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Chapter 4 Stoichiometry of Chemical Reactions 211 The plan for this calculation is similar to others used in stoichiometric calculations, the central step being the connection between the moles of BaSO4 and CaSO4 through their stoichiometric factor. Once the mass of CaSO4 is computed, it may be used along with the mass of the sample mixture to calculate the requested percentage concentration. The mass of CaSO4 that would yield the provided precipitate mass is 0.6168 g BaSO4 × 1 mol BaSO4 × 1 mol CaSO4 × 136.14 g CaSO4 = 0.3597 g CaSO4 233.43 g BaSO4 1 mol BaSO4 1 mol CaSO4 The concentration of CaSO4 in the sample mixture is then calculated to be percent CaSO4 = mass CaSO4 × 100% mass sample 0.3597 g × 100% = 79.05% 0.4550 g Check Your Learning What is the percent of chloride ion in a sample if 1.1324 g of the sample produces 1.0881 g of AgCl when treated with excess Ag+? Ag+(aq) + Cl−(aq) ⟶ AgCl(s) Answer: 23.76% The elemental composition of hydrocarbons and related compounds may be determined via a gravimetric method known as combustion analysis. In a combustion analysis, a weighed sample of the compound is heated to a high temperature under a stream of oxygen gas, resulting in its complete combustion to yield gaseous products of known identities. The complete combustion of hydrocarbons, for example, will yield carbon dioxide and water as the only products. The gaseous combustion products are swept through separate, preweighed collection devices containing compounds that selectively absorb each product (Figure 4.17). The mass increase of each device corresponds to the mass of the absorbed product and may be used in an appropriate stoichiometric calculation to derive the mass of the relevant element.PDF Image | Stoichiometry of Chemical Reactions
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