAL EXAMINATION


3. Convert the following:

(a) 2.25 mL into L (c) 3125 ML into kL (e) 25 cm/µs into km/s

4. If 1 L of granite has a mass of 5.50 kg,

(a) what is the mass of 7.00 L of granite?

(b) what is the volume occupied by 22 kg of granite?

5. A student measured the volume of an iron nail to be 0.880 mL and found that the mass was 6.92 g. What is the density of the iron?

6. A sample of vegetable oil had a density of 0.916 g/mL. Calculate the mass of 0.250 L of the oil.

7. What volume would 2.86 g of silver occupy? The density of silver is 10.5 g/mL.

8. Write the following numbers in scientific notation:

(a) 23 000 (c) 21 700 000 (e) 95 007 000

9. Write the following numbers in decimal notation:

(a) 2.25 x 103 (c) 3.125 x 10-4 (e) 2.57 x 106

10. How many significant figures does each of the following measurements have?

(a) 3218.04 cm (c) 6.84 x 10-4 mmol (e) 2500 s

(b) 250.000 mL (d) 9 000 000 µs (f) 5.2500 x 10-6 cg



11. Determine the volumes of the following graduated cylinders:

12. Determine the reading on the following scales:

13 State the rule for rounding to the correct number of significant figures after multiplying

or dividing numbers.



14. Perform the indicated operations and the give the answer to the correct number of

significant figures.

(a) 35.8 x 0.12 (d) 1750 x (6.7254 x 102)

(b) 128.62 ÷ 9.25 (e) (6.1428 x 103) ÷ 0.004810

15. In the following mixed calculations perform multiplications and divisions before doing

the additions and subtractions. Keep track of the number of significant figures at each

stage of a calculation.

(a) 65.00 x 0.24000 – 15.78 x 0.148

(d)

(0 .1741+0 .876 )(0 .0147−0 .011)

16. Which of the following statements describe physical properties and which describe chemical properties?

(a) glass is transparent

(b) salt melts at 801°C

(c) Adding lye to fat makes soap

(d) copper conducts electricity

(e) fumes from ammonia and

hydrochloric acid mix to

produce a white smoke

17. Which of the following are intensive properties and which are extensive?

(a) shape

(b) smell

(c) length

(d) colour

(e) time to dissolve

(f) density

18. Briefly describe the characteristics of solids, liquids, and gases.

19. Classify each of the following as one of element, compound, solution, or mechanical

mixture.

(a) gravel (d) iron (g) orange juice

(b) coffee (e) water (h) ammonia



20. Classify each of the following as one of an atom, molecule, or ion.

(a) NH3 (c) Pb (e) SO42-

(b) Cr2O72- (d) PCl5 (f) Co

21. How can you separate all the components in a mixture containing sand, iron filings,

water, gasoline, red water-soluble dye, and blue water-soluble dye? In pure form the

dyes are powders.

22. Which of the following represents the cooling curve for a pure substance. Explain how

you know. (Bonus).

23. Classify each of the following as either a chemical (primarily) or physical change.

(a) formation of fog (d) rusting nail

(b) burning paper (e) dissolving salt into water

(c) plant growing (f) filtering sand and water

24. List 4 characteristics of metals.

25. List 4 characteristics of nonmetals.



26. Indicate which terms apply to each species. There is more than one term which applies to each species.

N (neutral) C (cation) A (anion)

M (monatomic) D (diatomic) P (polyatomic)

(a) SO42- (c) Ba2+ (e) N2H5

+

(b) NH3 (d) ClO- (f) Fe

27. Write the formulae for the following ionic compounds.

(a) calcium dihydrogen phosphate (b) uranium (IV) sulphate

28. Name the following ionic compounds.

(a) Ag3PO4 (b) Na2HPO4

29. Write the formulae for the following covalent compounds.

(a) diphosphorus trichloride (b) oxygen diiodide

30. Name the following covalent compounds.

(a) S4N2 (b) ClF3

31. Write the formulae for the following hydrated compounds.

(a) zinc perchlorate hexahydrate (b) iron (III) sulphate nonhydrate

32. Name the following hydrated compounds.

(a) FeSO4•5H2O (c) Co3(PO4)2•8H2O

33. Write the formulae for the following acids.

(a) sulphuric acid (c) acetic acid

(b) nitric acid (d) hydrochloric acid



34. Name the following acids.

(a) HF (c) H3PO4

(b) H2SO3 (d) HNO2

The Mole Concept

35. Review the following terms: Avogadro’s hypothesis, mole, atomic mass, molar mass,

molar volume, STP, density, empirical formula, molecular formula, empirical mass,

concentration, dilution, molarity.

36. Calculate the molar mass of each of the following.

(a) NCl3 (b) Al2(SO4)3


(a) NiSO4•7H2O (b) Cr(NO3)3•9H2O

38. Calculate the mass of the following.

(a) 4.50 mol of PCl3 (b) 5.64 x 10-5 mol of AuCl3

39. Calculate the number of moles in the following.

(a) 85.6 g of CaO (b) 6.48 kg of KMnO4

40. Calculate the molar mass of 0.00496 mol sample of cholesterol has a mass of 1.894 g

41. What is STP and what are the experimental conditions of STP?



42. Calculate the volume at STP occupied by the following.

(a) 24.8 mol of NH3 (b) 0.0861 mol of HCl

43. Calculate the number of moles in the following gases at STP.

(a) 64.8 L of Xe(g) (b) 645 mL of SO2(g)

44. How many atoms are contained in the following.

(a) 1 molecule of CH3CO2H (b) 2.56 mol of (NH4)3PO4

45. Find the mass, in grams, of each of the following.

(a) 1 Pb atom (b) 5.62 x 1018 Fe(OH)3 molecules

46. How many atoms are contained in each of the following?

(a) 60.5 g of AlCl3 (b) 84.6 mL of HCl(g) at STP

47. What volume at STP is occupied by each of the following?

(a) 8.27 x 1020 molecules of O2(g) (b) 125.0 g of Cl2(g)

48. Calculate the percentage composition of the following.

(a) NaHCO3 (b) CuSO4•5H2O

49. Calculate the percentage composition of the bold species in each of the following.

(a) Cr(NO3)6Cl3•H2O (b) Al2(SO4)3•18H2O



50. Find the empirical formula for the following compounds.

(a) 12.6% Li, 29.2% S, 58.2% O (b) 38.8% Fe, 16.7% C, 44.5% O

51. A gas has the empirical formula CH2. If 0.550 L of the gas at STP has a mass of 3.44 g,

what is the molecular formula?

52. A sample of gas is analyzed and found to contain 33.0% Si and 67.0% F. If the gas has a density of 7.60 g/L at STP, what is the molecular formula?

53. Calculate the molar concentration of the following solutions.

(a) 0.578 mol of NaCl in 52.0 mL of solution

(b) 50.0 g of Fe(NO3)3 in 150.0 mL of solution

54. Calculate the mass of solute needed to make the following solutions.

(a) 125.0 mL of 0.0750 M KOH, from solid KOH

(b) 500.0 mL of 0.120 M FeCl3, from solid FeCl3•6H2O

55. What is the concentration of the solution that results when 250.0 mL of water is added to

550.0 mL of 3.50 M NaOH?

56. If 500.0 mL of 0.100 M LiOH is boiled down to 200.0 mL, what is the concentration?

57. What is the resulting concentration when 500.0 mL of 0.250 M NaCl is mixed with

250.0 mL of 0.450 M NaCl and the mixture is boiled down to 400.0 mL?

58. If 250.0 mL of solution A containing 28.0 g of LiOH is mixed with 500.0 mL of

solution B containing 56.0 g of LiOH and the resulting solution is boiled down to

600.0 mL, what is the concentration?

Unit VI Chemical Reactions59. How can you tell that a chemical reaction has occurred?



60. What is the Law of Conservation of Mass?

61. How can you tell that a chemical equation is balanced?

3. Balance the following chemical reactions:

A. ___ Si4H10 + ___ O2 ___ SiO2 + ___ H2O

B. ___ Ca3(PO4)2 + ___ SiO2 + ___ C ___ CaSiO3 + ___ CO + ___ P4

C. ___ C3H7N2O7 + ___ O2 ___ CO2 + ___ H2O + ___ N2

62. Write and balance the following word equations:

A. Aluminum + Copper (II) sulphate Aluminum sulphate + Copper

___________________________________________________________________

B. Magnesium nitride + Water Magnesium hydroxide + Ammonia (NH3)

___________________________________________________________________

C. Calcium hydroxide + Ammonium chloride Ammonia + Calcium chloride + Water

___________________________________________________________________

63. Complete and balance the following reactions and classify each equation as one of: synthesis, decomposition, single replacement, double replacement, neutralization or combustion.

A. ___ HF + ___ Fe(OH)3 _____________________________________________

B. ___ FeCl2 + ___ K2S _______________________________________________

C. ___ Al + ___ S8 ___________________________________________________

D. ___ N2O _________________________________________________________

E. ___ C3H6OS2 + ___ O2 ______________________________________________

F. ___ Mg + ___ HCl _________________________________________________



64. Define the terms:

A. Exothermic

B. Endothermic

65. Classify the following is exothermic or endothermic:

A. 2Na + 2H2O 2NaOH + H2 + 283 kJ

B. KClO3 + 41.4 kJ K+ + ClO3–

C. C2H6 + O2 CO2 + H2O ∆H = – 3718 kJ

D. 12CO2 + 11H2O C12H22O11 + 12O2 ∆H = +5638 kJ

Unit VII Stoichiometry

66. What are limiting and excess reactants?

67. Consider the reaction: 4C4H9SO2 + 25O2 16CO2 + 18H2O + 4SO2

A. How many oxygen molecules react with 20 molecules of C4H9SO2?

B. How many moles of C4H9SO2 are required to produce 100 moles of water?

C. What mass of SO2 is formed when 50.0 g of C4H9SO2 is reacted?

68. A 25.0 mL sample of Al(OH)3 is titrated with 67.8 mL of 0.450 M HCl according to the reaction

Al(OH)3 + 3HCl AlCl3 + 3H2O

What is the concentration of the original Al(OH)3 solution?



69. What mass of CS2 is produced when 25.8 g of C are reacted with 54.2 g of SO2 according to the equation

5C + 2SO2 CS2 + 4CO

A. What mass of CS2 is produced?

B. What mass of the excess reactant will be left over?

70. Consider the reaction

K2Cr2O7 + 6NaI + 7H2SO4 Cr2(SO4)3 + 3I2 + 7H2O + 3Na2SO4 + K2SO4

A 35.0 g sample of pure K2Cr2O7 produces 9.67 g of H2O. What is the percentage yield

.

72. Fill in the following table:

SYMBOL PROTONS NEUTRON ELECTRONS

Rh

107Pd2+

123Sb3–

93 89

50 46

AnswersREVIEW FOR FINAL EXAMINATION


1. An old barometer hanging on the wall of a mountain hut has a reading of 25.5 inches of mercury. If 1 inch of mercury equals 0.0334 atm (atmoshperes) and 1 atm = 101.3 kPa and 1 kPa = 7.50 torr. What is the pressure reading of the barometer in torr? 647 torr

2. If sugar is $9.80 for 10 kg, what is the cost of: (a) 90.0 kg of sugar? $88.20 (b) 6.00

tonnes of sugar (recall 1 tonne = 1000 kg)? $5.88E3

QUANTITY WRITTEN UNIT UNIT SYMBOL

length Metre M

mass g g

time Second S

amount of substance Mole Mol

volume Litre L

WRITTEN PREFIX AND UNIT PREFIX AND UNIT SYMBOLS EXPONENTIAL EQUIVALENTS

1.3 kilograms 1.3 kg 103

1.25 micromoles 1.25 µmol 1.25 E -6

7.25 megatonnes 7.25 Mt 7.25 x 106 t

37.5 millimoles 37.5 mmol 37.5E-3 mol

38.3 dekametres 38.3dam 38.3 E1 m

93.5 centilitres 93.5 cL 93.5 E-2 L



3. Convert the following:

(a) 2.25 mL into L

2.25E-3L

(c) 3125 ML into kL

3.125E6 kL

(e) 25 cm/µs into km/s

2.5 E 2 km/s

4. If 1 L of granite has a mass of 5.50 kg,

(a) what is the mass of 7.00 L of granite? 38.5 kg

(b) what is the volume occupied by 22 kg of granite? 4L

5. A student measured the volume of an iron nail to be 0.880 mL and found that the mass was 6.92 g. What is the density of the iron? 7.86 g/mL

6. A sample of vegetable oil had a density of 0.916 g/mL. Calculate the mass of 0.250 L of the oil. 229g

7. What volume would 2.86 g of silver occupy? The density of silver is 10.5 g/mL.. 0.272mL

8. Write the following numbers in scientific notation:

(a) 23 000, 2.3E4 (c) 21 700 000, 2.17E7 (e) 95 007 000,

9.5007E7

9. Write the following numbers in decimal notation:

(a) 2.25 x 103, 2250 (c) 3.125 x 10-4,

0.0003125

(e) 2.57 x 106

2 570 000

10. How many significant figures does each of the following measurements have?

(a) 3218.04 cm 6 (c) 6.84 x 10-4 mmol 3 (e) 2500 s 2

(b) 250.000 mL 6 (d) 9 000 000 µs 1 (f) 5.2500 x 10-6 cg 5



11. Determine the volumes of the following graduated cylinders:

54.2+/-.1 82+/-1 38.0+/-.5

12. Determine the reading on the following scales:

15.17+-.01 15.69+-.01

10.0+-.02 16.4+-.02

6.40+-.05 7.60+-.05

13 State the rule for rounding to the correct number of significant figures after multiplying

or dividing numbers. Lowest number for mult and div, only one uncertain column for

add and sub



14. Perform the indicated operations and the give the answer to the correct number of

significant figures.

(a) 35.8 x 0.12 =4.3 (d) 1750 x (6.7254 x 102)=1.18E6

(b) 128.62 ÷ 9.25=13.9 (e) (6.1428 x 103) ÷ 0.004810=

1.277E6

15. In the following mixed calculations perform multiplications and divisions before doing

the additions and subtractions. Keep track of the number of significant figures at each

stage of a calculation.

(a) 65.00 x 0.24000 – 15.78 x 0.148

=13.26 (d)

(0 .1741+0 .876 )(0 .0147−0 .011) =3E2

16. Which of the following statements describe physical properties and which describe chemical properties?

(a) glass is transparent P

(b) salt melts at 801°C P

(c) Adding lye to fat makes soap C

(d) copper conducts electricity P

(e) fumes from ammonia and

hydrochloric acid mix to

produce a white smoke C

17. Which of the following are intensive properties and which are extensive?

(a) shape e

(b) smell i

(c) length e

(d) colour i

(e)time to dissolve e

(f) density i

18. Briefly describe the characteristics of solids (fixed shape and volume, particles touching

with only vibrations), liquids (fixed volume, particles can slide past one another, and

gases (particles move quickly and are separated by lots of space).



19. Classify each of the following as one of element, compound, solution, or mechanical

mixture.

(a) gravel m (d) iron e (g) orange juice m

(b) coffee s (e) water c (h) ammonia c

20. Classify each of the following as one of an atom, molecule, or ion.

(a) NH3 m (c) Pb a (e) SO42- i

(b) Cr2O72- i (d) PCl5 m (f) Co a

21. How can you separate all the components in a mixture containing sand, iron filings,

water, gasoline, red water-soluble dye, and blue water-soluble dye? In pure form the

dyes are powders…magnet (iron), filter (sand), sep funnel (gas), evaporate (water),

chromatography (dyes)



22. Which of the following represents the cooling curve for a pure substance. Explain how

you know.

c cooling and plateus at phase change

23. Classify each of the following as either a chemical (primarily) or physical change.

(a) formation of fog p (d) rusting nail c

(b) burning paper c (e) dissolving salt into water p

(c) plant growing c (f) filtering sand and water p

24. List 4 characteristics of metals. Shiny, ductile, malleable, conductor

25. List 4 characteristics of nonmetals. Brittle, dull, poor conductor, usually gas

26. Indicate which terms apply to each species. There is more than one term which applies to each species.

N (neutral) C (cation) A (anion)

M (monatomic) D (diatomic) P (polyatomic)


(a) A, P, SO42- (c) C, M, Ba2+ (e) C, P, N2H5

+

(b) N, P, NH3 (d) A, D, ClO- (f) N, M, Fe


27. Write the formulae for the following ionic compounds.

(a) calcium dihydrogen phosphate

Ca2(H2PO4)2

(b) uranium (IV) sulphate

U(SO4)2

28. Name the following ionic compounds.

(a) Ag3PO4

Silver phosphate

(b) Na2HPO4

sodium monohydrogen phosphate

29. Write the formulae for the following covalent compounds.

(a) diphosphorus trichloride P2Cl3 (b) oxygen diiodide OI2

30. Name the following covalent compounds.

(a) S4N2 tetrasulphur dinitride (b) ClF3 Chlorine trifluoride

31. Write the formulae for the following hydrated compounds.

(a) zinc perchlorate hexahydrate

Zn(ClO4)2.6H2O

(b) iron (III) sulphate nonhydrate

Fe2(SO4)3.9H2O

32. Name the following hydrated compounds.

(a) FeSO4•5H2O

Iron (II) sulphate pentahydrate

(b) Co3(PO4)2•8H2O

Cobalt (II) phosphate octahydrate

33. Write the formulae for the following acids.

(a) sulphuric acid H2SO4 (c) acetic acid CH3COOH

(b) nitric acid HNO3 (d) hydrochloric acid HCl

34. Name the following acids.

(a) HF hydrofluoric acid (c) H3PO4 phosphoric acid

(b) H2SO3 sulphurous acid (d) HNO2 nitrous acid



The Mole Concept


(b) NCl3

120.5g/mol

(c) Al2(SO4)3

342.3g/mol


(a) NiSO4•7H2O

280.8g/mol

(b) Cr(NO3)3•9H2O

400.0g/mol

38. Calculate the mass of the following.

(a) 4.50 mol of PCl3

619 g

(b) 5.64 x 10-5 mol of AuCl3

0.0171 g

39. Calculate the number of moles in the following.

(a) 85.6 g of CaO

1.53 mol

(b) 6.48 kg of KMnO4

41.0 mol

40. Calculate the molar mass of 0.00496 mol sample of cholesterol has a mass of 1.894 g.

382 g/mol

41. What is STP and what are the experimental conditions of STP? Standard temp (0-oC) and

pressure (101.3 kPa)

42. Calculate the volume at STP occupied by the following.

(c) 24.8 mol of NH3

556 L

(c) 0.0861 mol of HCl

1.93L

43. Calculate the number of moles in the following gases at STP.

(a) 64.8 L of Xe(g)= 2.89 mol (b) 645 mL of SO2(g) = 2.88E-2 mol

44. How many atoms are contained in the following.



(a) 1 molecule of CH3CO2H

8

(b) 2.56 mol of (NH4)3PO4

3.08E25

45. Find the mass, in grams, of each of the following.

(a) 1 Pb atom

3.44E-22 g

(b) 5.62 x 1018 Fe(OH)3 molecules

9.97E-4 g

46. How many atoms are contained in each of the following?

(a) 60.5 g of AlCl3= 1.09E24 (b) 84.6 mL of HCl(g) at STP=

4.55E21

47. What volume at STP is occupied by each of the following?

(a) 8.27 x 1020 molecules of O2(g)

30.1mL

(b) 125.0 g of Cl2(g)

39.4L

48. Calculate the percentage composition of the following.

(a) Na (27.4)H (1.2)C (14.3) O3(57.1) (c) CuSO4•5H2O

Cu-25.4, S-12.1, O-57.7, H-4.0

49. Calculate the percentage composition of the bold species in each of the following.

(a) Cr(NO3)6Cl3•H2O

67.8%

(b) Al2(SO4)3•18H2O

43.3%

50. Find the empirical formula for the following compounds.

(a) 12.6% Li, 29.2% S, 58.2% O

Li2SO4

(b) 38.8% Fe, 16.7% C, 44.5% O

FeC2O4

51. A gas has the empirical formula CH2. If 0.550 L of the gas at STP has a mass of 3.44 g,

what is the molecular formula? C10H20



52. A sample of gas is analyzed and found to contain 33.0% Si and 67.0% F. If the gas has a density of 7.60 g/L at STP, what is the molecular formula? Si2F6

53. Calculate the molar concentration of the following solutions.

(a) 0.578 mol of NaCl in 52.0 mL of solution. 11.1M

(b) 50.0 g of Fe(NO3)3 in 150.0 mL of solution 1.38M

54. Calculate the mass of solute needed to make the following solutions.

(a) 125.0 mL of 0.0750 M KOH, from solid KOH 0.526g

(b) 500.0 mL of 0.120 M FeCl3, from solid FeCl3•6H2O

55. What is the concentration of the solution that results when 250.0 mL of water is added to

550.0 mL of 3.50 M NaOH? 2.41M

56. If 500.0 mL of 0.100 M LiOH is boiled down to 200.0 mL, what is the concentration?

0.25M

57. What is the resulting concentration when 500.0 mL of 0.250 M NaCl is mixed with

250.0 mL of 0.450 M NaCl and the mixture is boiled down to 400.0 mL?0.594M

58. If 250.0 mL of solution A containing 28.0 g of LiOH is mixed with 500.0 mL of

solution B containing 56.0 g of LiOH and the resulting solution is boiled down to

600.0 mL, what is the concentration? 5.86M

Unit VI Chemical Reactions59. How can you tell that a chemical reaction has occurred?

New properties due to new substances.

(d) What is the Law of Conservation of Mass?

Mass of products = mass of reactants in a closed reaction

60. How can you tell that a chemical equation is balanced?

a. Equal #s of atoms on each side



61. Balance the following chemical reactions:

A. 2 Si4H10 + 13 O2 8 SiO2 + 10 H2O

B. 2 Ca3(PO4)2 + 6 SiO2 + 10 C 6 CaSiO3 + 10 CO + 1 P4

C. 4C3H7N2O7 + 5 O2 12 CO2 + 14 H2O + 4 N2

62. Write and balance the following word equations:

A. Aluminum + Copper (II) sulphate Aluminum sulphate + Copper

2Al + 3CuSO4 1Al2(SO4)3 + 3Cu

B. Magnesium nitride + Water Magnesium hydroxide + Ammonia (NH3)

1Mg3N2 + 6H2O 3Mg(OH)2 + 2NH3

C. Calcium hydroxide + Ammonium chloride Ammonia + Calcium chloride + Water

1Ca(OH)2 + 2NH4Cl 2NH3 + 1CaCl2 + 2H2O

63. Complete and balance the following reactions and classify each equation as one of: synthesis, decomposition, single replacement, double replacement, neutralization or combustion.

A. 3 HF + 1 Fe(OH)3 neut 3H2O + 1FeF3

B. 1 FeCl2 + 1K2S dr 1FeS + 2KCl

C. 16 Al + 3 S8 syn 8Al2S3

D. 2N2O decom 2N2 + 1O2

E. 1C3H6OS2 + ___ O2 combust 3CO2 + 3H2O + 2SO2

F. 1 Mg + 2 HCl s.r. 1MgCl2 + 2H2

64. Define the terms:

A. Exothermic

Heat exits the system

B. Endothermic

Heat enters the system



65. Classify the following is exothermic or endothermic:

A. 2Na + 2H2O 2NaOH + H2 + 283 kJ ex

B. KClO3 + 41.4 kJ K+ + ClO3– en

C. C2H6 + O2 CO2 + H2O ∆H = – 3718 kJ ex

D. 12CO2 + 11H2O C12H22O11 + 12O2 ∆H = +5638 kJ en

Unit VII Stoichiometry

65. What are limiting (runs out and determines the amount of product) and excess (there is more than is needed to fully react with the limiting reactant )reactants?

66. Consider the reaction: 4C4H9SO2 + 25O2 16CO2 + 18H2O + 4SO2

A. How many oxygen molecules react with 20 molecules of C4H9SO2?

125

B. How many moles of C4H9SO2 are required to produce 100 moles of water?

22.2

C. What mass of SO2 is formed when 50.0 g of C4H9SO2 is reacted? 26.5g

67. A 25.0 mL sample of Al(OH)3 is titrated with 67.8 mL of 0.450 M HCl according to the reaction

Al(OH)3 + 3HCl AlCl3 + 3H2O

What is the concentration of the original Al(OH)3 solution? 0.407M

68. What mass of CS2 is produced when 25.8 g of C are reacted with 54.2 g of SO2 according to the equation

5C + 2SO2 CS2 + 4CO

A. What mass of CS2 is produced? 32.2g

B. What mass of the excess reactant will be left over? 0.4g C



69. Consider the reaction

K2Cr2O7 + 6NaI + 7H2SO4 Cr2(SO4)3 + 3I2 + 7H2O + 3Na2SO4 + K2SO4

A 35.0 g sample of pure K2Cr2O7 produces 9.67 g of H2O. What is the percentage yield? 64.5%

Unit VIII Atoms, Periodic Table, and Bonding71. Fill in the following table:

SYMBOL PROTONS NEUTRON ELECTRONS

Rh 45 58 45

107Pd2+ 46 61 44

123Sb3– 51 72 54

237Np4+ 93 144 89

119Sn4+ 50 69 46


web viewchemistry 11 midterm review questions. 1.an old barometer hanging on the wall of a mountain...

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