ring Calorimetry (ã) 80f 11 Part A A calorimeter is an insulated device in which a chemical reaction is contained. By measuring the temperature change, AT, we can calculate the heat released or absorbed during the reaction using the following equation bus A calorimeter contains 280 mL of water at 12.0ãCãwhen 250 g otX (a substance with a molar mass of 76.0 g/mol ) is added, it dissolves via the reaction X(s) +H20(l)-+X(aq) and the temperature of the solution increases to 260 C Calculate the enthalpy change, Î H. for this reaction per mole of x. Assume that the specific heat of the resulting solution is equal to that of water 14.18 J/( surroundings. Express the change in enthalpy in kilojoules per mole to three significant figures. View Available Hint(s) q = specific heat à mass à ÎT mic ules Or, if the calorimeter has a predetermined heat capacity, C, the equation becomes C)L, that At constant pressure, the enthalpy change for the Settin reaction, AH, is equal to the heat, g,: that is, se Toc but it is usually expressed per mole of reactant and with a sign opposite to that of q for the surroundings. The total internal energy change, AE (sometimes referred to as Î is the sum of heat, g, and work done, w kJ/mol However, at constant volume (as with a bomb calorimeter) te = 0 and so ÎE=%- Submit signme Part 涨 boo F rs F7