{"id":7371,"date":"2021-06-08T21:55:57","date_gmt":"2021-06-08T21:55:57","guid":{"rendered":"https:\/\/opentextbc.ca\/introductorychemistry\/chapter\/end-of-chapter-6-material\/"},"modified":"2021-09-24T16:33:33","modified_gmt":"2021-09-24T16:33:33","slug":"end-of-chapter-6-material","status":"publish","type":"chapter","link":"https:\/\/opentextbc.ca\/introductorychemistry\/chapter\/end-of-chapter-6-material\/","title":{"raw":"End-of-Chapter Material","rendered":"End-of-Chapter Material"},"content":{"raw":"[latexpage]\r\n
\r\n

Additional Exercises<\/p>\r\n\r\n<\/header>\r\n

\r\n
    \r\n \t
  1. What is the pressure in pascals if a force of 4.88 kN is pressed against an area of 235 cm2<\/sup>?<\/li>\r\n \t
  2. What is the pressure in pascals if a force of 3.44 \u00d7 104<\/sup>\u00a0MN is pressed against an area of 1.09 km2<\/sup>?<\/li>\r\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>\r\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>\r\n \t
  5. Propose a combined gas law that relates volume, pressure, and amount at constant temperature.<\/li>\r\n \t
  6. Propose a combined gas law that relates amount, pressure, and temperature at constant volume.<\/li>\r\n \t
  7. A sample of 6.022 \u00d71023<\/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>\r\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>\r\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>\r\n \t
  10. Use two values of R<\/em> to determine how many joules are in a litre-atmosphere.<\/li>\r\n \t
  11. At 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:\r\n
      \r\n \t
    1. initial volume before ascent?<\/li>\r\n \t
    2. final volume when it reaches 40 km in altitude? (Assume the pressure of the gas equals the surrounding pressure.)<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
    3. If a balloon is filled with 1.000 mol of He at 760 torr and 22\u00b0C, what is its:\r\n
        \r\n \t
      1. initial volume before ascent?<\/li>\r\n \t
      2. final 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?<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
      3. Air \u2014 a mixture of mostly N2<\/sub> and O2\u00a0<\/sub>\u2014 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.)<\/li>\r\n \t
      4. Air \u2014 a mixture of mostly N2<\/sub> and O2\u00a0<\/sub>\u2014 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.)<\/li>\r\n \t
      5. On 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>.)<\/li>\r\n \t
      6. On 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>.)<\/li>\r\n \t
      7. HNO3<\/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?<\/li>\r\n \t
      8. NaHCO3<\/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?<\/li>\r\n \t
      9. Determine if the following actions will cause the pressure of a particular gas sample to increase, decrease, or remain the same:\r\n
          \r\n \t
        1. decreasing the temperature<\/li>\r\n \t
        2. decreasing the molar mass of the gas<\/li>\r\n \t
        3. decreasing the volume of the container<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
        4. Under what conditions do gases deviate\u00a0most from ideal gas behaviour? Explain your answer.<\/li>\r\n \t
        5. Place the following gases in order from lowest to highest average molecular speed at 25\u00b0C: He, Ar,\u00a0O2,<\/sub> I2<\/sub>.<\/li>\r\n \t
        6. The 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.<\/li>\r\n \t
        7. Use the van der Waals 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?<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n
          \r\n

          Answers<\/p>\r\n\r\n<\/header>\r\n

          \r\n
            \r\n \t
          1. 208,000 Pa<\/li>\r\n<\/ol>\r\n
              \r\n \t
            1. 1,874 K<\/li>\r\n<\/ol>\r\n
                \r\n \t
              1. [latex]\\dfrac{P_1V_1}{n_1}=\\dfrac{P_2V_2}{n_2}[\/latex]<\/li>\r\n<\/ol>\r\n
                  \r\n \t
                1. 3.72 \u00d7 10\u221223<\/sup> L<\/li>\r\n<\/ol>\r\n
                    \r\n \t
                  1. 1 atm = 760 torr<\/li>\r\n<\/ol>\r\n
                      \r\n \t
                    1. \r\n
                        \r\n \t
                      1. 24.2 L<\/li>\r\n \t
                      2. 3155 L<\/li>\r\n<\/ol>\r\n<\/li>\r\n<\/ol>\r\n
                          \r\n \t
                        1. 1.19 g\/L<\/li>\r\n<\/ol>\r\n
                            \r\n \t
                          1. 67.2 g\/L<\/li>\r\n<\/ol>\r\n
                              \r\n \t
                            1. 3.99%<\/li>\r\n<\/ol>\r\n
                                \r\n \t
                              1. \r\n
                                  \r\n \t
                                1. decreased pressure<\/li>\r\n \t
                                2. increased pressure<\/li>\r\n \t
                                3. increased pressure<\/li>\r\n<\/ol>\r\n<\/li>\r\n<\/ol>\r\n
                                    \r\n \t
                                  1. I2\u00a0<\/sub>< Ar < O2\u00a0<\/sub><\u00a0He<\/li>\r\n<\/ol>\r\n
                                      \r\n \t
                                    1. van der Waals: 9.94 atm, ideal: 9.85 atm<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>","rendered":"
                                      \n
                                      \n

                                      Additional Exercises<\/p>\n<\/header>\n

                                      \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 \u00d7 104<\/sup>\u00a0MN is pressed against an area of 1.09 km2<\/sup>?<\/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 \u00d71023<\/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 litre-atmosphere.<\/li>\n
                                      11. At 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
                                          \n
                                        1. initial volume before ascent?<\/li>\n
                                        2. final volume when it reaches 40 km in altitude? (Assume the pressure of the gas equals the surrounding pressure.)<\/li>\n<\/ol>\n<\/li>\n
                                        3. If a balloon is filled with 1.000 mol of He at 760 torr and 22\u00b0C, what is its:\n
                                            \n
                                          1. initial volume before ascent?<\/li>\n
                                          2. final 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?<\/li>\n<\/ol>\n<\/li>\n
                                          3. Air \u2014 a mixture of mostly N2<\/sub> and O2\u00a0<\/sub>\u2014 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.)<\/li>\n
                                          4. Air \u2014 a mixture of mostly N2<\/sub> and O2\u00a0<\/sub>\u2014 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.)<\/li>\n
                                          5. On 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>.)<\/li>\n
                                          6. On 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>.)<\/li>\n
                                          7. HNO3<\/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?<\/li>\n
                                          8. NaHCO3<\/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?<\/li>\n
                                          9. Determine if the following actions will cause the pressure of a particular gas sample to increase, decrease, or remain the same:\n
                                              \n
                                            1. decreasing the temperature<\/li>\n
                                            2. decreasing the molar mass of the gas<\/li>\n
                                            3. decreasing the volume of the container<\/li>\n<\/ol>\n<\/li>\n
                                            4. Under what conditions do gases deviate\u00a0most from ideal gas behaviour? Explain your answer.<\/li>\n
                                            5. Place the following gases in order from lowest to highest average molecular speed at 25\u00b0C: He, Ar,\u00a0O2,<\/sub> I2<\/sub>.<\/li>\n
                                            6. The 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.<\/li>\n
                                            7. Use the van der Waals 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?<\/li>\n<\/ol>\n<\/div>\n<\/div>\n
                                              \n
                                              \n

                                              Answers<\/p>\n<\/header>\n

                                              \n
                                                \n
                                              1. 208,000 Pa<\/li>\n<\/ol>\n
                                                  \n
                                                1. 1,874 K<\/li>\n<\/ol>\n
                                                    \n
                                                  1. \"\dfrac{P_1V_1}{n_1}=\dfrac{P_2V_2}{n_2}\"<\/li>\n<\/ol>\n
                                                      \n
                                                    1. 3.72 \u00d7 10\u221223<\/sup> L<\/li>\n<\/ol>\n
                                                        \n
                                                      1. 1 atm = 760 torr<\/li>\n<\/ol>\n
                                                          \n
                                                        1. \n
                                                            \n
                                                          1. 24.2 L<\/li>\n
                                                          2. 3155 L<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n
                                                              \n
                                                            1. 1.19 g\/L<\/li>\n<\/ol>\n
                                                                \n
                                                              1. 67.2 g\/L<\/li>\n<\/ol>\n
                                                                  \n
                                                                1. 3.99%<\/li>\n<\/ol>\n
                                                                    \n
                                                                  1. \n
                                                                      \n
                                                                    1. decreased pressure<\/li>\n
                                                                    2. increased pressure<\/li>\n
                                                                    3. increased pressure<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n
                                                                        \n
                                                                      1. I2\u00a0<\/sub>< Ar < O2\u00a0<\/sub><\u00a0He<\/li>\n<\/ol>\n
                                                                          \n
                                                                        1. van der Waals: 9.94 atm, ideal: 9.85 atm<\/li>\n<\/ol>\n<\/div>\n<\/div>\n","protected":false},"author":90,"menu_order":9,"template":"","meta":{"pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[48],"license":[],"class_list":["post-7371","chapter","type-chapter","status-publish","hentry","contributor-david-w-ball"],"part":7346,"_links":{"self":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/7371","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/wp\/v2\/users\/90"}],"version-history":[{"count":1,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/7371\/revisions"}],"predecessor-version":[{"id":8356,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/7371\/revisions\/8356"}],"part":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/parts\/7346"}],"metadata":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/7371\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/wp\/v2\/media?parent=7371"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapter-type?post=7371"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/wp\/v2\/contributor?post=7371"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/wp\/v2\/license?post=7371"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}