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Ionization Enthalpy

10. Calculate...

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10. Calculate half cell potential at 298k for the reaction Zn\pm +2 ===Zn if [Zn]=2M, Enot Zn\pm /Zn = -0.76V

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Similar questions

Q. Calculate the half-cell potential at

298 K

for the reaction,

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

[Z n^{2 +}] = 0.1 M

E^{\circ} = - 0.76 v o l t

.

Q. Reduction potential for the following half/cell reaction are

Z n \to Z n^{2 +} + 2 e^{-} (E_{(Z n^{2 +} / Z n)}^{0} = - 0.76 V)

F e \to F e^{2 +} + 2 e^{-} E^{0} = 0.41 V

The EMF for the cell reaction

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

Q. The standard reduction potential

E^{o}

for the half reactions are as

Z n ⟶ {Z n}^{2 +} + 2 e^{-}

E^{o} = + 0.76 V

F e ⟶ {F e}^{2 +} + 2 e^{-}

E^{o} = + 0.41 V

The emf for cell reaction,

{F e}^{2 +} + Z n ⟶ {Z n}^{2 +} + F e

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

Q. Calculate using Nernst equation cell potential of the following electrochemical cell at

298 K

.

Z n (s) | Z n_{(e q)}^{2 +} (0.04 M) | | S n_{(e q)}^{2 +} | S n_{(s)} (0.03 M)

E^{\circ} = - 0.76 V, E^{\circ} = - 0.14 V)

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Ionization Enthalpy

Standard X Chemistry