Question 3 - 3+5+4+4+2+8=26 marks In the 21st century, electric cars belonging to professors of Physics are typically powered by lithium (Li)-ion batteries that employ a chemical reaction to release energy in the form of electricity: PyCo0 Lit + e- Py + LiC002 Here Py represents a polymer that is not changed by the reaction. For this reaction the change in the Gibbs energy is AG = -357 kJ/mol and the enthalpy is AH - 342 kJ/mol under standard conditions at a temperature of T = 298 K. = State any assumptions you make to answer these questions: (a) What is the maximum possible electrical work available from this reaction per mole of Li? (b) How much internal chemical energy is provided per mole of Li to produce the electrical work? (c) Account for the source or sink of energy that arises from the difference between your answers to (a) and (b). (d) How much entropy flows into the environment per mole of Li as a result of this chemical reaction? (e) When the reaction is run in reverse to charge the battery, how much heat per mole of Li must be discharged to the environment to get rid of the excess entropy? (f) In no more than 1 page, compare the available work per mole of Li to that of octane (petrol). From this result, discuss the implications for the proportion of the mass of the vehicle devoted to storing the energy needed for propulsion for electric and petrol vehicles