Calculate [Fe^2]+ when the cell reaction reaches equilibrium?

Question

A voltaic cell is constructed based on the following reaction and initial concentrations:
Fe^2+,( 0.0055 M ) + Ag+,( 2.5 M ) ----> Fe^3+,( 0.0055 M ) + Ag(s)

Calculate [Fe^2]+ when the cell reaction reaches equilibrium

can someone please explain how to do this?

Answer 1

I forgot to mention that forward arrow is suppose to be an equilibrium arrow forward/reverse

Answer 2

First solve K or Q using the Nestern (I think that is how you spell it, if not shh)

then find the change in equilibrium

next use the quadratic equation to solve X and subtract with the concentration you are trying to find [Fe2+]