Home
Class 12
CHEMISTRY
The voltage of a cell whose half-cells a...

The voltage of a cell whose half-cells are given below is
`Mg^(2+)+2e^(-)rarrMg(s),E^(@)=-2.37V`
`Cu^(2+)+2e^(-)rarrCu(s),E^(@)=+0.34V`
standard EMF of the cell is

A

`-2.03`V

B

1.36 V

C

2.71 V

D

2.03 V

Text Solution

Verified by Experts

The correct Answer is:
C
`E_("cell")^(@) = E_("cathode")^(@) - E_("anode")^(@) = +0.34 -(-2.37) = +2.71 V`
Promotional Banner

Similar Questions

Explore conceptually related problems

Cu-2e^(-)rarrCu^(2+),E^(@)=-0.347V Sn-2e^(-)rarrSn^(2+),E^(@)=+0.143V The standard EMF of the cell constructed with these electrodes is

If for the half cell reaction E^(@) value are given Cu^(2+)+e^(-)rarrCu^(+),E^(@)=0.15V Cu^(2+)+2e^(-)rarrCu^(+),E^(@)=0.34V calculate E^(@) of the half cell reaction Cu^(+)+e^(-)rarrCu

The standard electrode potentials of the two half cells are given below: Ni^(2+)+2e rarr Ni(s),E^(o) = - 0.25V, Zn^(2+) + 2e rarr Zn(s) , E^(o) = - 0.77 V. The voltage of the final cell formed by combining the two half cells would be:

Consider a voltaic cell based on these half - cell reactions Ag^(+)(aq)+e^(-)rarrAg(s): E^(@)=+0.80V Cd^(+2)(aq)+2e^(-)rarrCd(s), E^(@)=-0.40V identify the anode and give the voltage of this cell under standard condition.

E^@ values for the half cell reactions are given below : Cu^(2+) + e^(-) to Cu^(+) , E^@ =0.15 V Cu^(2+) + 2e^(-) to Cu, E^@ =0.34 V What will be the E^@ of the half-cell : Cu^(+) + e^(-) to Cu ?

The standard potential E^(@) for the half reactions are as : Zn rarr Zn^(2+) + 2e^(-), E^(@) = 0.76V Cu rarr Cu^(2+) +2e^(-) , E^(@) = -0.34 V The standard cell voltage for the cell reaction is ? Zn +Cu^(2) rarr Zn ^(2+) +Cu