Matter and Energy (Due by Friday, Jan 20th) Name______________________________Chemistry

Matter

1. For each of the following, check the one box that applies.

Physical Property

Physical Change

Chemical Property

Chemical Change

a pond freezes overa puddle dries up

alcohol evaporatingblue color

boiling pointburning paperbutter melting

can neutralize a basecracking an egg

cutting paperdensity

digestion of fooddissolving sugar in water

flammabilityglass breaking

hardnessiron rusting

is reactive with waterleaves changing color

lighting a matchluster

magnetizing a nailmelting glassmelting point

mowing the lawnodor

paint fadingsolubilitysour taste

stretching a rubber bandsupports combustion

water boilingwill form H2 when mixed with acid

wood rottingClassification

22. Match each of the following statements with one or more of the following forms of matter.

E – Element C – Compound S – Solution M - Mixture (heterogeneous)

_____ soil _____ CH3OCH3 _____ perfume

_____ nitrogen gas (N2) _____ air _____ Jello

_____ tin _____ carbon dioxide _____ pizza

_____ helium _____ hot chocolate _____ oxygen (O2)

_____ salt _____ baking soda (NaHCO3) _____ mercury

_____ tap water _____ distilled water _____ gold ring

_____ diamond _____ sand (SiO2) _____ liquid dish detergent

_____ calcium _____ steam _____ smog

_____ Italian salad dressing _____ hot chocolate+marshmallows _____ brass

Elements3. Write the correct chemical symbol for each of the following elements.

hydrogen tungsten mercury oxygen

helium manganese boron sulfur

lithium iron aluminum fluorine

sodium nickel carbon chlorine

potassium palladium silicon bromine

beryllium platinum tin iodine

magnesium copper lead neon

calcium silver nitrogen argon

strontium gold phosphorus krypton

barium zinc arsenic xenon

chromium cadmium antimony radon

3Compounds

4. Complete the following table

FORMULA # FUNDAMENTAL PARTICLES # INDIVIDUAL ATOMS # TOTAL ATOMS

a) 2NaHCO3 2 Na: 2 H: 2 C: 2 O: 6 12

b) 3H3PO4

c) (NH4)3PO4

d) 4CaCO3

e) 2Al2O3

f) 3Ba(OH)2

g) CH3CH2OH

h) 4Ca(ClO3)2

i) Al2(SO4)3

j) 3(NH4)2SO4

4Mixture Separation

5. Complete the following sentences using the correct separation technique term.

filtration crystallization chromatography distillation

a. Heterogeneous mixtures are often separated by __________________________.

b. Separating sand from water can be done by ___________________________.

c. The sugar in sugar water can be removed by ___________________________.

d. The technique that takes advantage of different boiling points is __________________.

e. Removing chlorophyll pigment from leaves might be done by ______________________.

f. Crude oil is broken down by heat, vaporized, and allowed to condense into various liquids

such as gasoline. This process is called __________________________.

6. How could you separate a mixture of iron filings and aluminum filings? What property of these metals would allow such a separation?

7. How could you separate a mixture of alcohol, water, oil, and sand?

8. Explain what it means to say that a mixture of substances can be separated by physical means. Give an example.

9. Explain what it means to say that a substance can be separated by chemical means. Give an example.

510. A liquid sample of unknown composition arrives in your laboratory. Although the sample appears

uniform throughout, you have been told that it is a mixture of at least two different liquids. You set up the distillation apparatus pictured below to separate the sample.

a. You notice that your sample begins to boil at 96.2°C and liquid begins to drip into the

collection flask. What is happening?

b. Why is it a good idea to remove the collection flask and replace it with another as soon as the temperature of the solution begins to rise again?

c. The temperature rises steadily and the solution begins to boil again at 102.3°C. What is happening now?

d. The temperature again rises until it reaches 108°C and the rest of the solution boils. How many different liquids were contained in your sample? Explain.

e. As you complete the distillation, you notice a white, crystalline film lining the inside of the flask that contained the original sample. What could this substance be? Why didn’t you notice it in the original solution?

6Percent Concentration of Solutions

11. A 197.5 g sample of a solution is found to contain 61.5 g of sodium nitrate. Calculate the percent concentration of this solution.

12. Determine the percent concentration of a solution containing 25.0 g of table salt dissolved in 137 g of water.

13. How many grams of water must be added to 65.5 g of glucose to make a 14.5 % solution?

14. What is the mass of water in a 23.5 % solution containing 15.9 g of potassium chlorate?

15. A student attempts to experimentally determine the percent concentration of an aqueous solution by boiling off the water of a sample of the solution in an evaporating dish. Given the data below, calculate the concentration of the solution.

Mass of empty evaporating dish 42.983 gMass of evaporating dish and solution 58.841 gMass of evaporating dish and dry residue 52.139 g

7Solubility

Use the solubility curves above to answer the following questions:

a. Which salt is least soluble at 20°C?

b. How many grams of potassium chloride (KCl) can be dissolved in 200g of water at 80°C?

c. At 40°C, how much potassium nitrate (KNO3) can be dissolved in 300 g of water?

d. Which salt shows the least change in solubility?

e. A solution at 30°C contains 90g of sodium nitrate (NaNO3) in 100g of water. Is this solution saturated, unsaturated, or supersaturated?

f. How many grams of potassium chlorate (KClO3) will crystallize when a saturated solution is cooled from 80°C to 50°C?

g. How many grams of potassium chlorate (KClO3) are needed to saturate 10 g of water at 30°C?

h. Describe what will happen to an ammonia (NH3) solution as it is slowly heated.

8i. Describe what will happen when 80g of potassium nitrate (KNO3) is added to 100g of

water at 40°C and stirred.

j. A solution containing 20g of ammonium chloride (NH4Cl) dissolved in 50g of water at 100°C is slowly cooled. At what temperature will the solution begin to crystallize?

k. List 2 chemicals from the graph that would be more soluble at higher pressures.

l. List 2 chemicals from the graph whose solubility is unaffected by pressure.

m. Describe what would happen to a small crystal of the solute that is added to a solution of that solute that is:

i. Saturated –

ii. Unsaturated –

iii. Supersaturated –

9Energy Concepts

16. _________________ is the capacity to do work or cause change. .

17. Sunlight is an example of _________________ energy.

18. The gasoline in your car is an example of ___________________ energy.

19. The SI unit for energy is the _____________.

20. The Law of Conservation of Energy states that in any process, energy is neither

________________ nor ___________________.

21. ____________________energy is the energy of motion.

22. Match the energy-requiring process with the correct energy transformation it involves.

______ burning gas to drive a car a. electrical to mechanical______ friction b. light to chemical______ photosynthesis c. mechanical to heat______ electric mixer d. chemical to electrical to light______ steam turbine making electricity e. thermal to mechanical to electrical______ flashlight f. chemical to thermal to mechanical

23. If a process is endothermic, then:

a. Energy is ___________________________________.

b. The system has __________________ energy at the end of the process.

c. The temperature of the surroundings will ___________________________.

24. If a process is exothermic, then:

a. Energy is ___________________________________.

b. The system has __________________ energy at the end of the process.

c. The temperature of the surroundings will ___________________________.

10Phase Changes

25. Answer the following questions using the heating curve above.

a. Does the temperature increase during melting? __________________________

b. Is energy required for both melting and boiling? __________________________

c. What state(s) of matter is(are) present at region A? __________________________

d. What state(s) of matter is(are) present at region D? __________________________

e. Is condensation endothermic or exothermic? __________________________

f. Is melting endothermic or exothermic? __________________________

g. How would you describe the change in arrangement of particles as heat energy and temperature increase region A to region E.

h. What is the name given to the temperature at region D? __________________________

i. What happens to the density of water as it moves from point A to point C? _____________

j. What happens to the density of water as it moves from point C to point E? _____________

k. Describe the change in the motion of particles from regions A to E.

26. Explain the roles of intermolecular forces and kinetic energy in the states of matter and in phase changes.

SOLID

LIQUID

VAPOR

MELTING

FREEZING

BOILING

CONDENSATION

A

B

C

D

E

1127. How much heat (in kJ) is required to melt a 10.0 g ice cube at:

a. 0°C?

b. −15°C?

28. How many calories of heat are required to melt 157 g of gold at its melting point?

29. Aluminum has a melting point of 660.4˚C. How much heat is required to melt a 10.0 kg block of aluminum at 77.0˚C?

30. Benzene, C6H6, boils at 80.1˚C and has a density of 0.877 g/cm3. Determine the quantity of heat, in kilocalories, that are required to boil a 64.3 mL sample of benzene at 25.0˚C.

31. Determine the amount of heat (in kJ) required to convert 50.5 g of ice at 0°C to steam at 100°C.

1232. How many grams of ice at 0°C can be melted by the condensation of 12.39 g of steam at 100°C,

assuming a complete transfer of thermal energy?

33. How much heat is required to convert 31.5 g of H2O from 45.0°C to 145.0°C?

34. How many grams of iron at its melting point can be melted by the addition of 39.5 kJ of heat?

35. A jet of steam at 100°C is applied to a 2.00 kg block of titanium at its melting point. How many grams of steam would be required to completely melt the titanium assuming a complete transfer of thermal energy?

Gas Laws

36. What happens to the volume of a gas if:

a. the pressure is doubled? _____________________________

b. the pressure is quartered? _____________________________

37. What happens to the pressure exerted on a gas if:

a. the volume is halved? _____________________________

b. the volume is tripled? _____________________________

1338. What happens to the volume of a gas if:

a. the temperature is doubled? _____________________________

b. the temperature is quartered? _____________________________

39. What happens to the temperature of a gas if:

a. the volume is halved? _____________________________

b. the volume is tripled? _____________________________

40. What happens to the pressure of a gas if the temperature:

a. is quadrupled? ______________________

b. is halved? ______________________

41. What happens to the volume of a gas if:

a. the pressure is halved and the temperature is doubled? ______________________

b. the temperature is halved and the pressure is doubled? ______________________

c. both the temperature and pressure are tripled? ______________________

42. The volume of a helium balloon is 2.9 L at 91.2 kPa. Determine the volume at standard pressure. P1 = P2 =

V1 = V2 =

43. A gas occupies of volume of 29.5 mL at 25°C. If the pressure remains constant, determine the volume of the gas if the temperature is increased to 57°C.

V1 = V2 =T1 = T2 =

1444. A sample of carbon dioxide has a volume of 2.88 L at 73°C and 655 torr. Determine the volume

of this gas at STP.P1 = P2 =V1 = V2 =T1 = T2 =

45. A gas with a pressure of 1560 torr at 198.0°C is cooled to −16.3°C. Calculate the new pressure.

46. What is the pressure on a sulfur dioxide sample with a volume of 346 mL if it occupies a volume of 0.790 L at 125 kPa?

47. A gas has a volume of 41.3 mL at 19°C. What temperature would this gas have at 0.121 L?

48. What is the volume of a gas at STP if it occupies of volume of 14.9 L at –16.8°C and 136 kPa?

1549. The pressure of a gas at 55°C is increased from 169.2 kPa to 3.65 atm. What will its Celsius

temperature become?

50. What is the Celsius temperature of 68.2 mL of methane, if it occupies a volume of 0.0220 L at 50.0°C?

51. A sample of ammonia gas has a volume of 592 mL at 119°C and 3.71 atm. What is the Celsius temperature if the pressure of the gas is changed to 232 kPa and its volume becomes 1.10 L?

52. A rigid container has 25.0 g of steam at 100.°C that is exerting a pressure of 93.5 kPa on the walls of the container. If 857 J of heat are added to the container, what pressure will the steam exert?

53. A piston contains 37.9 g of steam. The piston is able to expand and contract to maintain a constant pressure. If the steam occupies a volume of 455 mL at 100.°C, what will the volume be after the addition of 549 cal of thermal energy?

16Dalton’s Law of Partial Pressures

54. The total pressure of a mixture of helium, neon, and hydrogen is 498 mm Hg. If the partial pressures of helium and neon are 168 mm Hg and 192 mm Hg respectively, what is the partial pressure of hydrogen?

55. A gas is collected over water at 20.0°C in a eudiometer tube until the pressure is equilibrated with the atmospheric pressure. What is the pressure of the dry gas if the barometric pressure is 771torr?

56. A gas is collected over water in a eudiometer tube until the pressure is equilibrated with the

atmospheric pressure. The volume of gas in the eudiometer is 32.9 mL. The temperature of the water is 40.0°C and the barometric pressure is 754.0 mm Hg. What is the volume of this gas at STP?

57. A gas is collected over water in a eudiometer tube until the pressure is equilibrated with the atmospheric pressure. The volume of gas in the eudiometer is 25.3 mL. The temperature of the water is 50.0°C and the barometric pressure is 760.0 mm Hg. If the pressure remains constant, what will the volume of the gas be at 75.0 °C?

1758. Refer to the diagram below. If the valves were both opened and all three gases were allowed to

diffuse and mix equally, what would the total pressure be?

Review

59. List five properties that would be considered physical properties.

60. List three properties that would be considered chemical properties.

61. Indicate if the following changes are chemical or physical in nature.a. Knocking down bowling pinsb. Chopping a logc. Burning a logd. Frying an egge. Water boilingf. Dissolving sugar into waterg. Combining vinegar and baking sodah. A precipitate is formedi. A liquid freezesj. A gas is produced in a reaction

1862. Complete the following chart.

63. Which of the following will have a higher solubility? (Use graph on page 7 as a reference)

a. Sugar and water at 50°C or at 25°C?

b. Carbon dioxide and water at 50°C or 25°C?

c. Sugar and water at 1.5 atm or 2.5 atm?

d. Carbon dioxide and water at 1.5 atm or 2.5 atm?

64. Why does a sugar cube dissolve more slowly than granulated sugar?

65. When a crystal of a solid solute is added to a solution containing that solute, the solution begins to crystallize. What kind of solution was it before it crystallized? What kind of solution was it after it crystallized?

66. Explain the difference between separating the components of a mixture and separating the components of a compound. Give one concrete example of each.

67. What is the primary difference between a mixture and a solution? What do they have in common?

68. What is the primary difference between an element and a compound? What do they have in common?

Homogeneous or Heterogeneous

Element, Compound, Mixture, Solution

salt water

iron

salt

magnesium bromide

chocolate chip cookie

ocean water

carbon dioxide

manganese

paint

snickers bar

1969. Given: 4 (NH4)3PO4

a. How many formula units are present? __________

b. How many nitrogen atoms? __________

c. How many hydrogen atoms? __________

d. How many phosphorus atoms? __________

e. How many oxygen atoms? __________

f. How many total atoms? __________

70. Use the given heating curve to answer the questions below

Heating Curve for Iron

0

500

1000

1500

2000

2500

3000

3500

4000

0 2 4 6 8 10 12

Time (minutes)

Tem

pera

ture

(o C)

a. What is the melting point for iron? ______________

b. What is the freezing point for iron? ______________

c. What is the boiling point for iron? ______________

d. What is the condensation point for iron? ______________

e. What phase is iron at room temperature? ______________

f. What phase is iron at 1000°C? ______________

g. What phase is iron at 2000°C? ______________

h. What phase is iron at 3000°C? ______________

i. What happens to the temperature of iron during melting? ___________________________

2071. List the names of the 6 phase changes and indicate if they are endothermic or exothermic.

72. How many calories of heat are required to change 35.0 g H2O at −7.0°C to 90.0°C?

73. Determine the volume of a gas at 25.0 atm if it has a volume of 2.30 L at 1025 mmHg.

74. The volume of a gas is 12.54 mL at 455 torr. What pressure is required to change the volume to 0.750 L?

75. A mixture carbon dioxide and carbon monoxide has a total pressure of 0.659 atm. If the carbon dioxide has a partial pressure that is twice that of carbon monoxide, determine the partial pressure of each gas in torr.

76. A gas is collected by water displacement at 23°C and the pressure is equilibrated with the air. The eudiometer reads 45.0 mL and the barometer reads 72.3 cm Hg. Convert to STP.

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77. A balloon is filled to a volume of 758 mL with 169 grams of steam at 125.0°C. After a brief period of cooling, the balloon’s volume is measured to be 745 mL. How much heat energy did the steam lose?

Cumulative Questions

78. The density of copper was experimentally determined to be 8.52 g/mL. The accepted density of copper is 8.92 g/mL. What is the percent error?

79. What is the density of a 55.5 g object, in g/L, if the dimensions of the object are as follows: 5.4 cm x 1.2 cm x 3.8 cm?

80. Convert the following measurements to the specified unit:

a. 2.55 nL = ____________________________ daL

b. 340 cg = ____________________________ μg

81. Convert 35.98 kilograms into pounds and express the answer in scientific notation.

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82. A block occupies 0.2587 ft3. What is its volume in mm3?

83. If a car is traveling at 55 mph, what is its speed in nm per second?

84. A 28.9 grams sample of silicon dioxide was heated from 22.4°C to 65.0°C. How much heat energy was absorbed by the silicon dioxide in this process?