Question

2mno4 + 5so2 + 2h2o = 2mn +5so4 +4h

Answer 1

Answer:

Answer:

2MnO4^- + 5SO2 + 2H2O = 5SO4^2- + 2Mn^2+ +4H^+ In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent.

Answer 2

• The chemical equation shown describes an oxidation-reduction reaction in which the reactants go through both processes. 2MnO4, 5SO2, and 2H2O are the reactants on the left side of the equation, whereas 2Mn, 5SO2, and 4H are the products.

• MnO4 functions as an oxidising and SO2 as a reducing agent in this reaction. The SO2 is oxidised to SO4, while the MnO4 is reduced to Mn. Water molecules are created when oxygen atoms from the MnO4 react with hydrogen atoms from the H2O molecules.

• The balanced equation implies that for every two moles of MnO4, five moles of SO2, and two moles of H2O, two moles of Mn, five moles of SO4, and four moles of H are created. As each element has the equal amount of atoms on both sides of the equation, the equation is balanced.

• In the laboratory and in industrial operations, where it is employed to create sulfuric acid and manganese dioxide, this chemical equation represents a valuable reaction.

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