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Introduction & Overview
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The laboratory preparation of ammonia predominantly involves the reaction between ammonium chloride (NHβCl) and slaked lime (Ca(OH)β). This section delves into the chemical reaction, physical properties, and uses of ammonia, emphasizing its significance in industrial applications.
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Reaction of Ammonium Chloride and Slaked Lime
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β By heating ammonium chloride with slaked lime:
2NH4Cl+Ca(OH)2β2NH3β+CaCl2+2H2O
2NH_4Cl + Ca(OH)_2
ightarrow 2NH_3 + CaCl_2 + 2H_2O
Detailed Explanation
In this reaction, ammonium chloride (NHβCl) is heated together with slaked lime (calcium hydroxide, Ca(OH)β). During the reaction, ammonium chloride decomposes and produces ammonia gas (NHβ), calcium chloride (CaClβ), and water (HβO). The equation represents that for every two parts of ammonium chloride used, one part of slaked lime is required, resulting in two volumes of ammonia gas released.
Examples & Analogies
Imagine baking cookies where ammonium chloride is like flour and slaked lime is like baking powder. When you combine them under heat (mix and bake), you get delicious cookies (ammonia gas) along with leftover ingredients (calcium chloride and water) that are not needed for the final treat.
Products of the Reaction
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β³ 2NH3β + CaCl2 + 2H2O
Detailed Explanation
The reaction produces three important products: ammonia gas (NHβ), calcium chloride (CaClβ), and water (HβO). The ammonia gas is the desired product in this preparation, which can be collected from the reaction. This gas is used in various applications including agriculture as fertilizer. The remaining calcium chloride and water can also be used in other chemical processes or as by-products.
Examples & Analogies
Think about when you brew your favorite tea. The tea leaves (ammonia) that come out of the brewing process are what you want, but you also have leftover water (which can be reused for watering plants) and tea leaves (calcium chloride, potential use in composting).