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 2000C : CaCO3(s)CaO(s)+CO2(g)H=177.8kJ/mol Slaked lime is produced by treating quicklime with water: CaO(s)+H2O(()Ca(OH)2(s)H=65.2kJ/mol The exothermic reaction of quicklime with water and the rather small specific heats of both quicklime (0.946J/gC) and slaked lime (1.20J/gC) make it hazardous to store and transport lime in vessels made of wood. Wooden sailing ships carrying lime would occasionally catch fire when water leaked into the hold. (a) If a 500-g sample of water reacts with an equimolar amount of CaO (both at an initial temperature of 25C ), what is the final temperature of the product, Ca(OH)2 ? Assume that the product absorbs all of the heat released in the reaction. (5 pts)