# Worksheet Chapter 1 (WGD)

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```							Name:___________________________                                                         Date:_________________
AP Chemistry – BISD

Summer Review Problems – Complete By First Day, Discuss On 2 nd Day

Show all work for the following dimensional analysis problems on a separate sheet of paper and write the correct
answer below.

___________1. 6.7 cm = ___mm

___________2. 58 liters = ___m3

___________3. 56.000 ft/s = ___in/hr

___________4. 5.0 ft3 = ___cm3 (1in = 2.54cm)

___________5. 300.0 lb/mL= ___g/dm3 (1 lb = 454 g) – SHOW ANSWER IN SCIENTIFIC NOTATION!

Significant digit problems: Write answers in correct number of significant digits.

___________6. 5.67 X 4.6

___________7. 3.44 + 5.6 + 7.80

___________8. 1.3 X 10-5 - 0.0057 (If the answer bothers you, think about it.)

___________9. (2.33 +9.1) / (3.55-1.2)

___________10. Volume of solid sample: 32.52 cm3
Mass of empty container: 2.5 g
Mass of container plus solid sample: 24.7 g
What is the density of the sample with answer showing correct sig figs?

Physical (P) or Chemical (C) Change. List each as a physical change, chemical change, or both.

___________11. Burning wood                          ___________12. Dissolving salt in water

___________13. Melting ice                           ___________14. Souring of milk

___________15. Baking soda on an acid spill

Physical (P) or Chemical (C) Properties. List each as a chemical or physical property.

___________16. Color                        ___________17. Sodium reacts with Chlorine

___________18. Density                      ___________19. Iron rusts

___________20. Melting point

Tell if the following are homogeneous or heterogeneous

___________21. Sugar water solution                  ___________22. Air

___________23. Water                                 ___________24. Milk

___________25. Iron and salt
Which of the following are pure substances: answer yes or no

___________26. Table salt                             ___________27. Water

___________28. Copper Sulfate solution                ___________29. Gold

___________30. Air

Show all work on a separate sheet of paper for #31-#41and write the final answer below each question.

31. The mass ratio of iron to oxygen in ferric oxide, Fe 2O3, is _________ to 1.00.

32. How many grams of aluminum nitrate, Al(NO3)3, contain 18.0 grams of oxygen atoms? ________

33. The simplest formula for a hydrocarbon that is 82.8% carbon is _________

34. How many molecules of nitrogen in 3.5 grams of N 2? _______How many atoms of nitrogen?______

35. How many grams of potassium permanganate contain 27.5 grams of oxygen?__________

36. How many hydrogen atoms are present in 1.00 mole of acetic acid, CH3COOH?____________ How many would be
present in 28.5 grams of acetic acid?________

37. 11.17 grams of iron metal is allowed to react with oxygen. At the end of the reaction, the compound formed has a mass of
14.37 grams. What is the formula of the compound formed?________

38. How many grams of carbon are present in 0.25 moles of butane, C 4H10? _____________ (Do NOT use a calculator!)

39. What is the percent of sulfur in H2SO4?___________

40. What is the simplest formula for a compound that is 26.6% potassium, 35.4% chromium, and 38.0% oxygen?______

41. A 15.0 gram sample of an unknown hydrocarbon is burned in excess oxygen. The combustion forms 48.4 grams of carbon
dioxide and 16.47 grams of water. If the hydrocarbon has a molar mass of 123 g/mole, what is the molecular formula for the
hydrocarbon? __________
Directions: State what type of reaction is occurring. Then write and balance the equation.

EXAMPLE: Sodium metal is added to hydrofluoric acid to produce sodium fluoride and hydrogen gas.
ANSWER: Single Replacement Reaction: 2 Na + 2 HF  2 NaF + H2

42.   Small chunks of potassium are added to water. It violently reacts to make hydrogen gas and potassium hydroxide.

43.   Calcium metal is added to a solution of hydrochloric acid and produces calcium chloride and hydrogen gas

44.   Lithium metal is burned in air creating lithium oxide.

45.   Manganese(II) nitrate solution is mixed with rubidium hydroxide solution making manganese(II) hydroxide and
rubidium nitrate.

46.   Sodium carbonate solution and hydrochloric acid yield sodium chloride, carbon dioxide and water

47.   Solid magnesium carbonate is strongly heated and breaks down to form magnesium oxide and carbon dioxide.

48.   The hydrocarbon hexane (C6H14) is burned in excess oxygen generating carbon dioxide and water

49.   Sodium hydroxide and hydrochloric acid are mixed and their neutralization forms sodium chloride and water.

50.   Phosphoric acid is heated to produce diphosphorus pentoxide and water.

51.   Aluminum oxide in water makes aluminum hydroxide.

52.   Distilled liquid water is boiled.
Name: KEY                                                                                 Date:Summer 2012
AP Chemistry – BISD

Summer Review Problems – Complete By First Day, Discuss On 2 nd Day

Show all work for the following dimensional analysis problems on a separate sheet of paper and write the correct
answer below.

___67______       1. 6.7 cm = ___mm

___0.058___       2. 58 liters = ___m3

___2419200_       3. 56.000 ft/s = ___in/hr

___140000_____4. 5.0 ft3 = ___cm3 (1in = 2.54cm)

___1.326 X 108__5. 300.0 lb/mL= ___g/dm3 (1 lb = 454 g) – SHOW ANSWER IN SCIENTIFIC NOTATION!

Significant digit problems: Write answers in correct number of significant digits.

____26_____6. 5.67 X 4.6

____16.8___ 7. 3.44 + 5.6 + 7.80

___- 0.0057_ 8. 1.3 X 10-5 - 0.0057 (If the answer bothers you, think about it.)

____4.8____ 9. (2.33 +9.1) / (3.55-1.2)

_0.683 g/cm310. Volume of solid sample: 32.52 cm3
Mass of empty container: 2.5 g
Mass of container plus solid sample: 24.7 g
What is the density of the sample with answer showing correct sig figs?

Physical (P) or Chemical (C) Change. List each as a physical, chemical change, or both.

_____C_____11. Burning wood                           ____BOTH__12. Dissolving salt in water

_____P_____13. Melting ice                            ______C____14. Souring of milk

_____C_____15. Baking soda on an acid spill

Physical (P) or Chemical (C) Properties. List each as a chemical or physical property.

_____P_____16. Color                                  _____C_____17. Sodium reacts with Chlorine

_____P_____18. Density                                _____C_____19. Iron rusts

_____P_____20. Melting point

Tell if the following are homogeneous or heterogeneous

Homogeneous21. Sugar water solution                   Homogeneous 22. Air

Homogeneous 23. Water                                 Homogeneous 24. Milk

Heterogeneous25. Iron and salt
Which of the following are pure substances: answer yes or no. Be prepared to defend your answer.

____Yes____26. Table salt                              ____ Yes ____27. Water

____No_____28. Copper Sulfate solution                 ____Yes _____29. Gold

____No_____30. Air

Show all work on a separate sheet of paper for #31-#41and write the final answer below each question.

31. The mass ratio of iron to oxygen in ferric oxide, Fe 2O3, is __2.33___ to 1.00.

32. How many grams of aluminum nitrate, Al(NO3)3, contain 18.0 grams of oxygen atoms?            26.6 g

33. The simplest formula for a hydrocarbon that is 82.8% carbon is C2H5

34. How many molecules of nitrogen in 3.5 grams of N 2?7.5 X 1022How many atoms of nitrogen?1.5 X 1023

35. How many grams of potassium permanganate contain 27.5 grams of oxygen?              67.9 g

36. How many hydrogen atoms are present in 1.00 mole of acetic acid, CH3COOH?2.41 X 1024 How many would be present
in 28.5 grams of acetic acid?1.14 X 1024

37. 11.17 grams of iron metal is allowed to react with oxygen. At the end of the reaction, the compound formed has a mass of
14.37 grams. What is the formula of the compound formed? FeO

38. How many grams of carbon are present in 0.25 moles of butane, C 4H10? 12 grams (Do NOT use a calculator!)

39. What is the percent of sulfur in H2SO4? 32.7%

40. What is the simplest formula for a compound that is 26.6% potassium, 35.4% chromium, and 38.0% oxygen?K2Cr2O7

41. A 15.0 gram sample of an unknown hydrocarbon is burned in excess oxygen. The combustion forms 48.4 grams of carbon
dioxide and 16.47 grams of water. If the hydrocarbon has a molar mass of 123 g/mole, what is the molecular formula for the
hydrocarbon? C9H15
Directions: State what type of reaction is occurring. Then write and balance the equation.

EXAMPLE: Sodium metal is added to hydrofluoric acid to produce sodium fluoride and hydrogen gas.
ANSWER: Single Replacement Reaction: 2 Na + 2 HF  2 NaF + H2

42.   Small chunks of potassium are added to water. It violently reacts to make hydrogen gas and potassium hydroxide.

Single Replacement: 2 K + 2 H2O  H2 + 2 KOH

43.   Calcium metal is added to a solution of hydrochloric acid and produces calcium chloride and hydrogen gas

Single Replacement: Ca + 2 HCl  CaCl2 + H2

44.   Lithium metal is burned in air creating lithium oxide.

Synthesis/Combustion: 4 Li + O2  2 Li2O

45.   Manganese(II) nitrate solution is mixed with rubidium hydroxide solution making manganese(II) hydroxide and
rubidium nitrate.

Double Replacement: Mn(NO3)2 + 2 RbOH  Mn(OH)2  2 RbNO3

46.   Sodium carbonate solution and hydrochloric acid yield sodium chloride, carbon dioxide and water

Gas Forming Reaction: Na2CO3 + 2 HCl  2 NaCl + CO2 + H2O

47.   Solid magnesium carbonate is strongly heated and breaks down to form magnesium oxide and carbon dioxide.

Decomposition: MgCO3  MgO + CO2

48.   The hydrocarbon hexane (C6H14) is burned in excess oxygen generating carbon dioxide and water

Combustion: 2 C6H14 + 19 O2  12 CO2 + 14 H2O

49.   Sodium hydroxide and hydrochloric acid are mixed and their neutralization forms sodium chloride and water.

Double Replacement/Neutralization: NaOH + HCl  NaCl + H2O

50.   Phosphoric acid is heated to produce diphosphorus pentoxide and water.

Decomposition: 2 H3PO4  P2O5 + 3 H2O

51.   Aluminum oxide in water makes aluminum hydroxide.

Synthesis: Al2O3 + 3 H2O  2 Al(OH)3

52.   Distilled liquid water is boiled.

Vaporization(Phase Change, NOT Chemical Change): H2O(l)  H2O(g)

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