Answer:
To calculate the cell potential of the given cell, we need to use the Nernst equation. The Nernst equation relates the cell potential (Ecell) to the standard cell potential (E°cell), the gas constant (R), the temperature (T), the number of electrons transferred (n), and the concentrations of the reactants and products. The Nernst equation is given as follows: Ecell = E°cell - (RT/nF) * ln(Q) Where: Ecell is the cell potential E°cell is the standard cell potential R is the gas constant (8.314 J/(mol·K)) T is the temperature in Kelvin (298 K in this case) n is the number of electrons transferred in the balanced redox equation F is the Faraday constant (96,485 C/mol) ln(Q) is the natural logarithm of the reaction quotient (Q) In this case, we have a cell composed of a cathode and an anode, both consisting of Fe wires immersed in Fe2+ solutions. The balanced redox equation for the reaction occurring at the cathode is: Fe2+(aq) + 2e- -> Fe(s) And the balanced redox equation for the reaction occurring at the anode is: Fe2+(aq) + 2e- -> Fe(s) Since both half-reactions involve the same reactants and products, the value of n in the Nernst equation will be 2. To calculate the reaction quotient (Q) in the Nernst equation, we need to know the concentrations of the reactants and products. In this case, we are given the concentrations of Fe2+ in both the cathode and anode solutions. Plugging in the given values into the Nernst equation and solving for Ecell will give us the cell potential.
Step-by-step explanation: