1. The problem statement, all variables and given/known data The Heat of combustion of Ethane is 373 kcal/mole. Assuming that 60% of the heat is useful , how many liters of ethane,, measured at standard temperature and pressure, must be burned to convert 50.0kg of water ar 10.0C to steam at 100.0C? One mole of a gas occupies 22.4 liters at precisely 0C and 1atm. 2. Relevant equations PV=nRT Q=mcΔT 3. The attempt at a solution Qburned=Q heat up =mL + mcΔT 540g/C(50g)+ 50(1cal/gC)(100-10) Q=31500 cal n= Q/heat of combustion(60%) n=0.1407mol PV=nRT V=0.1407mol(8314j/kmolK)(273K)/1atm V=3193680 L The book has it at 315000. Is there something wrong here? I feel like im missing a term or left something out???