Please answer the following

[16 points] You purchase a new car that runs on 100% ethanol (assume this is possible) and the vehicle gets 16 mpg. How does the annual CO2 emissions compare to a gasoline-powered vehicle that gets 16 mpg? Use 10,500 miles per year for both vehicles. The density of ethanol is 789 kg/m'. a) Determine the molar mass for ethanol: CH,O b) Convert 1.00 gal of ethanol to moles of ethanol using molar mass and density. c) Write out the balanced combustion reaction for etharol. d) Calculate the pounds of CO2 generated from 1 mole of ethanol. (Hint: you need to use the stoichiometry from the balanced equation; Refer to Video #0 as a guide] e) Calculate the emission rate for ethanol in lb CO/gal. (Hint: you can get this answer from parts 'b' and 'd'] f) Calculate the annual number of gallons of ethanol used. g) Calculate that annual CO2 emissions for ethanol in lb CO2. h) Compare the answer in part g to the annual CO2 emissions for the 16 mpg vehicle in question 2. [Hint: "compare' by finding the percent difference)