Lime is a term that includes calcium oxide (CaO, also called quicklime) and calcium hydroxide [Ca(OH)2,...

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Lime is a term that includes calcium oxide (CaO, also called quicklime) and calcium hydroxide [Ca(OH)2, also called slaked lime]. It is used in the steel industry to remove acidic impurities, in air-pollution control to remove acidic oxides such as SO2, and in water treatment. Quicklime is made industrially by heating limestone (CaCO3) above 2000°C. Slaked lime is produced by treating quicklime with water. The exothermic reaction of quicklime with water and the rather small specific heats of both quicklime (0.946 J/g? °C) and slaked lime (1.20 J/g? °C) make it hazardous to store and transport lime in vessels made of wood. Wooden sailing ships carrying lime would occasionally catch fi re when water leaked into the hold. If a 50-g sample of water reacts with an equimolar amount of Cao (both at an initial temperature of 25°C), what is the final temperature of the product, Ca(OH)2? Assume that the product absorbs all of the heat released in the reaction. CACO3(s) → CaO(s) + CO2(g) ΔΗ = 177.8 kJ/mol CaO(s) + H2O(1) → Ca(OH)2(s) AH° = -65.2 kJ/mol Lime is a term that includes calcium oxide (CaO, also called quicklime) and calcium hydroxide [Ca(OH)2, also called slaked lime]. It is used in the steel industry to remove acidic impurities, in air-pollution control to remove acidic oxides such as SO2, and in water treatment. Quicklime is made industrially by heating limestone (CaCO3) above 2000°C. Slaked lime is produced by treating quicklime with water. The exothermic reaction of quicklime with water and the rather small specific heats of both quicklime (0.946 J/g? °C) and slaked lime (1.20 J/g? °C) make it hazardous to store and transport lime in vessels made of wood. Wooden sailing ships carrying lime would occasionally catch fi re when water leaked into the hold. If a 50-g sample of water reacts with an equimolar amount of Cao (both at an initial temperature of 25°C), what is the final temperature of the product, Ca(OH)2? Assume that the product absorbs all of the heat released in the reaction. CACO3(s) → CaO(s) + CO2(g) ΔΗ = 177.8 kJ/mol CaO(s) + H2O(1) → Ca(OH)2(s) AH° = -65.2 kJ/mol

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Given CaOH2OCaOH2H652KJmol Specific heat ofCaOH212JgmC To calculate the amount of heat released ... View the full answer