1. The problem statement, all variables and given/known data When 1.00g of ethanol was burned under a container of water, it was found that 100g of water was heated from, 15°C to 65°C, The process was known to be only 70% efficient. Calculate the enthalpy change of combustion of ethanol taking specific heat capacity of water to be 4.18 J g^-1 k^-1. 2. Relevant equations q= mc ΔT; ΔHr= - q/ moles of limiting reagent. 3. The attempt at a solution I calculate q = 100 x 4.18 x 50 x(70/100) = 14630J. Then I found the number of moles of ethanol which is 1/46 = 0.0217 Therefore enthalpy change will then be -14630/0.0217 = -672980J = -673 kJ mol^-1 but the answer given is -1.37 x 10^3 kJ mol^-1. Where did I go wrong??