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Electrochemical Series

Standard redu...

Question

Standard reduction potentials of the half-reactions are given below:

$F_{2} (g) + 2 e^{-} \to 2 F^{-} (a q) : E^{0} = + 2.85 V$
$C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q) : E^{0} = + 1.36 V$
$B r_{2} (l) + e^{-} \to 2 B r^{-} (a q) : E^{0} = + 1.06 V$
$I_{2} (g) + e^{-} \to 2 I^{-} (a q) : E^{0} = + 0.53 V$

The strongest oxidizing and reducing agent among the given reactions are ____________ respectively.

A

B r_{2}

and

C l^{-}

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B

C l_{2}

and

B r^{-}

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C

C l_{2}

and

I_{2}

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D

F_{2}

and

I^{-}

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Solution

The correct option is A $F_{2}$ and $I^{-}$
An element or a species is said to be a strong oxidising agent if it has large and positive reduction potential. Which means it must easily undergo reduction.

In the data provided the reduction of $F_{2}$ the standard reduction potential $E^{0}$ is the highest i.e $+ 2.85 V$ .

A strong reducing agent has a comparatively lower value for reduction potential and should undergo oxidation easily.

As per these equations, $I^{-}$ has lower value for standard reduction potential $E^{0}$ ie $+ 0.53 V$ .

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Q. Standard reduction potentials of the half reactions are given below:

F_{2 (g)} + 2 e^{-} \to 2 F_{(a q)}^{-}; E^{o} = + 2.85 V

{C l}_{2 (g)} + 2 e^{-} \to 2 {C l}_{(a q)}^{-}; E^{o} = + 1.36 V

{B r}_{2 (l)} + 2 e^{-} \to 2 {B r}_{(a q)}^{-}; E^{o} = + 1.06 V

I_{2 (g)} + e^{-} \to 2 I_{(a q)}^{-}; E^{o} = + 0.53 V

The strongest oxidising and reducing agents respectively are:

Q. Standard reduction potentials of the half reactions are given below

F_{2} (g) + 2 e^{-} \to 2 F^{-} (a q); E^{0} = + 2.85 V

C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q); E^{0} = + 1.36 V

B r_{2} (l) + 2 e^{-} \to 2 B r^{-} (a q); E^{0} = + 1.06 V

I_{2} (s) + 2 e^{-} \to 2 I^{-} (a q); E^{0} = + 0.53 V

The strongest oxidising and reducing agents respectively are:

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. 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

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 .

Which of the following reaction(s) is/are spontaneous:

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