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Final Question

Final Question. Mixtures - 100. Silver and gold is an example of which solute-solvent combination?. Answer: solid-solid. Back. Random Points. 200 points. Mixtures - 200. This can be used to separate liquids that have different densities. Answer: Centrifuge. Back. Mixtures - 300.

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Final Question

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  1. Final Question

  2. Mixtures - 100 • Silver and gold is an example of which solute-solvent combination? Answer: solid-solid Back

  3. Random Points 200 points

  4. Mixtures - 200 • This can be used to separate liquids that have different densities. Answer: Centrifuge Back

  5. Mixtures - 300 • What does not experience the Tyndall effect? Answer: Solutions or homogeneous mixtures Back

  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 Back

  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 Back

  8. Vocabulary - 100 • In a solution, the substance that is dissolved. Answer: Solute Back

  9. Vocabulary - 200 • A water-soluble cleaner that can emulsify dirt and oil. Answer: Detergent Back

  10. Vocabulary - 300 • A compound that concentrates at the boundary surface between two immiscible phases (solid-liquid, liquid-liquid, or liquid-gas). Answer: Surfactant Back

  11. Daily Double

  12. Vocabulary - DD • The law that relates partial pressure of a gas to its solubility is ____________________. Answer: Henry’s Law Back

  13. Vocabulary - 500 • The random movement of microscopic particles suspended in a fluid is known as: Answer: Brownian Motion Back

  14. Concentration Problems - 100 • A sample of 1500.0 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 1000000 Back

  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 = 0.550 L M = mol/L = 1.3/0.550 = 2.36 M Back

  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) Back

  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 Back

  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 1000000 x = 0.00225 g x 1000 = 2.25 mg Back

  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 Back

  21. Solubility - 200 • How can the solubility of a gas be increased? Answer: Increase pressure, decrease temp, decrease agitation Back

  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 Back 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 Back

  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 Back

  26. Ideal Gases - 100 What is the ideal gas law formula? PV=nRT Back

  27. Ideal Gases - 200 According to the diagram to the right, at what pressure do all the gases most resemble an ideal gas? Back 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) Back

  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 Back

  30. Daily Double

  31. Ideal Gases - DD 2H2O(l) + electricity  2H2(g) + O2(g) What mass of H2O is needed to create 15.64 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 Back

  32. Gas Laws - 100 What happens to the volume of a gas during compression? The Volume Decreases Back

  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 Back

  34. Gas Laws - 300 Charles’s law is the direct relationship between ____________________ and volume. Temperature Back

  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 Back

  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 Back

  37. Gas Law Problems - 100 A mixture of gases with a pressure of 800.0 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 Back

  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 Back

  39. Gas Law Problems - 300 T1 = 76 C P1 = 4 atm V1 = 560 mL T2 = 92 C P2 = 2 atm V2 = ? 1171 mL PTV Chart Back

  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 Back

  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 Back

  43. Random Points 100 points

  44. Diffusion Concepts - 100 This is the passage of a gas under pressure through a tiny opening. Effusion Back

  45. Diffusion Concepts - 200 The rate of diffusion of a gas depends on the ____________ of the gas. Molar Mass Back

  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 Back

  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= √((14.0+16.0)/(14.0x2)) Back

  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? 59.6 g/mol va/vb= √(MMb/MMa) 258/125= √(126.9x2(for I2)/x) Square both sides (2.064)2=253.8/x Solve for x Back

  49. Miscellaneous - 100 The average kinetic energy of random motion is proportional to the temperature in what unit? Kelvin Back

  50. Miscellaneous - 200 Standard temperature and pressure for a gas is __________&__________ 0°C (or 273 K) and 1 atm. Back

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