Find Delta H for the Combustion of Ethanol?

Find ΔH for the combustion of ethanol (C2H6O) to carbon dioxide and liquid water from the following data. The heat capacity of the bomb calorimeter is 34.65 kJ/K and the combustion of 1.766 g of ethanol raises the temperature of the calorimeter from 294.95 K to 296.46 K.


Any help would be very appreciated, thanks :)

Find DeltaT by subtracting the two temperature. Then find the amount of heat added to the calorimeter knowing that each K rise in temperature requires 34.65 kJ. So you want 34.65 x Delta T.

Then you know that 1.776g ethanol releases this amount of heat. Find the heat released by 1 mole of ethanol (approx 46g)