Chemistry 1-2 HD Review Problem Set



Review Semester 2 Final 2008 Name ___________________________

Physical or chemical change

boiling water

burning wood

melting aluminum

separating sand from water

Element names/symbols 

know element symbols from quiz on symbols

Metric prefixes (centi-, milli-, kilo-) 

Convert 54 mm to m.

Convert 9.2 X 10-5 cL to L.

Convert 5.12 kg to g.

Celcius to Kelvin conversion OR Kelvin to Celcius

Convert 23 degrees C to Kelvin

Convert 50 K to degrees C

Significant digits

Round 8.9456 to 3 significant digits.

Round 513431 to 2 significant digits.

Add 4.324 + 345.1, and round your answer properly.

Multiply 32.56 X 103, and round your answer properly.

Scientific notation

Express 3712 in scientific notation.

Express 0.0377561 in scientific notation.

Density What is the volume of a solid with a density of 7.8 g/mL and a mass of 11.8 g ?

Unit conversions (you should know these conversions

Convert 54 hours to seconds

Convert 84 mg to grams

Convert 1234 m to km

Convert 2.3 L to mL

Protons, Neutron, Electrons

|Symbol |Protons |Neutrons |Electrons |Charge |

| |4 |5 | |0 |

| |47 |61 | |0 |

|[pic] | | | | |

| |16 |17 | |-2 |

| |13 |15 | |+3 |

| | |47 |35 |-1 |

|[pic] | | | | |

|[pic]-2 | | | | |

|[pic]-2 | | | | |

Nomenclature  {naming compounds, writing formulas}

Write the formula for each of the following compounds:

1. Sulfur hexafluoride

2. Lithium nitride

3. Chromium (III) carbonate

4. Tin (II) chloride

5. Ammonium acetate

6. Mercury (I) chloride

7. Potassium bromate

8. Sulfuric acid

9. Chloric acid

Name each of the following compounds.

1. CuSO4

2. AlF3

3. HI

4. NO

5. H2Se (aq)

6. HNO3

7. NaHSO4

Mole conversions & molar mass

Convert 2.34 moles of H2O to molecules

Convert 36 grams of H2O to moles

Convert 98 grams of Na to atoms

Convert 4.32 X 1021 molecules of SO2 to moles

Convert 2.1 X 1024 atoms of Mg to grams

Balance these equations:

1. _____Ca(OH)2(s) + _____HCl(aq) ---> ____CaCl2(aq) + _____H2O(l)

2. _____Ag2O(s) ---> _____Ag(s) + _____O2(g)

3. _____C4H10(g) + _____O2(g) ---> _____CO2(g) + _____H2O(g)

4 _____Al(s) + _____H2SO4 (aq) ---> _____Al2(SO4)3(aq) + _____H2(g)

Find the molecular weight of each compound.

|5. BaI2 |6. AgC2H3O2 |

Convert.

7. 0.4 moles of Sn to atoms

8. 32 g of K2O to molecules

9. 800 g of CaCl2 to moles

10. 0.75 moles of H2O to grams

11 9.0 g of Cl2 to atoms

Empirical and Molecular Formulas

12. NutraSweet is 57.14% C, 6.16% H, 9.52% N, and 27.18% O.  Calculate the empirical formula of NutraSweet and find the molecular formula.  (The molar mass of NutraSweet is 294.30 g/mol)

Stoichiometry

13. Na + I2 ---> NaI If 2.8 grams of sodium were used for the reaction, and an excess of iodine was present, how many moles of sodium iodide would be produced?

14. Pb(NO3)2 + K2CrO4 --> PbCrO4 + 2 KNO3

If you started with 0.97 g of K2CrO4 and excess Pb(NO3)2, how many grams of KNO3 could be produced?

Reactions. Complete and balance.

15. K2CO3 + BaCl2 --->

16. NaCl + O2 --->

17. Zn(CO3) --->

18. RaCl2 --->

19. C6H6 + O2 --->

20. Ra + Cl2 --->

Gases. Solve.

21. Given 500cm3 of methane gas at 2.5atm and 20oC. What would be the volume of the gas at STP?

22. What pressure is exerted by 2 moles of a gas in a 500 cm3 container at 25oC?

23. Two hundred cubic centimeters of a gas are collected by water displacement. The conditions at time are 1.1atm and 30oC. The vapor pressure of water at 30oC is 23.4 mm Hg. What would be the pressure of the dry gas at STP?

24. 2 C2H6 + 7 O2 --> 4 CO2 + 6 H2O

How many milliliters of ethane (C2H6) at STP are required to produce 22 g of carbon dioxide?

Solutions.

25. A solution is prepared by mixing 10.0 grams of benzene (C6H6) in 150 g of water to create a solution total volume of 162 ml. Calculate the molarity of benzene in the solution.

26. If I dilute 200mL of 0.10 M lithium acetate solution to a volume of 750 mL, what will the concentration of this solution be?

Nuclear Chem

27. When the uranium-235 nucleus is struck with a neutron, the zinc-72 and samarium-160 nuclei are produced along with some neutrons. How many neutrons are produced?

A. 3

B. 5

C. 4

D. 6

E. 2

Light and electrons

28. The bright yellow light emitted by a sodium vapor light consists of an emission line with a wavelength of 589.0 nm.

What is the frequency of this light?

What is the energy of a photon of this light?

What is the energy in kJ/mole?

Organic Naming

29. Butane has how many structural isomers?

A. three

B. one

C. five

D. two

E. four

30. Name the following molecule.

A. 3-methylpentane

B. hexane

C. methyl-diethylmethane

D. 3-methyl-hexane

E. 1,2,3-trimethylpropane

31. In lecture, the professor named a molecule 2-ethyl-4-tertiary-butylpentane. An alert student pointed out that although the correct structure could be drawn, the name did not follow systematic rules. What is the correct systematic name for the molecule?

A. 2-butyl-5-methylhexane

B. 2,2,3,5-tetramethylheptane

C. undecane

D. 2-ethyl-4,5,5-trimethylhexane

E. 3,5-dimethylnonane

32. Name the following:

A. 1,1,1-trichloro-5-bromo-2-pentene

B. 1,1,1-trichloro-5-bromo-3-pentene

C. 1,1,1-trichloro-5-bromo-3-pentyne

Titration Lab

33. Calculate the [H+] in a solution that shows a pH of 11.70.

A. 2.0 x 10-12 M

B. 5.0 x 10-3 M

C. 11.7 M

D. 2.3 M

E. None of the above

34. Calculate the [H+] in a solution that shows a pH of 2.30.

A. 5.0 x 10-3 M

B. 2.3 M

C. 2.0 x 10-12 M

D. 11.7 M

E. None of the above

35. A solution has [H+] = 4.0 x 10-8 M. The pH of this solution is

A. 7.40

B. 10.80

C. 6.60

D. 3.20

E. None of the above

36. Determine the volume of 0.100 M NaOH needed to titrate 20.0 mL of 0.400 M HCl.

A. 5.00 mL

B. 60.0 mL

C. 80.0 mL

D. 20.0 mL

E. 40.0 mL

Hydrate Lab

37. Calculate the molecular formula of a compound with the empirical formula CH2O and a molar mass of 150 g/mol.

A. C2H4O2

B. C6H12O6

C. C5H10O5

D. C3H6O3

E. C4H8O4

38. A Calcium Nitrate hydrate was heated in an experiment to release the water. The initial mass was 2.93 grams. The final mass was 1.97 grams. What is the formula of the hydrate?

a. Ca(NO3)2.H2O

b. Ca(NO3)2.2H2O

c. Ca(NO3)2.3H2O

d. Ca(NO3)2.4H2O

e. Ca(NO3)2.5H2O

Heat of Solution Lab

39. The device used to determine the heat associated with a chemical reaction is called a

A. heatometer

B. barometer

C. joulorometer

D. calorimeter

E. None of the above

40. Which of the following is exothermic?

A. A reaction in which the products are higher in potential energy than the reactants.

B. The melting of a solid.

C. The condensation of a gas.

D. Rolling a ball up a hill.

E. None of the above

41. In an endothermic reaction, energy flows

A. into the system.

B. into the surroundings.

C. into the universe.

D. out of the system.

E. None of the above

Enthalpy of Reactions

42. When 1 mole of propane (C3H8) is burned at constant pressure, 2221 kJ of energy is released as heat. Calculate ΔH for a process in which 25.0 g of propane is burned at constant pressure.

A. 740 kJ

B. -1260 kJ

C. 1260 kJ

D. -740 kJ

E. None of the above

IMF’s

43. Of the following substances, choose the one with the greatest vapor pressure.

A. Xe(l)

B. He(l)

C. Ar(l)

D. Rn(l)

E. Ne(l)

44. Which of the following has the highest melting temperature?

A. H2O

B. CO2

C. MgF2

D. S8

E. P4

45. The intermolecular forces called hydrogen bonding will not exist between molecules of

A. H2

B. H2O

C. HF

D. NH3

E. any of these

46. Order the intermolecular forces (dipole-dipole, London dispersion, ionic, and hydrogen bonding) from weakest to strongest.

A. hydrogen bonding, dipole-dipole, London dispersion, ionic

B. London dispersion, ionic, dipole-dipole, hydrogen bonding

C. dipole-dipole, London dispersion, ionic, hydrogen bonding

D. dipole-dipole, ionic, London dispersion, hydrogen bonding

E. London dispersion, dipole-dipole, hydrogen bonding, ionic

47. Which of the following should have the lowest boiling point?

A. N2

B. H2O

C. HF

D. NH3

E. Na2S

48. Which of the following is most likely to be a solid at room temperature?

A. Na2S

B. HF

C. NH3

D. H2O

E. N2

Equilibrium (Le Chatelier’s)

The following question(s) refer to the equilibrium shown here: 4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g)

49. What would happen to the system if oxygen were added?

A. More ammonia would be produced.

B. The equilibrium would shift to the left.

C. Nothing would happen.

D. The equilibrium would shift to the right.

E. The concentration of NO(g) would decrease.

50. What would happen to the system if the total pressure were decreased?

A. More oxygen would be produced.

B. The water vapor would become liquid water.

C. The NO concentration will increase.

D. The ammonia concentration would increase.

E. Nothing would happen.

Periodicity

51. Which of the following has the largest atomic radius?

A. Mg

B. Na

C. O

D. P

E. N

52. Which of the following has the highest ionization energy?

A. N

B. C

C. Ca

D. O

E. K

53. Which of the following has the smallest atomic radius?

A. F

B. N

C. S

D. Br

E. Cl

54. Which of the following atoms has the highest ionization energy?

A. Sb

B. P

C. As

D. Al

E. Si

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