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Unit: Stoichiometry Lesson: #10 Topics: Solvay Process

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Unit: Stoichiometry Lesson: #10 Topics: Solvay Process Unit: Stoichiometry Lesson: #10 Topics: Solvay Process The Solvay Process: A Case Study Many important industrial processes involve chemical reactions that are difficult to perform and still be economically feasible. In some cases, the overall process must follow a series of reaction steps. Sodium carbonate is a chemical that is needed in large amounts – it is used in the production of glass and soap. Historically, sodium carbonate was produced by burning plants or coal and mixing the ashes with water This method was both inefficient and very expensive because of the large amount of material that needed to be burned. The Solvay process was developed as a cost effective alternative. It involves a series of reaction steps and has a net reaction of: CaCO3 (s) + 2 NaCl (aq) Na2CO3 (aq) + CaCl2 (aq) A net reaction is determined by looking at the various reaction steps and eliminating any chemical that appears as both a reactant and a product in the various steps. These chemicals are known as intermediates. Step 1: Calcium carbonate (limestone) is decomposed by heat to form calcium oxide (lime) and carbon dioxide. CaCO3 (s) CaO (s) + CO2 (g) Step 2: Carbon dioxide reacts with aqueous ammonia and water to form aqueous ammonium hydrogen carbonate. CO2 (g) + NH3 (aq) + H2O (l) NH4HCO3 (aq) Step 3: The aqueous ammonium hydrogen carbonate reacts with sodium chloride to produce ammonium chloride and solid baking soda. NH4HCO3 (aq) + NaCl (aq) NH4Cl (aq) + NaHCO3 (s) Step 4: The baking soda is heated up and decomposed into sodium carbonate, water vapor and carbon dioxide. 2 NaHCO3 (s) Na2CO3 (s) + H2O (g) + CO2 (g) Step 5: The lime that was produced in the first step is mixed with water to produce slaked lime (calcium hydroxide). CaO (s) + H2O (l) Ca(OH)2 (s) Step 6: The slaked lime is added to the ammonium chloride produced in the third step to produce ammonia, calcium chloride and water. Ca(OH)2 (s) + 2 NH4Cl (aq) 2 NH3 (aq) + CaCl2 (aq) + 2 H2O (l) Net Reaction): CaCO3 (s) + 2 NaCl (aq) Na2CO3 (s) + CaCl2 (aq) The two raw materials used up in the Solvay process (calcium carbonate and sodium chloride) are abundantly available and very cheap. The primary product is the sodium carbonate. A by-product is the calcium chloride which can be sold as a dessicant or as road salt to melt ice. The baking soda made in step 3 can also be sold as a byproduct but this limits the amount of sodium carbonate that can be produced. Homework: See accompanying sheet. Chem 20 Stoichiometry and the Solvay Process Use a above balanced equation to answer each of the following questions. 1. What mass of lime (see step 1 for names) can be produced by the decomposition of 400 kg of limestone in step 1 of the Solvay process? m = 224 kg 2. What volume of 1.45 mol/L ammonia would be required to produce 275 kg of ammonium hydrogen carbonate in step 2 of the Solvay process? V = 2.40 X 103 L 3. What volume of 0.75 mol/L sodium chloride would be required to react with 350 kg of ammonium hydrogen carbonate in step 3 of the Solvay process? V = 5.9 X 103 L 4. What volume of carbon dioxide gas will be generated at SATP by the decomposition of 180 kg of sodium hydrogen carbonate in step 4 of the Solvay process? V = 2.66 X 104 L 5. What mass of water is required to react with lime in step 5 of the Solvay process in order to produce 370 kg of slaked lime? m = 90.0 kg 6. Calculate the concentration of ammonium chloride if 87 kL is required to react with 190 kg of slaked lime in step 6 of the Solvay process. C = 0.059 mol/L 7. What mass of sodium carbonate can be produced during the Solvay process if 250 kg of calcium carbonate is allowed to react with 3000 L of 1.72 mol/L sodium chloride (refer to the net reaction equation)? m = 265 kg .
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