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Given the standard electrode potentials:...

Given the standard electrode potentials:
`K^(+)|K=-2.93V`,
`Ag^(+)|Ag=0.80V, " "Hg^(2+)|Hg=0.79V`,
`Mg^(2+)|Mg=-2.37V, " "Cr^(3+)|Cr=-0.74V`
Arrange these metals in their increasing order of reducing power.

Text Solution

Verified by Experts

* The lower the reduction potential, the higher is the reducing power.
The given standard electrode potentials increase in the order of
`(E_(K^(+)|K)^(Theta)=-2.93V) lt (E_(Mg^(2+)|Mg)^(Theta)=-2.37V)lt(E_(Cr^(3+)|Cr)^(Theta)=-0.74V) lt (E_(Hg^(2+)|Hg)^(Theta)=0.79V) lt (E_(Ag^(+)|Ag)^(Theta)=0.80V)`
The metal which has low standard reduction potential will work as strong reducing agent.
* Hence, the reducing power of the given metals increases in the following order:
`Ag lt Hg lt Cr lt Mg lt K`.
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Knowledge Check

  • If given are following standard electrodes potential, then find out standard potential of cell. [Zn^(+2)|Zn=-0.763V,Ag^(+)|Ag=+0.799V] .

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