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2KMnO4+3Na2SO3+H2O→2MnO2+3Na2SO4+2KOH

In a reaction, the reducing agent is the element or compound that donates electron or the one tht loses electrons. The oxidized species. The opposite is called the oxidizing agent. It is the one who accepts the electrons lost. For this reaction KMnO4 is reduced into MnO2.

Answer:

Reducing agent: [tex]Na_2SO_3[/tex]

Explanation:

Reducing species is a chemical species which itself undergoes oxidation and reduces other chemical species in a redox reaction.

[tex]2KMnO_4\ + \ 3Na_2SO_3 + H_2O \rightarrow 2MnO_2 + 3Na_2SO_4+2KOH[/tex]

Oxidation state of each element is:

Before the reaction                                           After the reaction

[tex]KMnO_4[/tex]                                                  [tex]MnO_2[/tex]                        

Oxidation state of K = +1                       Oxidation state of Mn = +4

Oxidation state of Mn = +7                      Oxidation state of O = -2

Oxidation state of O = -2                                      

Before the reaction                                           After the reaction

[tex]Na_2SO_3[/tex]                                     [tex]Na_2SO_4[/tex]                        

Oxidation state of Na = +1                   Oxidation state of Na = +1

Oxidation state of S = +4                      Oxidation state of S = +6

Oxidation state of O = -2                        Oxidation state of O = -2

Only oxidation states of S and Mn are changes during the reaction.

Oxidation of Mn is decreased and oxidation number of S is increased during the reaction. Hence, [tex]Na_2SO_3[/tex] undergoes oxidation, so acts as reducing agent.

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