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Standard XII

Chemistry

Representation of Cell

The standard ...

Question

The standard electrode potentials $E_{I_{2} / I^{-}}^{\circ}, E_{B r^{-} / B r_{2}}^{\circ} and E_{F e / F e^{2 +}}^{\circ}$ are respectively $+ 0.54 V$ , $- 1.09 V$ and $0.44 V$ .
On the basis of the above data which of the following process is nonspontaneous?

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

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

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

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

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Solution

The correct option is D $I_{2} + 2 B r^{-} \to 2 I^{-} + B r_{2}$
$B r_{2} + 2 I^{_{-}} ⟶ 2 B r^{-} + I_{2}$
$E_{c e l l} = E_{B r_{2} / B r^{-}} - E_{I_{2} / I^{-}} = 1.36$ $V$ spontaneous
$F e + B r_{2} ⟶ F e^{2 +} + 2 B r^{-}$
$E_{c e l l} = E_{B r_{2} / B r^{-}} - E_{F e / F e^{2 +}} = 0.65$ $V$ spontaneous
$F e + I_{2} ⟶ F e^{2 +} + 2 I^{-}$
$E_{c e l l} = E_{I_{2} / I^{-}} - E_{F e / F e^{2 +}} = 0.1$ $V$ spontaneous
$I_{2} + 2 B r^{-} ⟶ 2 I^{-} + B r_{2}$
$E_{c e l l} = E_{I_{2} / I^{-}} - E_{B r_{2} / B r^{-}} = - 1.36$ $V$ Non- spontaneous

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Similar questions

Q. 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:

Q. 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 .

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. 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 .

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. Iodine

(I_{2})

and bromine

(B r_{2})

are added to a solution containing iodide

(I^{-})

and bromide

(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

(ii)

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

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The standard electrode potentials E∘I2/I−,E∘Br−/Br2andE∘Fe/Fe2+ are respectively +0.54V, −1.09V and 0.44V. On the basis of the above data which of the following process is nonspontaneous?

The standard electrode potentials $E_{I_{2} / I^{-}}^{\circ}, E_{B r^{-} / B r_{2}}^{\circ} and E_{F e / F e^{2 +}}^{\circ}$ are respectively $+ 0.54 V$ , $- 1.09 V$ and $0.44 V$ .
On the basis of the above data which of the following process is nonspontaneous?