CHEMISTRY REVIEW



HONORS CHEMISTRY REVIEW

1. Classify each of the following as a chemical or a physical change:

a) grass growing, b) sugar dissolving in water, c) crushing a rock,

d) cooking potatoes, e) bleaching clothes, f) boiling water.

2. The melting point of silver is 9620C. Express this temperature in

Kelvin.

3. Classify each of the following as an element, compound or mixture:

a) an egg, b) a cake, c) dry ice (CO2), d) iron powder.

4. Identify the larger quantity in each of these pairs of measurements:

a) centigram and milligram d) cubic decimeter and milliliter

b) decileter and kiloliter e) micrometer and nanometer

c) millisecond and microsecond

5. How many significant figures are there in each of these measurements?

a) 5.12 g, b) 3.456 x 106 kg, c) 0.000078 dm3, d) 0.04504 mm,

e) 985.20 K, f) 65.02 s.

6. Round each of the following measurements to two significant figures:

a) 4.607 mg, b) 4.35 x 104 km, c) 0.00150 mL, d) 60.09 kg.

7. What is the mass of 5.42 cm3 of platinum? The density of platinum is

22.5 g/cm3.

8. An aquarium measures (55.0 cm)(1.10 m)(80.0 cm). How many cm3 of

water will this aquarium hold?

9. Make the following conversions:

a) 775 mL to microliters

b) - 650C to K

c) 8.32 mg of Ag to centigrams of silver

10. How many protons and electrons are in each of these ions?

a) magnesium ion c) strontium ion

b) bromide ion d) sulfide ion

11. A student finds that 6.62 g of a substance occupies a volume of

12.3 cm3. What is the density of the substance?

12. Name these compounds. a) Fe(OH)3 b) NH4I c) Na2CO3 d) CCl4

13. Write the formulas for the following compounds.

a) potassium nitrate c) magnesium nitride

b) copper (II) oxide d) silver fluoride

14. Calculate the number of moles in each of the following substances.

a) 54.0 L of nitrogen dioxide at STP.

b) 1.68 g of magnesium ions

c) 69.6 g of sodium hypochlorite

d) 4.27 x 1024 molecules of carbon monoxide

15. Many coffees and colas contain the stimulant caffeine. The percent

composition of caffeine is 49.5% C, 5.20% H, 16.5% O, and 28.9% N.

What is the molecular formula of caffeine if its molar mass is

194.1 g/mol?

16. How many grams of beryllium are in 147 g of the mineral beryl,

Be3Al2Si6O18?

17. Balance these equations.

a) V2O5 + H2 ( V2O3 + H2O

b) (NH4)2Cr2O7 ( Cr2O3 + N2 + H2O

c) NH3 + O2 ( NO + H2O

d) C6H14 + O2 ( CO + H2O

18. Perchloric acid is formed by the reaction of water with dichlorine

heptoxide. Cl2O7 + H2O ( HClO4

a) How many grams of Cl2O7 must be reacted with an excess of H2O

to form 56.2 g of HClO4?

b) How many mL of water are needed to form 3.40 mol of HClO4?

19. How many moles are there of each substance?

a) 888 g of sulfur dioxide

b) 2.84 x 1022 molecules of ammonia

c) 0.47 L of carbon dioxide (at STP)

20. Calculate the heat required, in Joules and in calories, to change 15.00 g

ice at – 10.00C to water at 15.00C.

21. What fraction of the average kinetic energy of hydrogen gas at 100 K

does hydrogen gas have at 40 K?

22. Calculate the molar mass of each of these substances.

a) Ca(CH3CO2)2 c) C12H22O11

b) H3PO4 (aq) d) Pb(NO3)2

23. Name these compounds.

a) SnBr2 b) BaSO4 c) Mg(OH)2 d) IF5

24. An atom of lead-206 weighs 17.16 times as much as an atom of carbon.

a) What is the molar mass of this isotope of lead?

b) How many protons, electrons and neutrons are in this atom of lead?

25. Write a balanced chemical equation for each of these chemical reactions.

a) Calcium reacts with water to form calcium hydroxide and hydrogen

gas.

b) Tetraphosphorous decoxide reacts with water to form phosphoric

acid.

c) Mercury and oxygen are prepared by heating mercury (II) oxide.

d) Aluminum hydroxide and hydrogen sulfide form when aluminum sulfide

reacts with water.

26. How many kilojoules and kcal of heat are required to raise 40.0 g of

water from – 12.00C to 130.00C?

27. Classify each of the reactions in problem #25.

28. Calculate the molecular formula of each of these compounds.

a) The empirical formula is C2H4O and the gmm = 88.0 g/mol

b) The empirical formula is CH and the gmm = 104.0 g/mol

c) The gmm = 90.0 g/mol. The percent composition is 26.7% C,

71.1% O, and 2.2%H.

29. A piece of metal has a mass of 9.92 g and measures 4.5 cm x 1.3 cm x

1.6 mm. What is the density of the metal?

30. Calculate the percent composition of 2-propanol, C3H7OH.

31. Aluminum oxide is formed from its elements.

Al + O2 ( Al2O3

a) Balance the equation.

b) How many grams of each reactant are needed to form 583 g of Al2O3?

32. The temperature of a gas at STP is changed to 125.00C at constant

volume. Calculate the final pressure of the gas in atmospheres.

33. A 2.00 L flask at 27.00C contains 4.40 g of carbon dioxide and 2.00 g

of nitrogen gas. What is the pressure, in atmospheres, of each of the

two components?

34. Balance the following equations.

a) Ag + S ( Ag2S

b) Na2SO4 + Ba(OH)2 ( BaSO4 + NaOH

c) Zn + HNO3 ( Zn(NO3)2 + H2

d) H2O + SO2 + O2( H2SO4

35. The smelting of iron ore consists of heating the ore with carbon.

2 Fe2O3 + 3 C ( 4 Fe + 3 CO2

What mass of iron can be obtained from 100.0 g of the ore?

36. Distinguish among gases, liquids, and solids with respect to shape,

volume, relative density, and motion of particles.

37. What is the volume in liters occupied by 8.0 g of oxygen gas at STP?

38. Use the gas laws and the kinetic theory to complete these

statements. Unless otherwise stated, assume a constant

amount of gas.

a) As the volume of a gas increases at constant temperature,

its pressure _______________.

b) As the temperature of a gas increases and its pressure

decreases, its volume ____________.

c) At constant pressure, a decrease in the volume of a gas is

caused by a/an __________ in its temperature.

d) An increase in the volume and pressure of a gas is caused by

a/an ___________ in its temperature.

e) At constant volume, a decrease in the temperature of a gas

causes the pressure to ___________.

f) If the volume of a gas is increased while its temperature is

increased, the pressure will ____________.

39. Calculate the number of molecules in4.5 x 10-3 grams of H2O.

40. The normal boiling point of a substance depends on both the molecular

mass and the intermolecular attractions. Considering these, arrange the

following in order of decreasing boiling points and explain your answers.

a) HBr, HCl, H2O

b) NH3, H2O, CH4

41. Explain the following terms as they are applied to solutions.

a) solute e) supersaturated

b) solvent f) nonelelectrolyte

c) saturated g) weak electrolyte

d) unsaturated h) strong electrolyte

42. Use ionic charges as a guide to write the formulas for each of the

following compounds.

a) calcium chloride e) barium carbonate

b) aluminum sulfide f) ammonium nitrate

c) magnesium nitrate g) potassium sulfate

d) aluminum carbonate h) aluminum phosphate

43. How would you prepare 400.0 mL of a 0.680 M KOH solution?

44. How would each change affect the position of equilibrium of this

reaction?

2 H2 (g) + O2 (g) ( 2 H2O (g) + heat

a) increasing the pressure

b) adding a catalyst

c) increasing the concentration of H2 (g)

d) cooling the reaction

e) removing water vapor from the container

45. Calculate the pH of solutions with the following hydrogen ion

concentrations.

a) 4.6 x 10-6 M c) 3.0 x 10-1 M

b) 5.0 x 10-12 M d) 9.8 x 10-10 M

46. Determine the oxidation number of phosphorous in each substance.

a) P4O8 d) P4O6

b) PO43- e) H2PO4-

c) P2O5 f) PO33-

47. Calculate the pH of solutions with the following hydrogen ion or

hydroxide ion concentrations.

a) (H+( = 0.00001 M c) (OH-( = 1 x 10-1 M

b) (OH-( = 1 x 10-4 M d) (H+( = 3 x 10-7 M

48. How many mL of a 4.00 M KOH solution are needed to neutralize

45.0 mL of a 2.5 M H2SO4 solution?

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