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Gibb's Free Energy

For I 2+2 e -...

Question

For $I_{2} + 2 e^{-} \to 2 I^{-} standard reduction potential = + 0.54 Volt .$
For $2 B r^{-} \to B r_{2} + 2 e^{-} standard oxidation potential = - 1.09 Volt .$
For $F e \to F e^{2 +} + 2 e^{-}, standard oxidation potential = + 0.44 Volt .$
Which of the following reaction(s) is/are spontaneous:

A

B r_{2} + 2 I^{-} \to 2 B r^{-} + I_{2}

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B

F e + B r_{2} \to F e^{2 +} + 2 B r^{-}

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C

F e + I_{2} \to F e^{2 +} + 2 I^{-}

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D

I_{2} + 2 B r^{-} \to 2 I^{-} + B r_{2}

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Solution

The correct options are
A $B r_{2} + 2 I^{-} \to 2 B r^{-} + I_{2}$
B $F e + B r_{2} \to F e^{2 +} + 2 B r^{-}$
C $F e + I_{2} \to F e^{2 +} + 2 I^{-}$
(a) $B r_{2} + 2 e^{-} \to 2 B r^{-} E_{B r_{2} / B r^{-}}^{o} = 1.09 V$
$2 I^{-} \to I_{2} + 2 e^{-} E_{I^{-} / I_{2}}^{o} = - 0.54 V$
$∴ for B r_{2} + 2 I^{-} \to I_{2} + 2 B r^{-} E^{o} = (1.09 - 0.54) V = 0.55 V$
Hence this is a spontaneous reaction.

(b)
$F e \to F e^{2 +} + 2 e^{-} E_{F e / F e^{2 +}}^{o} = 0.44 V$
$B r_{2} + 2 e^{-} \to 2 B r^{-} E_{B r_{2} / B r^{-}}^{o} = 1.09 V$
$∴ B r_{2} + F e \to F e^{2 +} + 2 B r^{-} E^{o} = (0.44 + 1.09) V = 1.53 V$
So this is also spontaneous

(c)
$F e \to F e^{2 +} + 2 e^{-} E_{F e / F e^{2 +}}^{o} = 0.44 V$
$I_{2} + 2 e^{-} \to 2 I^{-} E_{I_{2} / I^{-}}^{o} = 0.54 V$
$∴ I_{2} + F e \to F e^{2 +} + 2 I^{-} E^{o} = (0.44 + 0.54) V = 0.98 V$
Hence this is also a spontaneous reaction.

(d)
$I_{2} + 2 e^{-} \to 2 I^{-} E_{I_{2} / I^{-}}^{o} = 0.54 V$
$2 B r^{-} \to B r_{2} + 2 e^{-} E_{B r^{-} / B r_{2}}^{o} = - 1.09 V$
$∴ I_{2} + 2 B r^{-} \to B r_{2} + 2 I^{-} E^{o} = (0.54 - 1.09) V = - 0.55 V$
So this reaction is not spontaneous

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Similar questions

I_{2} + 2 e^{-} \to 2 I^{-}, standard reduction potential = + 0.54 Volt .

2 B r^{-} \to B r_{2} + 2 e^{-}, standard oxidation potential = - 1.09 Volt .

F e \to F e^{2 +} + 2 e^{-}, standard oxidation potential = + 0.44 Volt .

Out of the below given reactions, how many reactions are spontaneous in nature (predict from the above data) ?

B r_{2} + 2 I^{-} \to 2 B r^{-} + I_{2}

F e + B r_{2} \to F e^{2 +} + 2 B r^{-}

F e + I_{2} \to F e^{2 +} + 2 I^{-}

I_{2} + 2 B r^{-} \to 2 I^{-} + B r_{2}

I_{2} + 2 e^{-} \to 2 I^{-}, standard reduction potential = + 0.54 Volt .

2 B r^{-} \to B r_{2} + 2 e^{-}, standard oxidation potential = - 1.09 Volt .

F e \to F e^{2 +} + 2 e^{-}, standard oxidation potential = + 0.44 Volt .

Out of the below given reactions, how many reactions are spontaneous in nature (predict from the above data) ?

B r_{2} + 2 I^{-} \to 2 B r^{-} + I_{2}

F e + B r_{2} \to F e^{2 +} + 2 B r^{-}

F e + I_{2} \to F e^{2 +} + 2 I^{-}

I_{2} + 2 B r^{-} \to 2 I^{-} + B r_{2}

Q. Which of the following is the cell reaction that occurs when the following half-cells are combined?

I_{2} + 2 e^{-} \to 2 I^{-} (1 M)

E^{o} = + 0.54

V

B r_{2} + 2 e^{-} \to 2 B r^{-} (1 M); E^{o} = + 1.09

V

Given that : $I_{2} + 2 e^{-} \to 2 I^{-}; E_{I_{2} / I^{-}}^{o}$ = 0.54V; $B r_{2} + 2 e^{-} \to 2 B r^{-}; E_{B r_{2} / B r^{-}}^{o}$ = 1.69V. Predict which of the following is true:

(I_{2})

(B r_{2})

are added to a solution containing iodide

(I^{-})

(B r^{-})

ions. What reaction would occur if the concentration of each species is 1M? The electrode potentials for the reactions are:
(i)

I_{2} + 2 e^{-} \to 2 I^{-}, E^{\circ} = + 0.54 V

B r_{2} + 2 e^{-} \to 2 B r^{-}, E^{\circ} = + 1.08 V

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