I've come across an aspect of electrochemical cells that confuse me. From my understanding, if you have two half cells connected by a salt bridge and a wire, at the negative electrode the metal will be oxidised, for example Fe will be oxidised to Fe2+ and 2e-, and the electrons will flow through the wire to the positive half cell. To keep the charges balanced, since there are now more positively charged ions in the negative electrode, the negative ions in the salt bridge (perhaps Mn04-) will move into the negative electrode.
That's my current understanding of how this works, and applying that to this question I found (pictures of the question and mark scheme attached), I'm confused by the answer to part (eii). I thought that the Cl- ions would move into the negative electrode (the Fe2+/Fe half cell) and react with the Fe2+ ions, not go into the positive electrode and react with the Ag+ ions.
I don't know if this misunderstanding of the answer is due to some misconceptions I have, or if there's more to this than what I know, but I'd appreciate any help I could get answering this question. Thanks,