An Electrochemical Cell has two reactions the oxidation of N2H4 (hydrazine) to N2 and the reduction of O2 to water. The standard electrode potential for the reduction of N2 to N2H4 is -1.155 V, and for O2 to H2O is 0.401 V; these reactions occur under alkaline conditions.

(i) In a practical cell the concentrations of N2H4 and OH are 0.5 M and 1.0 M, respectively, and the pressures of O2 and N2 are 0.2 bar and 0.8 bar respectively, use the Nernst equation to estimate the cell EMF at 298 K, assuming all activity coefficients are unity.

(ii) If one were to generate an electrical current of 2 A in this cell, evaluate the rate of consumption of the hydrazine that is needed to produce this current.