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Standard electrode potential of Zn and F...

Standard electrode potential of Zn and Fe are known to be (i) -0.76V and (ii) -0.44V respectively. How does it explain that galvanization prevents rusting of iron while zinc slowly dissolves away

A

Since (i) is less than (ii), zinc becomes the cathode and iron the anode

B

Since (i) is less than (ii), zinc becomes the anode and iron the cathode

C

Since (i) is more than (ii), zinc becomes the anode and iron the cathode

D

Since (i) is more than (ii), zinc becomes the cathode and iron the anode

Text Solution

Verified by Experts

The correct Answer is:
B
`E_(Zn^(2+)//Zn)^(@) = -0.76V`
`E_(Fe^(2+)//Fe)^(@) = -0.44V`
`E_(Zn^(2+)//Zn)^(@) lt E_(Fe^(2+)//Fe)^(@)`
Hence reduction will happen for iron and Zn will oxidize. So Zn is anode and Fe is cathode.
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