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The cell reaction of a cell is Mg(s)+C...

The cell reaction of a cell is
`Mg(s)+Cu^(2+)(aq)rarrCu(s)+Mg^(2+)(aq)`
if the standard reduction potential of Mg and Cu are -2.37 V and +0.34 V respectively The emf of the cell is

A

2.03 V

B

`-2.03 V`

C

`+2.71 V`

D

`-2.71 V`

Text Solution

Verified by Experts

The correct Answer is:
C
`Cu^(2+) (aq) to Cu(s)`, Reduction at cathode
`E_(Cu^(2+)//Cu) = +0.34 V`
`Mg(s) to Mg^(2+) (aq)`, Oxidation at anode.
`E_(Mg^(2+) // Mg) = -2.37 V`
`EMF = E_("cathode")^(@) - E_("anode")^(@)`
`=0.34 - (-2.37) = 2.71 V`
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