this problem is quite long, all im asking is some for some help by clarifying and hints so i can try to solve this question. Thanks in advance! Consider the combustion of liquid ethanol, C2H5OH(l), to form CO2(g) and H2O(g). Suppose we have 1 mole of ethanol in the presence of 4 moles of O2 gas in balloon at a temperature of T = 298K and a pressure of 1 atm (i.e., pi = pext = 1atm). The ethanol combusts to completion, and assume we can neglect any changes in volume due to the liquid ethanol. All of the gases can be treated as ideal gases. a) If the combustion takes place such that the internal temperature of the gas remains constant, and the external pressuredoesn’t change, calculate ΔH, ΔE, q, w (hint: even though ΔT = 0, ΔE and ΔH are nonzero since the chemical energy and number of moles of gas have changed). b) Suppose instead that the balloon’s volume was fixed, and that that the balloon could not exchange heat with the surroundings (i.e., q = 0). Instead, the heat from combustion was used to only increase the temperature of the gases in the balloon. Question: what is ΔE, ΔH, w, and ΔT. What is the final temperature? What’s the final pressure? Hint: remember that ΔH = Ef + pfVf- ΔEi -ΔpiVi. c) Now suppose instead that the balloon was thermally isolated from the environment (i:e:; q = 0) and the balloon was allowed to expand the volume of the balloon against a constant pressure of 1 atm. What is the final temperature and volume of the balloon? What is ΔE, ΔH, w, and ΔT?