In a direct formic acid fuel cell, formic acid (HCOOH) isoxidised into carbon dioxide and water over an alloy nanoparticlecatalyst. The standard reduction potential for O2 is +1.23 V andfor the reduction of CO2 to HCOOH is -0.25 V. (a) Write downbalanced equations for each half-cell reaction and the overall cellreaction. Calculate the standard potential of the cell. (b) Underoperating conditions, the concentration of HCOOH is 5.0 mol dm-3,and the pressures of O2 and CO2 are 3.4 and 1.9 bar respectively.Assuming ideal behaviour, calculate the operating voltage of thecell at 298 K. (c) If the entropy change for the reaction is +34.2J K-1 mol-1, calculate the operating voltage of the cell at 353 K.Comment on the implications of your answers for the chosenoperating conditions.
