{"id":274,"date":"2017-12-14T21:31:20","date_gmt":"2017-12-14T21:31:20","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/chapter\/end-of-chapter-material-5\/"},"modified":"2017-12-14T21:31:20","modified_gmt":"2017-12-14T21:31:20","slug":"end-of-chapter-material-5","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-introductory-chemistry\/chapter\/end-of-chapter-material-5\/","title":{"raw":"End-of-Chapter Material","rendered":"End-of-Chapter Material"},"content":{"raw":"
\n

Additional Exercises<\/h3>\n
  1. What is the pressure in pascals if a force of 4.88 kN is pressed against an area of 235 cm2<\/sup>?<\/li>\n\t
  2. What is the pressure in pascals if a force of 3.44 \u00d7104<\/sup>\u00a0MN is pressed against an area of 1.09 k<\/span>m<\/span>2<\/sup>?<\/span><\/li>\n\t
  3. What is the final temperature of a gas whose initial conditions are 667 mL, 822 torr, and 67\u00b0C, and whose final volume and pressure are 1.334 L and 2.98 atm, respectively? Assume the amount remains constant.<\/li>\n\t
  4. What is the final pressure of a gas whose initial conditions are 1.407 L, 2.06 atm, and \u221267\u00b0C, and whose final volume and temperature are 608 mL and 449 K, respectively? Assume the amount remains constant.<\/li>\n\t
  5. Propose a combined gas law that relates volume, pressure, and amount at constant temperature.<\/li>\n\t
  6. Propose a combined gas law that relates amount, pressure, and temperature at constant volume.<\/li>\n\t
  7. A sample of 6.022 \u00d710<\/span>23<\/sup>\u00a0particles of gas has a volume of 22.4 L at 0\u00b0C and a pressure of 1.000 atm. Although it may seem silly to contemplate, what volume would one\u00a0particle of gas occupy?<\/li>\n\t
  8. One mole of liquid N2<\/sub>\u00a0has a volume of 34.65 mL at \u2212196\u00b0C. At that temperature, 1 mol of N2<\/sub> gas has a volume of 6.318 L if the pressure is 1.000 atm. What pressure is needed to compress the N2<\/sub> gas to 34.65 mL?<\/li>\n\t
  9. Use two values of R<\/em> to determine the ratio between an atmosphere and a torr. Does the number make sense?<\/li>\n\t
  10. Use two values of R<\/em> to determine how many joules are in a liter\u00b7atmosphere.<\/li>\n<\/ol>\n11. \u00a0At an altitude of 40 km above the earth\u2019s surface, the atmospheric pressure is 5.00 torr, and the surrounding temperature is \u221220\u00b0C. If a weather balloon is filled with 1.000 mol of He at 760 torr and 22\u00b0C, what is its\n\na) \u00a0initial volume before ascent?\n\nb) \u00a0final volume when it reaches 40 km in altitude? (Assume the pressure of the gas equals the surrounding pressure.)\n\n12. \u00a0If a balloon is filled with 1.000 mol of He at 760 torr and 22\u00b0C, what is its\n\na) \u00a0initial volume before ascent?\n\nb) \u00a0final volume if it descends to the bottom of the Mariana Trench, where the surrounding temperature is 1.4\u00b0C and the pressure is 1,060 atm?\n\n13. \u00a0Air, a mixture of mostly N2<\/sub> and O2<\/sub>, can be approximated as having a molar mass of 28.8 g\/mol. What is the density of air at 1.00 atm and 22\u00b0C? (This is approximately sea level.)\n\n14. \u00a0Air, a mixture of mostly N2<\/sub> and O2<\/sub>, can be approximated as having a molar mass of 28.8 g\/mol. What is the density of air at 0.26 atm and \u221226\u00b0C? (This is approximately the atmospheric condition at the summit of Mount Everest.)\n\n15. \u00a0On the surface of Venus, the atmospheric pressure is 91.8 atm, and the temperature is 460\u00b0C. What is the density of CO2<\/sub> under these conditions? (The Venusian atmosphere is composed largely of CO2<\/sub>.)\n\n16. \u00a0On the surface of Mars, the atmospheric pressure is 4.50 torr, and the temperature is \u221287\u00b0C. What is the density of CO2<\/sub> under these conditions? (The Martian atmosphere, similar to its Venusian counterpart, is composed largely of CO2<\/sub>.)\n\n17. \u00a0HNO3<\/sub> reacts with iron metal according to Fe(s) +\u00a02HNO3<\/sub>(aq) \u2192\u00a0Fe(NO3<\/sub>)2<\/sub>(aq) +\u00a0H2<\/sub>(g) In a reaction vessel, 23.8 g of Fe are reacted but only 446 mL of H2<\/sub> are collected over water at 25\u00b0C and a pressure of 733 torr. What is the percent yield of the reaction?\n\n18. \u00a0NaHCO3<\/sub> is decomposed by heat according to 2NaHCO3<\/sub>(s) \u2192\u00a0Na2<\/sub>CO3<\/sub>(s) +\u00a0H2<\/sub>O(\u2113) +\u00a0CO2<\/sub>(g) If you start with 100.0 g of NaHCO3<\/sub> and collect 10.06 L of CO2<\/sub> over water at 20\u00b0C and 0.977 atm, what is the percent yield of the decomposition reaction?\n\n19. \u00a0Determine if the following actions will cause the pressure of a particular gas sample to increase, decrease, or remain the same:\n\na) \u00a0decreasing the temperature\n\nb) \u00a0decreasing the molar mass of the gas\n\nc) \u00a0decreasing the volume of the container\n\n20. \u00a0Under what conditions do gases deviate\u00a0most from ideal gas behaviour? Explain your answer.\n\n21. \u00a0Place the following gases in order from lowest to highest average molecular speed at 25\u00b0C: He, Ar,\u00a0O2,<\/sub> I2.<\/sub>\n\n22. \u00a0The effusion rate of an unknown noble gas sample is 0.35 times that of neon, at the same temperature. Determine the molecular weight and identity of the unknown noble gas.\n\n23. \u00a0Use the van der Waal's equation to determine the pressure of 2.00 moles of helium in a 5.00 L balloon at 300.00 K. How does this value compare to what you would obtain with the ideal gas law?\n\n<\/div>\n\u00a0\n
    \n

    Answers<\/h3>\n1. <\/strong>208,000 Pa\n\n3. <\/strong>1,874 K\n\n5.<\/strong>\n\n\"Screen<\/a>\n\n7. <\/strong>3.72 \u00d7 10-23<\/sup> L\n\n9. <\/strong>1 atm = 760 torr\n\n11.<\/strong>\n

    11.1. 24.2 L\n11.2. 3155 L<\/p>\n13. <\/strong>1.19 g\/L\n\n15. <\/strong>67.2 g\/L\n\n17. <\/strong>3.99%\n\n19.<\/strong>\n

    19.1. decreased pressure\n19.2. increased pressure\n19.3. increased pressure<\/p>\n21. <\/strong>I2\u00a0<\/sub>< Ar < O2\u00a0<\/sub><\u00a0He\n\n23. <\/strong>van der Waals: 9.94 atm, ideal: 9.85 atm\n\n<\/div>\n\u00a0","rendered":"

    \n

    Additional Exercises<\/h3>\n
      \n
    1. What is the pressure in pascals if a force of 4.88 kN is pressed against an area of 235 cm2<\/sup>?<\/li>\n
    2. What is the pressure in pascals if a force of 3.44 \u00d7104<\/sup>\u00a0MN is pressed against an area of 1.09 k<\/span>m<\/span>2<\/sup>?<\/span><\/li>\n
    3. What is the final temperature of a gas whose initial conditions are 667 mL, 822 torr, and 67\u00b0C, and whose final volume and pressure are 1.334 L and 2.98 atm, respectively? Assume the amount remains constant.<\/li>\n
    4. What is the final pressure of a gas whose initial conditions are 1.407 L, 2.06 atm, and \u221267\u00b0C, and whose final volume and temperature are 608 mL and 449 K, respectively? Assume the amount remains constant.<\/li>\n
    5. Propose a combined gas law that relates volume, pressure, and amount at constant temperature.<\/li>\n
    6. Propose a combined gas law that relates amount, pressure, and temperature at constant volume.<\/li>\n
    7. A sample of 6.022 \u00d710<\/span>23<\/sup>\u00a0particles of gas has a volume of 22.4 L at 0\u00b0C and a pressure of 1.000 atm. Although it may seem silly to contemplate, what volume would one\u00a0particle of gas occupy?<\/li>\n
    8. One mole of liquid N2<\/sub>\u00a0has a volume of 34.65 mL at \u2212196\u00b0C. At that temperature, 1 mol of N2<\/sub> gas has a volume of 6.318 L if the pressure is 1.000 atm. What pressure is needed to compress the N2<\/sub> gas to 34.65 mL?<\/li>\n
    9. Use two values of R<\/em> to determine the ratio between an atmosphere and a torr. Does the number make sense?<\/li>\n
    10. Use two values of R<\/em> to determine how many joules are in a liter\u00b7atmosphere.<\/li>\n<\/ol>\n

      11. \u00a0At an altitude of 40 km above the earth\u2019s surface, the atmospheric pressure is 5.00 torr, and the surrounding temperature is \u221220\u00b0C. If a weather balloon is filled with 1.000 mol of He at 760 torr and 22\u00b0C, what is its<\/p>\n

      a) \u00a0initial volume before ascent?<\/p>\n

      b) \u00a0final volume when it reaches 40 km in altitude? (Assume the pressure of the gas equals the surrounding pressure.)<\/p>\n

      12. \u00a0If a balloon is filled with 1.000 mol of He at 760 torr and 22\u00b0C, what is its<\/p>\n

      a) \u00a0initial volume before ascent?<\/p>\n

      b) \u00a0final volume if it descends to the bottom of the Mariana Trench, where the surrounding temperature is 1.4\u00b0C and the pressure is 1,060 atm?<\/p>\n

      13. \u00a0Air, a mixture of mostly N2<\/sub> and O2<\/sub>, can be approximated as having a molar mass of 28.8 g\/mol. What is the density of air at 1.00 atm and 22\u00b0C? (This is approximately sea level.)<\/p>\n

      14. \u00a0Air, a mixture of mostly N2<\/sub> and O2<\/sub>, can be approximated as having a molar mass of 28.8 g\/mol. What is the density of air at 0.26 atm and \u221226\u00b0C? (This is approximately the atmospheric condition at the summit of Mount Everest.)<\/p>\n

      15. \u00a0On the surface of Venus, the atmospheric pressure is 91.8 atm, and the temperature is 460\u00b0C. What is the density of CO2<\/sub> under these conditions? (The Venusian atmosphere is composed largely of CO2<\/sub>.)<\/p>\n

      16. \u00a0On the surface of Mars, the atmospheric pressure is 4.50 torr, and the temperature is \u221287\u00b0C. What is the density of CO2<\/sub> under these conditions? (The Martian atmosphere, similar to its Venusian counterpart, is composed largely of CO2<\/sub>.)<\/p>\n

      17. \u00a0HNO3<\/sub> reacts with iron metal according to Fe(s) +\u00a02HNO3<\/sub>(aq) \u2192\u00a0Fe(NO3<\/sub>)2<\/sub>(aq) +\u00a0H2<\/sub>(g) In a reaction vessel, 23.8 g of Fe are reacted but only 446 mL of H2<\/sub> are collected over water at 25\u00b0C and a pressure of 733 torr. What is the percent yield of the reaction?<\/p>\n

      18. \u00a0NaHCO3<\/sub> is decomposed by heat according to 2NaHCO3<\/sub>(s) \u2192\u00a0Na2<\/sub>CO3<\/sub>(s) +\u00a0H2<\/sub>O(\u2113) +\u00a0CO2<\/sub>(g) If you start with 100.0 g of NaHCO3<\/sub> and collect 10.06 L of CO2<\/sub> over water at 20\u00b0C and 0.977 atm, what is the percent yield of the decomposition reaction?<\/p>\n

      19. \u00a0Determine if the following actions will cause the pressure of a particular gas sample to increase, decrease, or remain the same:<\/p>\n

      a) \u00a0decreasing the temperature<\/p>\n

      b) \u00a0decreasing the molar mass of the gas<\/p>\n

      c) \u00a0decreasing the volume of the container<\/p>\n

      20. \u00a0Under what conditions do gases deviate\u00a0most from ideal gas behaviour? Explain your answer.<\/p>\n

      21. \u00a0Place the following gases in order from lowest to highest average molecular speed at 25\u00b0C: He, Ar,\u00a0O2,<\/sub> I2.<\/sub><\/p>\n

      22. \u00a0The effusion rate of an unknown noble gas sample is 0.35 times that of neon, at the same temperature. Determine the molecular weight and identity of the unknown noble gas.<\/p>\n

      23. \u00a0Use the van der Waal’s equation to determine the pressure of 2.00 moles of helium in a 5.00 L balloon at 300.00 K. How does this value compare to what you would obtain with the ideal gas law?<\/p>\n<\/div>\n

      \u00a0<\/p>\n

      \n

      Answers<\/h3>\n

      1. <\/strong>208,000 Pa<\/p>\n

      3. <\/strong>1,874 K<\/p>\n

      5.<\/strong><\/p>\n

      \"Screen<\/a><\/p>\n

      7. <\/strong>3.72 \u00d7 10-23<\/sup> L<\/p>\n

      9. <\/strong>1 atm = 760 torr<\/p>\n

      11.<\/strong><\/p>\n

      11.1. 24.2 L
      \n11.2. 3155 L<\/p>\n

      13. <\/strong>1.19 g\/L<\/p>\n

      15. <\/strong>67.2 g\/L<\/p>\n

      17. <\/strong>3.99%<\/p>\n

      19.<\/strong><\/p>\n

      19.1. decreased pressure
      \n19.2. increased pressure
      \n19.3. increased pressure<\/p>\n

      21. <\/strong>I2\u00a0<\/sub>< Ar < O2\u00a0<\/sub><\u00a0He<\/p>\n

      23. <\/strong>van der Waals: 9.94 atm, ideal: 9.85 atm<\/p>\n<\/div>\n

      \u00a0<\/p>\n\n\t\t\t

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