1. 100 200 300 400 500 Final Question Mixtures Solution Vocab.
Conc. Problems
Solubility
Ideal Gases
Gas Laws
Gas Law Problems
Diffusion
Concepts
Misc.
Gas Vocab
100
200
300
400
500
Final Question

2. Mixtures - 100
Silver and gold is an example of which solute-solvent combination?
Answer: solid-solid
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3. Random Points
200 points

4. Mixtures - 200
This can be used to separate liquids that have different densities.
Answer: Centrifuge
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5. Mixtures - 300 Back What does not experience the Tyndall effect?
Answer: Solutions or homogeneous mixtures
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6. Mixtures - 400
Identify whether the following scenario describes a saturated, unsaturated or supersaturated solution.
A single grain of solute is added to the solution, it sinks to the bottom of the container, and nothing else happens.
Answer: Saturated
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7. Mixtures - 500
A student is trying to determine if a liquid is a colloid, solution or suspension. The student cannot see through the mixture and the particles are not settling out. The liquid should be classified as a _______________________.
Answer: Colloid
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8. Vocabulary - 100 Back In a solution, the substance that is dissolved.
Answer: Solute
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9. Vocabulary - 200
A water-soluble cleaner that can emulsify dirt and oil.
Answer: Detergent
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10. Vocabulary - 300
A compound that concentrates at the boundary surface between two immiscible phases (solid-liquid, liquid-liquid, or liquid-gas).
Answer: Surfactant
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11. Daily Double

12. Vocabulary - DD
The law that relates partial pressure of a gas to its solubility is ____________________.
Answer: Henry’s Law
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13. Vocabulary - 500
The random movement of microscopic particles suspended in a fluid is known as:
Answer: Brownian Motion
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14. Concentration Problems - 100
A sample of g of drinking water is found to contain 42 mg Pb. What is this concentration in parts per million?
Answer: 28 ppm
0.042g/1500.0g x
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15. Random Points
300 points

16. Concentration Problems - 200
A solution contains 76.0 g of NaCl and has a volume of 550 mL. Find the molarity of the solution.
Answer: 2.36 M
76.0g x 1 mol/58.5 g = 1.3 mol
550ml/1000 = L
M = mol/L = 1.3/0.550 = 2.36 M
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17. Concentration Problems - 300
You need to make 200 mL of 0.25 M HCl. How much 6.0 M HCl would you need?
Answer: 8.33 mL (use M1V1=M2V2)
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18. Concentration Problems - 400
How many grams of NaOH are required to prepare 1200 mL of a 0.50 M solution?
Answer: 24 g
0.50 = x/1.200 (M=mol/L)
x = 0.6 mol x 40g/1mol = 24 g
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19. Concentration Problems - 500
Legally, the concentration of methyl mercury needs to be less than 1.0 ppm in fish meat to be sold or eaten. What is the maximum amount in milligrams of methyl mercury allowed in a fish that weighs 2.25 kg?
Answer: 2.25 mg
1.0 = x/2250 x
x = g x 1000 = 2.25 mg
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20. Solubility - 100
Describe a condition that has an effect on solubility.
Answer:
Temperature – increases solubility of solids and liquids, decreases solubility of gases,
Agitation – increases solubility of liquids and solids
Surface area – the smaller the surface area, the greater impact on solubility
Polarity – has to be the same polarity to be soluble
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21. Solubility - 200 Back How can the solubility of a gas be increased?
Answer: Increase pressure, decrease temp, decrease agitation
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22. Random Points
200 points

23. Solubility - 300
What chemical has the most change in solubility as the temperature is changed from 0C to 100  C
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Answer: NaC2H3O2 or sodium acetate

24. Solubility - 400
At 10 °C, how much CsCl can be dissolved in 300 g of water?
Answer: about 513 g
171 x 3
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25. Solubilty - 500
At 90C, 30 g of Li2SO4 is dissolved in 100 g of water. Is this solution saturated, unsaturated, or supersaturated?
Answer: Unsaturated, because at 90C, water can hold 31 g of Li2SO4
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26. Ideal Gases - 100
What is the ideal gas law formula?
PV=nRT
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27. Ideal Gases - 200
According to the diagram to the right, at what pressure do all the gases most resemble an ideal gas?
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0 atm

28. Ideal Gases - 300
Calculate the approximate volume of a 2.50 mol sample of gas at -8.0°C and a pressure of 3.50 atm.
15.5 L
PV=nRT
(3.50)V=(2.5)(0.0821)(-8+273)
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29. Ideal Gases - 400
A 10.5 L sample of a gas has a mass of 95.9 g at 7.6 atm and 35°C. What is the molar mass of the gas? (Hint: divide the given mass by n).
30.4 g/mol
PV=nRT
(7.6)(10.5)=n(0.0821)(35+273)
n=3.15, so 95.9/3.15
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30. Daily Double

31. Ideal Gases - DD 2H2O(l) + electricity  2H2(g) + O2(g)
What mass of H2O is needed to create L of O2, if the temperature is 25°C and the pressure is 1.2 atm?
27.6 g
PV=nRT with Stoichiometry
(1.2)(15.64)=n(0.0821)(25+273)
n=0.767 mol x 2molH2O/1molO2 x 18g/1mol
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32. Gas Laws - 100 What happens to the volume of a gas during compression?
The Volume Decreases
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33. Gas Laws - 200
Who developed the concept that the total pressure of a mixture of gases is the sum of their partial pressures?
Dalton
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34. Gas Laws - 300
Charles’s law is the direct relationship between ____________________ and volume.
Temperature
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35. Gas Laws - 400
Who is accredited with the idea that in a reaction, two volumes of hydrogen gas will combine with one volume of oxygen gas to produce two volumes of water vapor?
Gay-Lussac
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36. Gas Laws - 500
The principle that under similar pressures and temperatures, equal volumes of gases contain the same number of molecules is attributed to ________________.
Avogadro
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37. Gas Law Problems - 100 320 mm Hg 800.0 x 0.40 Back
A mixture of gases with a pressure of mm Hg contains 60% nitrogen and 40% oxygen by volume. What is the partial pressure of oxygen in this mixture?
320 mm Hg
800.0 x 0.40
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38. Gas Law Problems - 200
A sample of oxygen occupies 350 mL when the pressure is 5 atm. At constant temperature, what volume does the gas occupy when pressure falls to 3 atm?
583 mL
PTV Chart
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39. Gas Law Problems - 300 T1 = 76 C P1 = 4 atm V1 = 560 mL
PTV Chart
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40. Daily Double

41. Gas Law Problems - DD
Nitrogen reacts with hydrogen to make ammonia [N2 (g) + 3H2 (g) --> 2NH3 (g)]. If one needs to produce 4 L of ammonia, how many liters of nitrogen are needed?
2 L
We needed to multiply the coefficient NH3 by 2, so we multiple N2 by 2 as well
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42. Gas Law Problems - 500
A sample of a gas has a pressure of 2.25 atm, a volume of 650 mL and a temperature of 36°C. What would the volume of the gas be if the pressure is increased to 3.20 atm and the temperature is decreased to 31°C?
449.6 mL
PTV Chart
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43. Random Points
100 points

44. Diffusion Concepts - 100
This is the passage of a gas under pressure through a tiny opening.
Effusion
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45. Diffusion Concepts - 200
The rate of diffusion of a gas depends on the ____________ of the gas.
Molar Mass
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46. Diffusion Concepts - 300
What scientist studied effusion in detail and determined that the rate of effusion is indirectly proportional to the square root of the molar mass of the gas, if pressure and temperature are kept constant.
(Thomas) Graham
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47. Diffusion Concepts - 400
To two decimal places, what will vA/vB be equal to if N2 is considered to be gas A and NO is considered to be gas B.
1.03
va/vb= √(MMb/MMa)
X= √(( )/(14.0x2))
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48. Diffusion Concepts - 500
What is the molar mass of a gas if it diffuses at a rate of 258 m/s while Iodine gas diffuses at 125 m/s at the same temperature?
29.7 g/mol
va/vb= √(MMb/MMa)
258/125= √(126.9x2(for I2)/x)
Square both sides (2.064)2=253.8/x
Cross Multiple and Solve for x
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49. Miscellaneous - 100
The average kinetic energy of random motion is proportional to the temperature in what unit?
Kelvin
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50. Miscellaneous - 200
Standard temperature and pressure for a gas is __________&__________
0°C (or 273 K) and 1 atm.
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51. Random Points
300 points

52. Miscellaneous - 300
What is the SI unit of pressure?
Pascal
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53. Miscellaneous - 400 A pressure of 165 kPa is equal to _____ atm.
(1 atm = Pa)
1.63
165kPa x 1000 = Pa x 1atm/ Pa
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54. Miscellaneous - 500 92 C Back
Line D represents water. If the atmospheric pressure in a flask is lowered to 70 kPa, water would boil at what temperature?
92 C
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55. Vocabulary - 100
What does the constant bombardment of gas molecules against the inside of a container cause?
Pressure
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56. Vocabulary - 200
The movement of particles from regions of higher concentrations to regions of lower concentration.
Diffusion
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57. Random Points
200 points

58. Vocabulary - 300
A device used to measure pressure is called a ____________________.
Barometer
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59. Vocabulary - 400
The pressure of each gas in a mixture is called the ____________________ pressure.
Partial
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60. Kinetic Molecular Theory
Vocabulary - 500
What is the theory that explains that the behavior of physical systems depends on the combined actions of the molecules constituting the system?
Kinetic Molecular Theory
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61. Final Quesion The final Question is on:
A vocabulary word and a question dealing with that term.
Make your wager!

62. Final Questions Answer: Colligative Property and a
(Definition) This is a property that is determined by the number of particles present in a system but that is independent of the properties of the particles themselves.
Which of the following is an example of using the concept of boiling point elevation?
a. Adding table salt in water to cook pasta
b. Adding rock salt on icy roads
c. Adding valve oil to a brass instrument during a Christmas parade to keep the valves from locking up.
d. Adding ethylene glycol (antifreeze) to a car engine during the winter.
Answer: Colligative Property and a