I was curious as to if you could help me with
a few Thermochemistry P Chem homework problems? I just need help with 4 and 6, please. However, completing 4 does require the answer from Problem 3, but I am almost so sure I completed that one (#3) correctly.
3) 2.3 g of gaseous ethylene oxide is burned at T = 298 K. The heat into the environment is qP;env = +68:2 kJ. Using this result and the data tables in the textbook determine Hof (298 K) of ethylene oxide. Assume that the reaction occurred with all species at partial pressure equal to 1 bar.
4)Use your result from the previous problem and the data tables in the textbook to determine the enthalpy change for oxidation of 1.00 g ethylene to ethylene oxide, at standard state. Compare your value to that for complete combustion of 1.00 g ethylene to CO2(g). Which is more exothermic?
6) Use the average bond energies in Table 4.3 to estimate UoR for the combustion of ethylene gas. Also calculate UoR from the HoR that you computed in Problem 4 noting that for ideal gases H = U + ngasRT. What is the percent error from using average bond energies?