Question below refers to the overall reaction and half-reactions with standard reduction potentials below- 2Fe2- - Cl2 - 2Fe3- - 2Cl- Fe3- - e- - Fe2- Eored - 0-77 volts Cl2 - 2e- - 2Cl- - Eored - 1-36 voltsFind the overall potential for the reaction -

The correct option is B 0.59 volts #160; E^o_rxn = E^o_Cl E^o_Fe = 1.36 0.77=0.59V Hence, the option (B) is the answer.Note: In the redox reaction, ...

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Standard XII

Chemistry

Electrolysis and Electrolytes

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Question below refers to the overall reaction and half-reactions with standard reduction potentials below.
$2 F e^{2 +} + C l_{2} \to 2 F e^{3 +} + 2 C l$ ?
$F e^{3 +} + e^{-} \to F e^{2 +}$ ; $E_{r e d}^{o}$ = 0.77 volts
$C l_{2} + 2 e^{-} \to 2 C l^{-}$ ; $E_{r e d}^{o}$ = 1.36 volts
Find the overall potential for the reaction ?

0.18 v o l t s

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0.59 v o l t s

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1.05 v o l t s

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2.13 v o l t s

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2.90 v o l t s

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Solution

The correct option is B $0.59 v o l t s$
$E_{r x n}^{o} = E_{C l}^{o} - E_{F e}^{o} = 1.36 - 0.77 = 0.59 V$
Hence, the option (B) is the answer.
Note: In the redox reaction, Fe(II) is oxidized. Hence, its potential is subtracted from the potential of chlorine.

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Similar questions

Q. Whats the potential of the reaction below given the half-reaction potentials:

2 F e_{2} + + C l_{2} \to 2 F e^{3 +} + 2 C l^{-}

F e^{3 +} + e^{-} \to F e^{2 +}; E = 0.77 V

C l_{2} + 2 e^{-} \to 2 C l^{-}; E = 1.36 V

Q. Determine the standard reduction potential for the half reaction.

{C l}_{2} + {2 e}^{-} \to {2 C l}^{-}

Given:

{P t}^{2 +} + {2 C l}^{-} \to P t + {C l}_{2}, E_{c e l l} = - 0.15 V

{P t}^{2 +} + {2 e}^{-} \to P t, E = 1.20 V

Q. The standard reduction potential for the half-cell reaction,

C l_{2} + 2 e^{-} \to 2 C l^{-}

if:

P t^{2 +} + 2 C l^{-} \to P t + C l_{2}, E_{cell}^{o} = - 0.15 V

P t^{2 +} + 2 e^{-} \to P t, E^{o} = 1.20 V

Determine the standard reduction potential for the half reaction:

{C l}_{2} + {2 e}^{-} ⟶ 2 {C l}^{-}

Given:

{P t}^{2} + 2 C l ⟶ P t + {C l}_{2}, E_{c e l l}^{0} = - 0.15 V

{P t}^{2} + {2 e}^{-} ⟶ P t, E^{0} = 1.20 V

Q. The standard reduction potential for the half-cell reaction,

C l_{2} + 2 e^{-} \to 2 C l^{-}

will be:

P t^{2 +} + 2 C l^{-} \to P t + C l_{2}, E_{c e l l}^{o} = - 0.15

P t^{2 +} + 2 e^{-} \to P t, E^{o} = 1.20

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Question below refers to the overall reaction and half-reactions with standard reduction potentials below.2Fe2++Cl2→2Fe3++2Cl?Fe3++e−→Fe2+; Eored = 0.77 voltsCl2+2e−→2Cl− ; Eored = 1.36 voltsFind the overall potential for the reaction ?

The correct option is B 0.59volts Eorxn=EoCl−EoFe=1.36−0.77=0.59VHence, the option (B) is the answer.Note: In the redox reaction, Fe(II) is oxidized. Hence, its potential is subtracted from the potential of chlorine.

The correct option is B $0.59 v o l t s$
$E_{r x n}^{o} = E_{C l}^{o} - E_{F e}^{o} = 1.36 - 0.77 = 0.59 V$
Hence, the option (B) is the answer.
Note: In the redox reaction, Fe(II) is oxidized. Hence, its potential is subtracted from the potential of chlorine.