GASES+Free+Response+worksheet - AP Gas Law Free Response Questions 1971 2 HCOONa H2SO4 2 CO 2 H2O Na2SO4 A 0.964 gram sample of a mixture of sodium

GASES+Free+Response+worksheet - AP Gas Law Free Response...

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AP* Gas Law Free Response Questions (1) AP ® is a registered trademark of the College Board. The College Board was not involved in the production of and does not endorse this product. (2) Test Questions are Copyright © 1984-2008 by College Entrance Examination Board, Princeton, NJ. All rights reserved. For face-to-face teaching purposes, classroom teachers are permitted to reproduce the questions. Web or Mass distribution prohibited. C. Calculate the percentage of sodium formate in the original mixture. 1971 At 20°C the vapor pressure of benzene is 75 torr, and the vapor pressure of toluene is 22 torr. Solutions in both parts of this question are to be considered ideal. (a)A solution is prepared from 1.0 mole of biphenyl, a nonvolatile solute, and 49.0 moles of benzene. Calculate the vapor pressure of the solution at 20°C. (b)A second solution is prepared from 3.0 moles of toluene and 1.0 mole of benzene. Determine the vapor pressure of this solution and the mole fraction of benzene in the vapor. 1972 A 5.00 gram sample of a dry mixture of potassium hydroxide, potassium carbonate, and potassium chloride is reacted with 0.100 liter of 2.0 molar HCl solution. (a)A 249 milliliter sample of dry CO2gas, measured at 22°C and 740 torr, is obtained from the reaction. What is the percentage of potassium carbonate in the mixture? (b)The excess HCl is found by titration to be chemically equivalent to 86.6 milliliters of 1.50 molar NaOH. Calculate the percentages of potassium hydroxide and of potassium chloride in the original mixture. 1973 A 6.19 gram sample of PCl5is placed in an evacuated 2.00 liter flask and is completely vaporized at 252°C. (a)Calculate the pressure in the flask if no chemical reaction were to occur. (b)Actually at 252°C the PCl5is partially dissociated according to the following equation: PCl5(g) PCl3(g)+ Cl2(gThe observed pressure is found to be 1.00 atmosphere. In view of this observation, calculate the partial )
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