2. The standard electrode potential for a half-cell made from iron metal in a solution of iron(II) ions, Fe** (aq), has the value - 0.45 V. (1) Define standard electrode potential. [2] (ii) Explain the significance of the minus sign in -0.45 V. [1] (b) Consider the following table of standard electrode potentials EV -0.45 -0.14 0.00 Fe (aq) + 2e Fe(s) Sn? (aq) + 2e Sn() H(aq) + = H,(8) Su" (aq) +2e=Sn" (aq) Fe (aq) + Fe (aq Ag (aq) + Ag(s) Br, (1)+eBr" (aq) +0.15 +0.77 +0.80 +1.07 From the list above State the species which is the strongest oxidizing agent. [1] (1) Deduce which species can reduce Sn* (aq) to Sn?" (aq) but will not reduce Sn" (aq) to Sn(s) under standard conditions [1] (i) Deduce which species can reduce So" (aq) to Sn (s) under standard conditions. (c) (1) Draw a labelled diagram of a voltaic cell made from an Fe(s) /Fe() half-cell connected to an Ag() / Ag" (aq) half-cell operating under standard conditions In your diagram identify the positive electrode (cathode), the negative electrode (node) and the direction of electron flow in the external circuit 15 (11) Deduce the equation for the chemical reaction occurring when the cell in part (c) (i) is operating under standard conditions and calculate the voltage produced by the cell 22