In H2SO4, the oxidation state of sulfur S can be determined by considering the oxidation states of hydrogen H and oxygen O . Hydrogen has an oxidation state of +1, and oxygen has an oxidation state of -2. The molecule has a neutral charge, so the sum of the oxidation states must be zero.2 +1 + x + 4 -2 = 02 + x - 8 = 0x = 6So, the oxidation state of sulfur in H2SO4 is +6.When H2SO4 reacts with Fe, the balanced chemical equation for the redox reaction is:H2SO4 + Fe FeSO4 + H2Now, let's determine the oxidation states of the species involved in the reaction:Fe: 0 elemental form S in FeSO4: +6 similar to H2SO4 O in FeSO4: -2H in H2: 0 elemental form Comparing the oxidation states before and after the reaction, we can see that:- Fe goes from an oxidation state of 0 to +2 Fe in FeSO4 , so it is being oxidized.- Sulfur remains at an oxidation state of +6, so it is neither oxidized nor reduced.- Hydrogen goes from an oxidation state of +1 in H2SO4 to 0 in H2 , so it is being reduced.Thus, the redox reaction can be represented as:Fe 0 Fe +2 + 2e- oxidation 2H +1 + 2e- H2 0 reduction In summary, the oxidation state of sulfur in H2SO4 is +6, and it does not change during the reaction with Fe. The balanced chemical equation for the redox reaction is H2SO4 + Fe FeSO4 + H2. In this reaction, Fe is being oxidized, and H is being reduced.