200. g of liquid phase octane (C8H18) are burned in air at atemperature of 100. degrees Celsius and a pressure of 1.00 atm,forming vapor phase water and carbon dioxide.
a) Write the balanced chemical reaction equation for thisprocess.
b) What is the magnitude of the difference between ΔE and ΔH forone mole of octane going through this process? (Hint: use the valueof R that makes life easiest.)
c) The reaction is in contact with a reservoir of water that isalso at 100 degrees Celsius. If that reservoir absorbs all of theheat released by the reaction (of the 200. g of octane), how manymoles of the water will evaporate? Each mole of C8H18 releases5074.482 kJ of heat when it goes through this process.
Part a I got no problem, but I can't seem to figure out parts band c. Thanks for the help!!
