Standard electrode potentials of Zn and Fe ar | vedclass

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(B) The standard electrode potential of $Zn$ is $-0.76 \ V$ and that of $Fe$ is $-0.44 \ V$. Since the reduction potential of $Zn$ is lower than that

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

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(B) The standard electrode potential of $Zn$ is $-0.76 \ V$ and that of $Fe$ is $-0.44 \ V$. Since the reduction potential of $Zn$ is lower than that of $Fe$,$Zn$ acts as the anode and undergoes oxidation $(Zn \rightarrow Zn^{2+} + 2e^-)$,while $Fe$ acts as the cathode. In galvanization,a layer of $Zn$ is coated on $Fe$. Because $Zn$ is more reactive (lower reduction potential),it acts as a sacrificial anode and gets oxidized instead of $Fe$,thereby preventing the rusting of iron.

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

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