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

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

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

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

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

Standard electrode potentials of \[Zn\] and \[Fe\] are known to be (i)

1.	Standard electrode potentials of \[Zn\] and \[Fe\] are known to be (i) \[-0.76\,V\] and (ii) \[-0.44\,V\] 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
Answer» C. Since (i) is more than (ii), zinc becomes the anode and iron the cathode

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

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