{"id":197,"date":"2016-01-11T19:59:43","date_gmt":"2016-01-11T19:59:43","guid":{"rendered":"https:\/\/opentextbc.ca\/introductorychemistryclone\/chapter\/mole-mass-and-mass-mass-calculations-2\/"},"modified":"2020-05-06T20:15:16","modified_gmt":"2020-05-06T20:15:16","slug":"mole-mass-and-mass-mass-calculations","status":"publish","type":"chapter","link":"https:\/\/opentextbc.ca\/introductorychemistryclone\/chapter\/mole-mass-and-mass-mass-calculations\/","title":{"raw":"Mole-Mass and Mass-Mass Calculations","rendered":"Mole-Mass and Mass-Mass Calculations"},"content":{"raw":"[latexpage]\r\n
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Learning Objectives<\/p>\r\n\r\n<\/header>\r\n

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  1. From a given number of moles of a substance, calculate the mass of another substance involved using the balanced chemical equation.<\/li>\r\n \t
  2. From a given mass of a substance, calculate the moles of another substance involved using the balanced chemical equation.<\/li>\r\n \t
  3. From a given mass of a substance, calculate the mass of another substance involved using the balanced chemical equation.<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\nMole-mole calculations are not the only type of calculations that can be performed using balanced chemical equations. Recall that the molar mass can be determined from a chemical formula and used as a conversion factor. We can add that conversion factor as another step in a calculation to make a [pb_glossary id=\"1478\"]mole-mass calculation[\/pb_glossary], where we start with a given number of moles of a substance and calculate the mass of another substance involved in the chemical equation, or vice versa.\r\n\r\nFor example, suppose we have the balanced chemical equation:\r\n

    2Al + 3Cl2<\/sub> \u2192 2AlCl3<\/sub><\/p>\r\nSuppose we know we have 123.2 g of Cl2<\/sub>. How can we determine how many moles of AlCl3<\/sub> we will get when the reaction is complete? First and foremost, chemical equations are not balanced in terms of grams; they are balanced in terms of moles<\/i>. So to use the balanced chemical equation to relate an amount of Cl2<\/sub> to an amount of AlCl3<\/sub>, we need to convert the given amount of Cl2<\/sub> into moles. We know how to do this by simply using the molar mass of Cl2<\/sub> as a conversion factor. The molar mass of Cl2<\/sub> (which we get from the atomic mass of Cl from the periodic table) is 70.90 g\/mol. We must invert this fraction so that the units cancel properly:\r\n\r\n\\[123.2 \\cancel{\\text{ g }\\ce{Cl2}}\\times \\dfrac{1\\text{ mol }\\ce{Cl2}}{70.90\\cancel{\\text{ g }\\ce{Cl2}}}=1.738\\text{ mol }\\ce{Cl2}\\]\r\n\r\nNow that we have the quantity in moles, we can use the balanced chemical equation to construct a conversion factor that relates the number of moles of Cl2<\/sub> to the number of moles of AlCl3<\/sub>. The numbers in the conversion factor come from the coefficients in the balanced chemical equation:\r\n\r\n\\[\\dfrac{2\\text{ mol }\\ce{AlCl3}}{3\\text{ mol }\\ce{Cl2}}\\]\r\n\r\nUsing this conversion factor with the molar quantity we calculated above, we get:\r\n\r\n\\[1.738\\cancel{\\text{ mol }\\ce{Cl2}}\\times \\dfrac{2\\text{ mol }\\ce{AlCl3}}{3\\cancel{\\text{ mol }\\ce{Cl2}}}=1.159\\text{ mol }\\ce{AlCl3}\\]\r\n\r\nSo, we will get 1.159 mol of AlCl3<\/sub> if we react 123.2 g of Cl2<\/sub>.\r\n\r\nIn this last example, we did the calculation in two steps. However, it is mathematically equivalent to perform the two calculations sequentially on one line:\r\n\r\n\\[123.2\\cancel{\\text{ g }\\ce{Cl2}}\\times \\dfrac{1\\cancel{\\text{ mol }\\ce{Cl2}}}{70.90\\cancel{\\text{ g }\\ce{Cl2}}}\\times \\dfrac{2\\text{ mol }\\ce{AlCl3}}{3\\cancel{\\text{ mol }\\ce{Cl2}}}=1.159\\text{ mol }\\ce{AlCl3}\\]\r\n\r\nThe units still cancel appropriately, and we get the same numerical answer in the end. Sometimes the answer may be slightly different from doing it one step at a time because of rounding of the intermediate answers, but the final answers should be effectively the same.\r\n

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    Example 5.8<\/p>\r\n\r\n<\/header>\r\n

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    Problem<\/h1>\r\nHow many moles of HCl will be produced when 249 g of AlCl3<\/sub> are reacted according to this chemical equation?\r\n

    2AlCl3<\/sub> + 3H2<\/sub>O(\u2113) \u2192 Al2<\/sub>O3<\/sub> + 6HCl(g)<\/p>\r\n\r\n

    Solution<\/h2>\r\nWe will do this in two steps: convert the mass of AlCl3<\/sub> to moles and then use the balanced chemical equation to find the number of moles of HCl formed. The molar mass of AlCl3<\/sub> is 133.33 g\/mol, which we have to invert to get the appropriate conversion factor:\r\n\r\n\\[1.87\\cancel{\\text{ mol }\\ce{AlCl3}}\\times \\dfrac{6\\text{ mol }\\ce{HCl}}{2\\cancel{\\text{ mol }\\ce{AlCl3}}}=5.61\\text{ mol }\\ce{HCl}\\]\r\n\r\nNow we can use this quantity to determine the number of moles of HCl that will form. From the balanced chemical equation, we construct a conversion factor between the number of moles of AlCl3<\/sub> and the number of moles of HCl:\r\n\r\n\\[\\dfrac{6\\text{ mol }\\ce{HCl}}{2\\text{ mol }\\ce{AlCl3}}\\]\r\n\r\nApplying this conversion factor to the quantity of AlCl3<\/sub>, we get:\r\n\r\n\\[1.87\\cancel{\\text{ mol }\\ce{AlCl3}}\\times \\dfrac{6\\text{ mol }\\ce{HCl}}{2\\cancel{\\text{ mol }\\ce{AlCl3}}}=5.61\\text{ mol }\\ce{HCl}\\]\r\n\r\nAlternatively, we could have done this in one line:\r\n\r\n\\[2.49\\cancel{\\text{ g }\\ce{AlCl3}}\\times \\dfrac{1\\cancel{\\text{ mol }\\ce{AlCl3}}}{133.33\\cancel{\\text{ g }\\ce{AlCl3}}} \\times \\dfrac{6\\text{ mol }\\ce{HCl}}{2\\cancel{\\text{ mol }\\ce{AlCl3}}} = 5.60\\text{ mol }\\ce{HCl}\\]\r\n\r\nThe last digit in our final answer is slightly different because of rounding differences, but the answer is essentially the same.\r\n

    Test Yourself<\/h1>\r\nHow many moles of Al2<\/sub>O3<\/sub> will be produced when 23.9 g of H2<\/sub>O are reacted according to this chemical equation?\r\n

    2AlCl3<\/sub> + 3H2<\/sub>O(\u2113) \u2192 Al2<\/sub>O3<\/sub> + 6HCl(g)<\/p>\r\n\r\n

    Answer<\/h2>\r\n0.442 mol\r\n\r\n<\/div>\r\n<\/div>\r\nA variation of the mole-mass calculation is to start with an amount in moles and then determine an amount of another substance in grams. The steps are the same but are performed in reverse order.\r\n
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    Example 5.9<\/p>\r\n\r\n<\/header>\r\n

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    Problem<\/h1>\r\nHow many grams of NH3<\/sub> will be produced when 33.9 mol of H2<\/sub> are reacted according to this chemical equation?\r\n

    N2<\/sub>(g) + 3H2<\/sub>(g) \u2192 2NH3<\/sub>(g)<\/p>\r\n\r\n

    Solution<\/h2>\r\nThe conversions are the same, but they are applied in a different order. Start by using the balanced chemical equation to convert to moles of another substance and then use its molar mass to determine the mass of the final substance. In two steps, we have:\r\n\r\n\\[33.9\\cancel{\\text{ mol }\\ce{H2}}\\times \\dfrac{2\\text{ mol }\\ce{NH3}}{3\\cancel{\\text{ mol }\\ce{H2}}}=22.6\\text{ mol }\\ce{NH3}\\]\r\n\r\nNow, using the molar mass of NH3<\/sub>, which is 17.03 g\/mol, we get:\r\n\r\n\\[22.6\\cancel{\\text{ mol }\\ce{NH3}}\\times \\dfrac{17.03\\text{ g }\\ce{NH3}}{1\\cancel{\\text{ mol }\\ce{NH3}}}=385\\text{ g }\\ce{NH3}\\]\r\n

    Test Yourself<\/h1>\r\nHow many grams of N2<\/sub> are needed to produce 2.17 mol of NH3<\/sub> when reacted according to this chemical equation?\r\n

    N2<\/sub>(g) + 3H2<\/sub>(g) \u2192 2NH3<\/sub>(g)<\/p>\r\n\r\n

    Answer<\/h2>\r\n30.4 g (Note: here we go from a product to a reactant, showing that mole-mass problems can begin and end with any substance in the chemical equation.)\r\n\r\n<\/div>\r\n<\/div>\r\nIt should be a trivial task now to extend the calculations to [pb_glossary id=\"1479\"]mass-mass calculations[\/pb_glossary], in which we start with a mass of some substance and end with the mass of another substance in the chemical reaction. For this type of calculation, the molar masses of two different substances must be used\u2014be sure to keep track of which is which. Again, however, it is important to emphasize that before the balanced chemical reaction is used, the mass quantity must first be converted to moles. Then the coefficients of the balanced chemical reaction can be used to convert to moles of another substance, which can then be converted to a mass.\r\n\r\nFor example, let us determine the number of grams of SO3<\/sub> that can be produced by the reaction of 45.3 g of SO2<\/sub> and O2<\/sub>:\r\n

    2SO2<\/sub>(g) +\u00a0O2<\/sub>(g) \u2192 2SO3<\/sub>(g)<\/p>\r\nFirst, we convert the given amount, 45.3 g of SO2<\/sub>, to moles of SO2<\/sub> using its molar mass (64.06 g\/mol):\r\n\r\n\\[45.3\\cancel{\\text{ g }\\ce{SO2}}\\times \\dfrac{1\\text{ mol }\\ce{SO2}}{64.06\\cancel{\\text{ g }\\ce{SO2}}}=0.707\\text{ mol }\\ce{SO2}\\]\r\n\r\nSecond, we use the balanced chemical reaction to convert from moles of SO2<\/sub> to moles of SO3<\/sub>:\r\n\r\n\\[0.707\\cancel{\\text{ mol }\\ce{SO2}}\\times \\dfrac{2\\text{ mol }\\ce{SO3}}{2\\cancel{\\text{ mol }\\ce{SO2}}}=0.707\\text{ mol }\\ce{SO3}\\]\r\n\r\nFinally, we use the molar mass of SO3<\/sub> (80.06 g\/mol) to convert to the mass of SO3<\/sub>:\r\n\r\n\\[0.707\\cancel{\\text{ mol }\\ce{SO3}}\\times \\dfrac{80.06\\text{ g }\\ce{SO3}}{1\\cancel{\\text{ mol }\\ce{SO3}}}=56.6\\text{ g }\\ce{SO3}\\]\r\n\r\nWe can also perform all three steps sequentially, writing them on one line as:\r\n

    \\(45.3\\cancel{\\text{ g }\\ce{SO2}}\\times \\dfrac{1\\cancel{\\text{ mol }\\ce{SO2}}}{64.06\\cancel{\\text{ g }\\ce{SO2}}}\\times \\dfrac{2\\cancel{\\text{ mol }\\ce{SO3}}}{2\\cancel{\\text{ mol }\\ce{SO2}}}\\times \\dfrac{80.06\\text{ g }\\ce{SO3}}{1\\cancel{\\text{ mol }\\ce{SO3}}}=56.6\\text{ g }\\ce{SO3}\\)<\/p>\r\nWe get the same answer. Note how the initial and all the intermediate units cancel, leaving grams of SO3<\/sub>, which is what we are looking for, as our final answer.\r\n

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    Example 5.10<\/p>\r\n\r\n<\/header>\r\n

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    Problem<\/h1>\r\nWhat mass of Mg will be produced when 86.4 g of K are reacted?\r\n

    MgCl2<\/sub>(s) + 2K(s) \u2192 Mg(s) + 2KCl(s)<\/p>\r\n\r\n

    Solution<\/h2>\r\nWe will simply follow the steps:\r\n

    mass K \u2192 mol K \u2192 mol Mg \u2192 mass Mg<\/p>\r\nIn addition to the balanced chemical equation, we need the molar masses of K (39.09 g\/mol) and Mg (24.31 g\/mol). In one line,\r\n\r\n\\[86.4\\cancel{\\text{ g K}}\\times \\dfrac{1\\cancel{\\text{ mol K}}}{39.09\\cancel{\\text{ g K}}}\\times \\dfrac{1\\cancel{\\text{ mol Mg}}}{2\\cancel{\\text{ mol K}}}\\times \\dfrac{24.31\\text{ g Mg}}{1\\cancel{\\text{ mol Mg}}}=26.87 \\text{ Mg}\\]\r\n

    Test Yourself<\/h1>\r\nWhat mass of H2<\/sub> will be produced when 122 g of Zn are reacted?\r\n

    Zn(s) + 2 HCl(aq) \u2192 ZnCl2<\/sub>(aq) + H2<\/sub>(g)<\/p>\r\n\r\n

    Answer<\/h2>\r\n3.77 g\r\n\r\n<\/div>\r\n<\/div>\r\n
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    Key Takeaways<\/p>\r\n\r\n<\/header>\r\n

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