A 150g piece of iron (cFe=0.45Jg−1∘C−1) at 180∘C is dropped into 350g of ethylene glycol (cEG=2.4Jg−1∘C−1) that is initially at 25∘C inside an insulated container. Assume no energy is exchanged with the container or the surroundings and that the specific heats remain constant over the temperature range encountered.
(1) Calculate the final equilibrium temperature of the iron–ethylene glycol system. Show all work, including unit analysis.
(2) Determine the quantity of thermal energy (in kJ) transferred between the iron and the ethylene glycol by the time equilibrium is reached.
(3) Discuss how your calculated equilibrium temperature would be affected if the specific heat capacity of ethylene glycol increased with temperature instead of remaining constant. Provide qualitative reasoning without performing additional calculations.