Question
Asked Nov 22, 2019
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How do I balance the following redox reaction?

O2 + As -> HAsO2 + H2O (condition not specified)

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Expert Answer

Step 1

As “As” oxidation state changes from 0 to +3, it is undergoing oxidation by losing electrons. And oxidation state of “O” changes from 0 to -2; it is undergoing reduction by gaining electrons.

Given reaction:

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02AsHAs02 + H20

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Step 2

As no medium is given, balancing redox reaction in acidic medium.

Balancing reduction half reaction:

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Step-1: For balancing O, add same number of H20 molecules. 0, — Н,о + Н,0 Step-2: For balancing of H, add same number of H ions at deficient side 02+4H2H20 Step-3: To balance charges, add same number of electrons at deficient side. 024H 4e »2H20 Step-4: Multiply the above equation by 3. 30212H + 12e~ -> 6H20

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Step 3

Balancing oxidation h...

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Step-1: Balance As atoms As HAS02 Step-2: For balancing O, add same number of H20 molecules. As 2H20 HAs02 Step-3: For balancing of H, add same number of H ions at deficient side. As 2H20 HAS02 3H Step-4: To balance charges, add same number of electrons at deficient side. As2H20 HAS02 3H+ +3e" Step-5: Multiply the above equation by 4 4HAS02 +12H+ +12e~ 4As8H20

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