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(Solved): 4.000 g of Compound with molecular formula C4Hg are burned in a constant-pressure calorimeter cont ...
4.000 g of Compound with molecular formula C4Hg are burned in a constant-pressure calorimeter containing 50.00 kg of water at 25 °C. The temperature of the water is observed to rise by 0.8603 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. kJ mol 010 3 x ? x10 ?
Expert Answer
Heat gained by water , Qwater = m * s * ?T => Qwater = 50.00kg * 4.184kJ/kgoC * 0.8603oC => Qwater = 179.975 kJ Thus, Heat of reaction, ?Hrxn = -179.975 kJ Mola