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Question 9 16 points Save Answer An electrochemical cell is composed of pure iron and pure cadmium electrodes immersed in solutions of their respective divalent ions. The standard potentials for Fe and Cd are -0.440 V and -0.403 V, respectively. (a) If the cell is a standard one (i.e., 1 M solution of both ions at 25 °C), 1> Which electrode (Fe or Cd) will be oxidized? 2> which of the following reactions (A or B) will occur spontaneounsly? (A) Fe+Cd²+ > Fe²+ + Col (B) Fe2+ + Cd -> Fe + Cd2+ 3> Calculate the voltage generated at 25 °C in this standard electrochemical cell. V=Vcathode vº anode= (b) For a 0.2 M concentration of Cd2+, the iron electrode is oxidized yielding a cell potential of 0.05 V. if the temperature is 25*C, For the formula, V=Vº_ 0.0592 n [M+] -log. [M₂+] According to the given information, determine the values of the following variables in the formula. Assume all units are the same as the one given in question. Note: Round to 2 decimal places for the calculated results of Fe2+ concentration. 1>n= 2>V= 3> [M+]= 4> [M₁¹]= -