Introduction:This experiment consists of two parts. In Part A, the rate constant at a particular temperature is determined. Part B is the determination of the activation energy. The bidentate ligand 1,10-phenanthroline (phen), like pyridine and ammonia, is a base and in acid solution it is protonated. The tris-(1,10-phenanthroline_ iron(II) cation is very stable for the reaction:Fe(H2O)6²++ 3phen → Fe(phen)3 ²++ 6H2OIf acid is added to a neutral solution of the ferrous complex, the equilibrium will be disturbed. Therefore, if there is an excess of acid present all of the 1,10-phenanthroline is protonated as the complex dissociates, with an overall reaction:Fe(phen)3²++ 3H++ 6H2O → Fe(H2O)6 ²++ 3 phen H+This first order reaction and its rate is what was investigated in this experiment. The datacollected in Part A and Part B was then used to find the activation energy of the reaction.Purpose:The purpose of this reaction was to determine the rate constant by measuring the rate of dissocation of (Fe(phen)32+) spectrophotometrically and calculate the activation energy from the half-life of the reaction.