SO2+KMnO4

SO2 + KMnO4 = SO3 + MnSO4 + K2SO4

This is a reaction in which the oxidation number of the S (Sulpher) and Mn  (Manganese) are changing. Therefore, This reaction is a Redox reaction. Here,  SO2 KMnO4 are the common chemicals in any chemistry research laboratories. In this particular reaction, sulfur dioxide and potassium permanganate are used as an aqueous solution. So they react with each other in the aqueous medium. The K2SO4, SO3, and MnSO4 produce through this reaction. As the reaction is a redox reaction, we can simply use the ion-electron method to balance this reaction. 

About SO2 KMnO4

The SO2 (Sulfur dioxide) is a very well known gas. This gas is soluble in water that means we can make an aqueous solution of SO2. It has a very ode smell as well as very harmful to our health.

The KMnO4 (Potassium Permanganate) is a very well known chemical. It is a chemical with oxidizing properties as well as readily soluble in water.

Sulfur dioxide reacts with potassium permanganate (SO2 + KMnO4)

When Sulfur dioxide reacts with potassium permanganate, it produces sulfur trioxide, manganese sulfate as well as potassium sulfate. In the aqueous medium-

SO2 + KMnO4 = SO3 + MnSO4 + K2SO4

Therefore, by using the ion-electron method we can balance the Oxidation-Reduction reaction.

Balancing the equation

The skeleton reaction for the redox reaction is-

SO2 + KMnO4 = SO3 + MnSO4 + K2SO4

Here,
The Oxidizing agent: KMnO4 or MnO4-1
The Reducing agent: SO2 or, S+4

Reduction Half Reaction:

⇒ Mn+7 +5e  = Mn2+ … …. …. …. (1)

Oxidation Half Reaction:

⇒ S+4 – 2e = S+6 … … … … (2)

Now,

equation (1)x2 + (2)x5,

2Mn+7 +10e = 2Mn+2

5S+4 – 10e = 5S+6 


2Mn+7 + 5S+4 = 2Mn+2 + 5S+6 

⇒ adding necessary ions and radicals we get,

2KMnO4 + 5SO2 = 2MnSO4 + 2SO3 + K2SO4

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Click to readily understand ion-electron balancing redox reaction

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