The standard reduction potential of the half cells at 298 K are-Ni2- aq -2e- Nis- Eo - -0-28 VMg2- aq - 2e- Mg s - Eo - - 2-37 VThe standard cell potential for a voltaic cell constructed using the two half reaction is

The standard reduction potential of the half cells are given. E^∘_Ni^2+(aq)/Ni(s)= 0.28 V E^∘_Mg^2+(aq)/Mg(s)= 2.37 V Metal which having higher reduction pot ...

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Standard XII

Chemistry

Gibb's Energy and Nernst Equation

The standard ...

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The standard reduction potential of the half cells at $298 K$ are,
$N i^{2 +} (a q) + 2 e^{-} \to N i (s); E^{o} = - 0.28 V$
$M g^{2 +} (a q) + 2 e^{-} \to M g (s); E^{o} = - 2.37 V$

The standard cell potential for a voltaic cell constructed using the two half reaction is

- 2.65 V

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- 2.09 V

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2.09 V

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+ 2.65

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Solution

The correct option is C $2.09 V$
The standard reduction potential of the half cells are given.
$E_{N i^{2 +} (a q) / N i (s)}^{\circ} = - 0.28 V$
$E_{M g^{2 +} (a q) / M g (s)}^{\circ} = - 2.37 V$

Metal which having higher reduction potential will undergo reduction and metal having lower reduction potential will undergo oxidation.
Thus, Ni electrode will act as cathode and $M g$ electrode will act as anode.

The standard cell potential ( $Δ E^{o}$ ) of a galvanic cell can be calculated by considering the standard reduction potentials of the two half cells $E^{o}$ .
$E_{c e l l}^{\circ} = SRP of substance reduced - SRP of substance oxidised$
(SRP - Standard reduction potential)

$E_{c e l l}^{\circ} = E_{c a t h o d e (r e d)}^{\circ} - E_{a n o d e (r e d)}^{\circ}$

$E_{c e l l}^{\circ} = E_{N i^{2 +} (a q) / N i (s)}^{\circ} - E_{M g^{2 +} (a q) / M g (s)}^{\circ}$

$E_{c e l l}^{\circ} = - 0.28 - (- 2.37)$
$E_{c e l l}^{\circ} = - 0.28 + 2.37$
$E_{c e l l}^{\circ} = 2.09 V$

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Q. The standard reduction potential

E^{o}

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Z n \to Z n^{2 +} + 2 e^{-}; E^{o} = - 0.76 V

F e^{2 +} + 2 e^{-} \to F e; E^{o} = + 0.41 V

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F e^{2 +} + Z n \to Z n^{2 +} + F e

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Q. The standard reduction potentials EO, for the half reaction are as

Z n \to Z n^{+ +} + 2 e^{-}, E^{0} = 0.76 V

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Q. The standard reduction potential of the half cells at

298 K

are,

N i^{2 +} (a q) + 2 e^{-} \to N i (s); E^{o} = - 0.28 V

M g^{2 +} (a q) + 2 e^{-} \to M g (s); E^{o} = - 2.37 V

The standard cell potential for a voltaic cell constructed using the two half reaction is

Q. The standard reduction potentials at 298K for the following half cell reaction are given below:

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C r^{3 +} (a q) + 3 e^{-} ⇌ C r (s); E^{o} = + 0.762 V

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Q. The standard reduction potential

E^{o}

for half reaction are:

Z n \to {Z n}^{2 +} + 2 e^{-}; E^{o} = + 0.76 V

F e \to {F e}^{2 +} + 2 e^{-}; E^{o} = + 0.41 V

The EMF of the cell reaction is:

{F e}^{2 +} + Z n \to {Z n}^{2 +} + F e

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Gibb's Energy and Nernst Equation

Standard XII Chemistry

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The standard reduction potential of the half cells at 298 K are, Ni2+(aq)+2e−→Ni(s);Eo=−0.28 V Mg2+(aq)+2e−→Mg(s);Eo=−2.37 V The standard cell potential for a voltaic cell constructed using the two half reaction is

The standard reduction potential of the half cells at $298 K$ are,
$N i^{2 +} (a q) + 2 e^{-} \to N i (s); E^{o} = - 0.28 V$
$M g^{2 +} (a q) + 2 e^{-} \to M g (s); E^{o} = - 2.37 V$

The standard cell potential for a voltaic cell constructed using the two half reaction is