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Question

In corrosion of iron,


A
electrons flow from anode to cathode through the metal, while ions flow through the water droplets
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B
an electrochemical (galvanic) cell is formed in which Fe acts as anode and O2 is reduced at cathode
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C
dissolved O2 oxidizes Fe2+ to Fe3+ before it is deposited as rust (Fe2O3.xH2O)
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D
All of the above takes place
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Solution

The correct option is B All of the above takes place
The corrosion of iron is an electrochemical process. The anode region and cathode region are present in iron. $$Iron(II)$$ is oxidized to $$Iron(III)$$ by oxygen and is then converted to rust. At the cathode, oxygen is reduced. The electron flow is from anode to cathode through metal. 
This is accompanied by the flow of ions through water droplets.

Chemistry

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