To calculate the standard electrode potential for the given redox reaction, we need to determine the individual half-reactions and then combine them.The given standard reduction potentials are:Fe aq + 2e Fe s E = -0.44 VAl aq + 3e Al s E = -1.66 VWe need to reverse the second half-reaction to make it an oxidation reaction:Al s Al aq + 3e E = +1.66 VNow, we need to balance the electrons in both half-reactions. In this case, we need to multiply the first half-reaction by 3 and the second half-reaction by 2 to get 6 electrons in both reactions:3[Fe aq + 2e Fe s ] 3E = 3 -0.44 V 2[Al s Al aq + 3e] 2E = 2 +1.66 V Now, we can add the two balanced half-reactions together:2Al s + 3Fe aq 3Fe s + 2Al aq Finally, we can calculate the standard electrode potential for the overall redox reaction by adding the potentials of the two half-reactions:E cell = E oxidation + E reduction E cell = 2 +1.66 V + 3 -0.44 V E cell = 3.32 V - 1.32 VE cell = 2.00 VSo, the standard electrode potential for the given redox reaction is 2.00 V at 298 K.