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Byju's Answer

Standard XII

Chemistry

EMF

Iodine I2 a...

Question

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

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Solution

The reaction having higher reduction potential will be taking place at cathode i.e., reduction and less reduction potential anode
$∴ B r_{2} + 2 I^{⊝} ⟶ 2 B r^{⊝} + I_{2}$
$E_{c e l l} = 0.54$ $V$

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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 .

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 .

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}

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:

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

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

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Iodine (I2) and bromine (Br2) are added to a solution containing iodide (I−) and bromide (Br−) ions. What reaction would occur if the concentration of each species is 1M? The electrode potentials for the reactions are:(i) I2+2e−→2I−,E∘=+0.54V(ii) Br2+2e−→2Br−,E∘=+1.08V

The reaction having higher reduction potential will be taking place at cathode i.e., reduction and less reduction potential anode∴Br2+2I⊝⟶2Br⊝+I2 Ecell=0.54 V

The reaction having higher reduction potential will be taking place at cathode i.e., reduction and less reduction potential anode
$∴ B r_{2} + 2 I^{⊝} ⟶ 2 B r^{⊝} + I_{2}$
$E_{c e l l} = 0.54$ $V$