Hello, I would need with this task: Write a balanced equation for the oxidation of dissolved H2S to sulfate by dissolved oxygen. Indicate the oxidation states of the redox-sensitive elements involved. - For each redox couple, write the oxidized and reduced species in an equation and balance the amount of element, except H and O. - Balance electroneutrality by adding electrons. - Balance the number of oxygen atoms by adding H2O. - Balance the number of protons (H) by adding H+. - Subtract the two half-reactions, canceling electrons to obtain the complete redox reaction. Sulfide to Sulfate: H2S ->SO4 2- Im not sure which are the redox couples and where to add electrons, but Ive got this so far: H2S + 1/2O2 -> S0 + H2O S0 + 1 1/2O2 + H2O -> SO4 2- + 2H+ Can someone provide his advice or comment if this is correct and how to proceed further? Thanks!