Chemistry I Final Study Guide - PC\|MAC



Chemistry I Final Study Guide

Determine the number of significant figures in the following:

1. 30040

2. 0.663

3. 20.05

4. 1500.

5. 0.0008

Perform the following calculations and express your answer w/ the correct number of significant figures.

6. 47.0 x 2.2

7. 140 x35

8. 7.945 + 82.3 + 0.02

9. 312 – 31.2 – 3.12

Perform the following density calculations:

10. The mass of a 5.00 cm3 sample of clay is 11.0 g. What is the density of the clay?

11. The density of lead is 11.35 g/cm3. What is the mass of a 10.0 cm3 piece of lead?

Identify the following as physical or chemical changes.

12. water boiling 13. sugar dissolving 14. oil burning

15. List the 3 subatomic particles in the atom, their location, charge, and approximate mass.

16. Determine the number of protons, neutrons, and electrons in C-14 and Na+1

17. Differentiate between ions and isotopoes

18. List properties and define three types of radioactive decay.

19. Define and identify uses of fusion and fission.

(Example: What type of reaction fuels a star? What type of reaction is used to produce energy in nuclear power plants?)

Write the superscript notation for the following:

20. C 21. Au 22. Eu

Name the following compounds using the designated system.

23. PI3-binary molecular

24. N2O4- binary molecular

25. Fe(NO3)2-old system

26. CuCO3-stock system

Write the formulas for the following compounds.

27. silicon dioxide 28. barium hydroxide 29. mercuric iodide 30. calcium sulfate

Convert the following:

31. 63.658 g Li to moles 32. 62 grams C to atoms 33. 3.2 mols Cl to atoms 34. 2.2 g Al(OH)3 to mols

Determine the percent composition of the following:

35. Al2O3 36. Ba(OH)2

37. Determine the % composition of water in CaSO4 *2H2O

Calculate the following using the following reaction-be sure to balance the equation.

P + O2 ( P4O10

38. What mass of phosphorous will be needed to produce 3.25 mols of P4O10?

39. If 0.489 mol of phosphorous burns, what mass of oxygen is used? What mass of P4O10 is produced?

Calculate the following using the following reaction-be sure to balance the equation.

CuSO4 + Fe ( Cu + Fe2(SO4)3

40. If you place 0.092 g of Fe in a solution containing 0.158 mol of CuSO4, what is the limiting reactant? How many moles of Cu will be formed?

Calculate the following using the given reaction-be sure to balance.

As2O3 + C ( CO2 + As

41. If 8.87 g of As2O3 is used in the reaction and 5.33 g of As is produced, calculate the percent yield.

Calculate the following gas law problems.

42. 2.2 L of hydrogen at 6.5 atm pressure is used to fill a balloon at a final pressure of 1.15 atm. What is the final volume?

43. A cylinder of gas has a pressure of 4.4 atm at 25 (C. At what temp. in (C will it reach a pressure of 6.5 atm?

44. A sample of hydrogen gas has a volume of 65 mL at a pressure of 0.922 atm and a temperature of 16 (C. What volume will it occupy at STP?

45. A student collects 425 mL of oxygen at a temperature of 24 ºC and a pressure of 0.899 atm. How many moles of oxygen did the student collect?

46. Use the following reaction to calculate the mass of BaO2 reacted if 265 mL of O2 is collected at 0.975 atm and 10( C? Be sure to balance the reaction.

BaO2 ( BaO + O2

47. If the following reaction occurs at STP, what mass of KlCO3 must be used to generate 5 L of O2? Be sure to balance the reaction.

KClO3 ( KCl + O2

48. What volume of water would you add to 15.0 mL of a 6.77 M solution of nitric acid in order to get a 1.5 M solution?

49. How many moles of sulfuric acid are in 2.5 L of a 4.25 M solution?

50. A 50.0 mL sample of sodium hydroxide solution is titrated with a 1.605 M solution of sulfuric acid. The titration requires 24.09 mL of the acid solution to reach the equivalence point. What is the molarity of the base solution?

H2SO4 + NaOH ( Na2SO4 + H2O

51. List factors that affect the rate of dissolving a solid and a liquid and a gas in a liquid.

52. Find the atomic mass, atomic number, number of protons, number of electrons, number of neutrons for

i. C-14

ii. Ag

53. List properties of metals , nonmetals, and metalloids.

54. In the following reaction, identify the products and reactants.

NaCl + Ba(OH)2 ( NaOH + BaCl2

55. Be able to read a phase diagram (see p. 347 in your text and answer the following)

a. At what temperature and pressure would the substance be at its triple point?

b. At standard pressure, at what temperature would the substance change from a liquid to a gas?

56. Be able to predict the products of a reaction using your Rules of Reactions

. a. What products form when Ba(ClO3)2 decomposes?

b. What are the products when the hydrocarbon CH4 undergoes complete combustion?

c. What are the products when Ca(NO3)2 reacts with AgCl?

57. Be able to identify a reaction as a synthesis, decomposition, combustion, double or single replacement reaction.

58. Know the colors of the visible spectrum in order of increasing energy. Be able to compare frequency, wavelength, and energy. For instance, which has the higher frequency, red or blue light?

59. Know properties of light

60. Use activity series to predict if reactions will occur.

61. Solve specific heat problems. Work practice problem 1 on p. 534 in your text.

62. Know the difference between endothermic and exothermic reactions.

63. Know how adding a solute to a solvent will affect freezing point, boiling point, and vapor pressure. (colligative properties)

64. How many carbon atoms are in Al2(CO3)3?

65. Convert 6 g of S to atoms.

66. An element represented by the symbol X forms a compound with the formula X2Y3. X could be which of the following elements ( Mg, P, Al, or Cl)

67. Understand how pressure, volume, temperature and moles of a gas are related.

a. If pressure increases what will happen to volume?

b. If temperature increases what will happen to pressure?

c. If the mols of gas decreases what will happen to pressure?

68. Explain how a catalyst is able to speed up a chemical reaction.

69. Describe the following separation techniques: filtration, distillation, and crystallization

70. What is the pH of a 1.0 x 10-5 HCl solution?

71. Determine the molecular formula for a compound that has a molecular mass of 28 g/mol and an empirical formula of CH2.

72. Explain the production of light that occurs when electrons gain additional energy.

73. The half-life of cobalt-60 is 5.27 years. How many mg of cobalt-60 remain after 52.7 years if you start with 10.0 mg?

74. Use the solubility chart on p. 414 in your text to answer the following:

a. Which substances solubility is least affected by in increase in temperature?

b. About how many grams of RbCl will dissolve in 100 g of water at 30 degrees Celsius?

c. Which substance is most soluble at 40 degrees Celsius?

75. Which piece of lab equipment would give the most accurate volume: a beaker, graduated cylinder, buret, digital balance, or a thermometer?

76. When liquid water is turned into a gas, the process is endothermic or exothermic?

77. Define Le Chatelier’s principle. If a mixture of water and ice at 0 degrees Celsius gains a quantity of heat, what change would occur?

Chemistry I Final Study Guide KEY

Determine the number of significant figures in the following:

1. 30040 4

2. 0.663 3

3. 20.05 4

4. 1500. 4

5. 0.0008 1

Perform the following calculations and express your answer w/ the correct number of significant figures.

6. 47.0 x 2.2 1.0 x 102

7. 140 x35 4900

8. 7.945 + 82.3 + 0.02 90.3

9. 312 – 31.2 – 3.12 278

Perform the following density calculations:

10. The mass of a 5.00 cm3 sample of clay is 11.0 g. What is the density of the clay? 2.20 g/cm3

11. The density of lead is 11.35 g/cm3. What is the mass of a 10.0 cm3 piece of lead? 114 g

Identify the following as physical or chemical changes.

12. water boiling 13. sugar dissolving 14. oil burning

Physical physical chemical

15. List the 3 subatomic particles in the atom, their location, charge, and approximate mass.

16. Determine the number of protons, neutrons, and electrons in C-14 and Na+1

C-14 6 protons, 8 neutrons, 6 electrons

Na+1 11 protons, 12 neutrons, 10 electrons

17. Differentiate between ions and isotopoes

Ions are atoms that have gained or lost electrons. Isotopes are atoms of the same element that have different numbers of neutrons

18. List properties and define three types of radioactive decay.

19. Define and identify uses of fusion and fission.

(Example: What type of reaction fuels a star? What type of reaction is used to produce energy in nuclear power plants?)

Fusion is when two nuclei are squeezed together to form one nucleus, for example two hydrogen atoms are fused into one helium atom. This gives off a great deal of heat and is the process the sun uses.

Fission is when a large nucleus is split into smaller nuclei. An example is Uranium being broken down into smaller nuclei. This is the process that nuclear power plants use to release energy and make electricity.

Write the superscript notation for the following:

20. C 1s2 2s2 2p2

21. Au 1s2 2s2 2p63s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d9

22. Eu 1s2 2s2 2p63s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f7

Name the following compounds using the designated system.

23. PI3-binary molecular phosphorus triiodide

24. N2O4- binary molecular dinitrogen tetroxide

25. Fe(NO3)2-old system ferrous nitrate

26. CuCO3-stock system copper (II) carbonate

Write the formulas for the following compounds.

27. silicon dioxide 28. barium hydroxide 29. mercuric iodide 30. calcium sulfate

SiO2 Ba(OH)2 HgI2 CaSO4

Convert the following:

31. 63.658 g Li to moles 32. 62 grams C to atoms 33. 3.2 mols Cl to atoms 34. 2.2 g Al(OH)3 to mols

9.17 moles 3.1x1024 1.9x1024 0.029 moles

Determine the percent composition of the following:

35. Al2O3 36. Ba(OH)2

Al- 53%, O- 47% Ba- 80.1%, O- 18.7%, H- 1.2%

37. Determine the % composition of water in CaSO4 *2H2O

20.9%

Calculate the following using the following reaction-be sure to balance the equation.

4P + 5O2 ( P4O10

38. What mass of phosphorous will be needed to produce 3.25 mols of P4O10? 402.61g P

39 If 0.489 mol of phosphorous burns, what mass of oxygen is used? What mass of P4O10 is produced?

19.5g O2, 34.70 g P4O10

Calculate the following using the following reaction-be sure to balance the equation.

3CuSO4 + 2Fe ( 3Cu + Fe2(SO4)3

40. If you place 0.092 g of Fe in a solution containing 0.158 mol of CuSO4, what is the limiting reactant? How many moles of Cu will be formed?

Fe, 2.47x10-3 or 0.00247moles Cu

Calculate the following using the given reaction-be sure to balance.

2As2O3 + 3C ( 3CO2 + 4As

41. If 8.87 g of As2O3 is used in the reaction and 5.33 g of As is produced, calculate the percent yield.

6.72 g is the expected yield so the percent yield is 79.3%

Calculate the following gas law problems.

42. 2.2 L of hydrogen at 6.5 atm pressure is used to fill a balloon at a final pressure of 1.15 atm. What is the final volume? 12L

43. A cylinder of gas has a pressure of 4.4 atm at 25 (C. At what temp. in (C will it reach a pressure of 6.5 atm?

167C

44. A sample of hydrogen gas has a volume of 65 mL at a pressure of 0.922 atm and a temperature of 16 (C. What volume will it occupy at STP? 57 mL

45. A student collects 425 mL of oxygen at a temperature of 24 ºC and a pressure of 0.899 atm. How many moles of oxygen did the student collect?

0.016 mol O2

46. Use the following reaction to calculate the mass of BaO2 reacted if 265 mL of O2 is collected at 0.975 atm and 10( C? Be sure to balance the reaction. 3.7g

2BaO2 ( 2BaO + O2

47. If the following reaction occurs at STP, what mass of KClO3 must be used to generate 5 L of O2? Be sure to balance the reaction.

2KClO3 ( 2KCl + 3O2

18.3 g KClO3

48. What volume of a 1.5 M solution would you add to 15.0 mL of a 6.77 M solution of nitric acid in order to get a 1.5 M solution? 52.7 mL

49. How many moles of sulfuric acid are in 2.5 L of a 4.25 M solution? 10.6 mol

50. A 50.0 mL sample of sodium hydroxide solution is titrated with a 1.605 M solution of sulfuric acid. The titration requires 24.09 mL of the acid solution to reach the equivalence point. What is the molarity of the base solution?

H2SO4 + 2NaOH ( Na2SO4 + 2H2O 1.55 M NaOH

51. List factors that affect the rate of dissolving a solid and a liquid and a gas in a liquid. Temperature, Surface Area, Agitation

52. Find the atomic mass, atomic number, number of protons, number of electrons, number of neutrons for

i. C-14 14 amu, 6, 6, 6, 8

ii. Ag 107.87amu, 47, 47, 47, not enough info to give # of neutrons

53. List properties of metals , nonmetals, and metalloids.

54. In the following reaction, identify the products and reactants.

NaCl + Ba(OH)2 ( NaOH + BaCl2

reactants products

55. Be able to read a phase diagram (see p. 347 in your text and answer the following)

a. At what temperature and pressure would the substance be at its triple point? .0060 atm + .01°C

b. At standard pressure, at what temperature would the substance change from a liquid to a gas? 100°C

56. Be able to predict the products of a reaction using your Rules of Reactions

a. What products form when Ba(ClO3)2 decomposes? BaCl2 + O2

b. What are the products when the hydrocarbon CH4 undergoes complete combustion? CO2 + H2O

c. What are the products when Ca(NO3)2 reacts with AgCl? CaCl2 + 2AgNO3

57. Be able to identify a reaction as a synthesis, decomposition, combustion, double or single replacement reaction.

58. Know the colors of the visible spectrum in order of increasing energy. Be able to compare frequency, wavelength, and energy. For instance, which has the higher frequency, red or blue light? Blue

59. Know properties of light

60. Use activity series to predict if reactions will occur.

61. Solve specific heat problems. Work practice problem 1 on p. 534 in your text. 0.14 J/gxK

62. Know the difference between endothermic and exothermic reactions. Endothermic reactions absorb energy and get colder, exothermic reactions release energy and get hotter.

63. Know how adding a solute to a solvent will affect freezing point, boiling point, and vapor pressure. (colligative properties) Decrease freezing point, increase boiling point and decrease vapor pressure.

64. How many carbon atoms are in Al2(CO3)3? 3

65. Convert 6 g of S to atoms. 1.13 x 1023

66. An element represented by the symbol X forms a compound with the formula X2Y3. X could be which of the following elements ( Mg, P, Al, or Cl)

67. Understand how pressure, volume, temperature and moles of a gas are related.

a. If pressure increases what will happen to volume? decrease

b. If temperature increases what will happen to pressure? increase

c. If the mols of gas decreases what will happen to pressure? decrease

68. Explain how a catalyst is able to speed up a chemical reaction. A catalyst decreases the amount of activation energy so it is easier for the molecules to react.

69. Describe the following separation techniques: filtration, distillation, and crystallization

70. What is the pH of a 1.0 x 10-5 HCl solution? 5

71. Determine the molecular formula for a compound that has a molecular mass of 28 g/mol and an empirical formula of CH2. C2H4

72.Explain the production of light that occurs when electrons gain additional energy.

73. The half-life of cobalt-60 is 5.27 years. How many mg of cobalt-60 remain after 52.7 years if you start with 10.0 mg? 0.0098 g

74. Use the solubility chart on p. 414 in your text to answer the following:

a. Which substances solubility is least affected by in increase in temperature? Li2SO4

b. About how many grams of RbCl will dissolve in 100 g of water at 30 degrees Celsius? 100g

c. Which substance is most soluble at 40 degrees Celsius? RbCl

75. Which piece of lab equipment would give the most accurate volume: a beaker, graduated cylinder, buret, digital balance, or a thermometer?

76. When liquid water is turned into a gas, the process is endothermic or exothermic? endothermic

77. Define Le Chatelier’s principle. If a mixture of water and ice at 0 degrees Celsius gains a quantity of heat, what change would occur? Some of the ice would melt into water but the temperature would stay the same.

................
................

In order to avoid copyright disputes, this page is only a partial summary.

Google Online Preview   Download