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Unformatted text preview: Version 094 – Homewrok 3 – Fakhreddine – (53605) 1 This printout should have 26 questions. Multiplechoice questions may continue on the next column or page – find all choices before answering. 001 1.0 points Several interesting observations from the world around you are listed below. Which of these is NOT explained by a colligative property? 1. Antifreeze is added to a car radiator to keep the car from overheating. 2. A lobster will die when placed in fresh water. 3. The freezing point of water is lowered when salt is added. 4. At high altitude it takes longer to cook spaghetti. correct 5. Water boils at a higher temperature when salt is added. Explanation: Colligative properties of a solution depend on the number of solute particles in solution, not the type. Boiling point variations due to pressure changes have nothing to do with solutions and colligative properties (boiling point variations due to particles in solution, etc.). 002 1.0 points The vapor pressure of pure CH 2 Cl 2 (molecu lar weight = 85 g/mol) is 133 torr at 0 ◦ C and the vapor pressure of pure CH 2 Br 2 (molecu lar weight 174 g/mol) is 11 torr at the same temperature. What is the total vapor pres sure of a solution prepared from equal masses of these two substances? 1. vapor pressure = 144 torr 2. vapor pressure = 105 torr 3. vapor pressure = 93 torr correct 4. vapor pressure = 89 torr 5. vapor pressure = 124 torr 6. vapor pressure = 72 torr Explanation: For CH 2 Cl 2 , P = 133 torr MW = 85 g / mol For CH 2 Br 2 , P = 11 torr MW = 174 g / mol This is a combination of Raoult’s Law and Dalton’s Law of Partial Pressures. The an swer does not depend on what the masses are, as long as they are equal. You can choose any mass you like, but to speed up calculations, it is convenient to choose the mass the same as one of the molecular weights given, so that the number of moles for one of the components is exactly ONE. So, for argument’s sake, choose 85 g to be the mass of each of the components. That way you have: (85 g CH 2 Cl 2 ) parenleftbigg 1 mol CH 2 Cl 2 85 g CH 2 Cl 2 parenrightbigg = 1 . 0 mol CH 2 Cl 2 Now calculate the moles of the other compo nent. (85 g CH 2 Br 2 ) parenleftbigg 1 mol CH 2 Br 2 174 g CH 2 Br 2 parenrightbigg = 0 . 49 mol CH 2 Br 2 Once you have the two values for moles you can calculate the mole fraction of each com ponent. n total = 1 . 0 + 0 . 49 = 1 . 49 mol X CH 2 Cl 2 = 1 . 0 mol 1 . 49 mol = 0 . 67 X CH 2 Br 2 = . 49 mol 1 . 49 mol = 0 . 33 Then use those values in Raoult’s Law to get the vapor pressure for each component. Raoult’s Law states that: P A = X A P A P CH 2 Cl 2 = (0 . 67)(133 torr) = 89 torr P CH 2 Br 2 = (0 . 33)(11 torr) = 3 . 6 torr Version 094 – Homewrok 3 – Fakhreddine – (53605) 2 Add the two together to get the total vapor pressure (Dalton’s Law)....
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This note was uploaded on 04/15/2009 for the course CH 53625 taught by Professor Fakhreddine during the Spring '09 term at University of Texas.
 Spring '09
 Fakhreddine
 Chemistry

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