Mass of water = volume x density = 22.0 x 1.00 = 22.0 g Mass of solution = mass of water + mass of X = 22.0 + 2.30 = 24.3 g Heat released by reaction = heat absorbed by solution = mass x specific heat x temperature change of solution = 24.3 x 4.18 x (25.5 - 12.0) = 1371.249 J Moles of X = mass/molar mass of X = 2.30/56.0 = 0.04107 mol H = -heat released by reaction/moles of X = -1371.249/0.04107 = -3.34 x 104 J/mol = -33.4 kJ/mol Note that H is negative as reaction is exothermic and heat is released Solution Mass of water = volume x density = 22.0 x 1.00 = 22.0 g Mass of solution = mass of water + mass of X = 22.0 + 2.30 = 24.3 g Heat released by reaction = heat absorbed by solution = mass x specific heat x temperature change of solution = 24.3 x 4.18 x (25.5 - 12.0) = 1371.249 J Moles of X = mass/molar mass of X = 2.30/56.0 = 0.04107 mol H = -heat released by reaction/moles of X = -1371.249/0.04107 = -3.34 x 104 J/mol = -33.4 kJ/mol Note that H is negative as reaction is exothermic and heat is released.