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Consider the cell reaction : Mg(s)+Cu^...

Consider the cell reaction `:`
`Mg(s)+Cu^(2+)(aq) rarr Cu(s) +Mg^(2+)(aq)`
If `E^(c-)._(Mg^(2+)|Mg(s))` and `E^(c-)._(Cu^(2+)|Cu(s))` are `-2.37` and `0.34V`, respectively. `E^(c-)._(cell)` is

A

`-2.71V`

B

`2.71V`

C

`-2.03V`

D

`2.03V`

Text Solution

Verified by Experts

The correct Answer is:
B
Cell reaction is
`Mg(s)+Cu^(2)+(aq)rarrCu(s)+Mg^(2+)(aq)`
Half reaction at LHE , i.e., oxidation
`MghArrMg^(2+)+2e^(-)`
Half reaction at LHE, i.e., Reduction
`Cu^(2+)(aq)+2e^(-)hArrCu(s)`
Now, `E_(LHE)^(@)=E_(Mg^(2+//Mg))^(@)=-237V`
`E_(RHE)^(@)=E_(Cu^(2+)//Cu)^(@)=+0.34V`
`therefore E_( "cell")^(@)=E_(RHE)^(@)-E_(LHE)^(@)`
`=0.34-(-2.37)=2.71V`
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