(a) All ion concentrations are 1.0 M, so E° values may be used. E°cell= Ered - Eox= E°Pt - E°Cr = 0.17 V - (-0.74 V)= +0.91 V
(b) At equilibrium, there is no driving force for the reaction and ΔG reaches zero. Therfore measured potential at equilibrium will be 0 V.
(c) The Cr3+ would be coverted to Cr causing chromium solution to decrease in charge, while the Pt° metal would become Pt+ increasing the charge on SO42-, H+, H2SO3 solution. Unless these charges were balanced by ion flow from or to the salt bridge, electrons would no longer flow away from Chromium solution to the SO42-,H+, H2SO3 solution and the reaction would cease.
(d) I would predict the increase in mass would happen to the mass of Platinum electrode as the reaction proceeded in the spontaneous direction.
(e)Chromium electrode is the anode and Platinum electrode is the cathode.
Are all the above-mentioned my answers to the questions asked correct? Let me know. Thanks for reading and interpreting my answers.