(NO2):N2O4(g)2NO2(g). For this this equilibrium, rH= 58.02kJ(molN2O4)1 and 55=176.1JK1(molN2O4)1 and are assumed to be constant with temperature. (i) Write a DIMENSIONLESS equation for the equilibrium (3 marks) constant K of this reaction. Assume the mixture behaves ideally. (ii) Determine the standard Gibbs energy for the reaction at (2 marks) 298.15K. (iii) Calculate the equilibrium constant at 298.15K. (2 marks) (iv) Name which species will predominate at 298.15K. (1 mark) (v) Calculate the temperature at which neither species will (2 marks) predominate. Atmospheric corrosion of steel involves gaseous oxygen dissolved in an aqueous environment present on the metal surface. The process includes two coupled redox reactions, Reactions A and B, that occur at different surface sites, forming an electrochemical cell: B: 2H2O(t)+O2(aq)+4e4OH(aq)EB=+0.40V (i) Write out the electrochemical cell for this atmospheric (2 marks) corrosion process using standard notation. Include all electrodes, phase boundaries and co-solutes