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Introduction to Oxidation and Reduction

An example of...

Question

An example of oxidation-reduction reaction is:

A

B C l_{3} + C l^{-} \to {B C l_{4}}^{-}

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B

H C N + H_{2} O \to H_{3} O^{+} + C N^{-}

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C

H_{2} O_{2} + 2 B r^{-} + 2 H^{+} \to 2 H_{2} O + B r_{2}

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D

2 N H_{3} (g) \to N_{2} (g) + 3 H_{2} (g)

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Solution

The correct option is C $H_{2} O_{2} + 2 B r^{-} + 2 H^{+} \to 2 H_{2} O + B r_{2}$
An oxidation-reduction (redox) reaction is a type of chemical reaction that involves a transfer of electrons between two species. An oxidation-reduction reaction is any chemical reaction in which the oxidation number of a molecule, atom, or ion changes by gaining or losing an electron. Hence option C is correct in which $H_{2} O_{2}$ is reduced in water where as bromine ion is oxidised to $B r_{2}$ .

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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:

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}

Given :

Oxidation :

$H_{2} O_{2} \to O_{2} + 2 H^{\oplus} + 2 e^{-}$

$E^{⊖} = - 0.69 V$ ;

$2 F^{⊖} \to F_{2} + 2 e^{-}$

$E^{⊖} = - 2.87 V$ ;

Reduction :

$H_{2} O_{2} + 2 H^{\oplus} + 2 e^{-} \to 2 H_{2} O$

$E^{⊖} = - 1.77 V$ ;

$2 I^{⊖} \to I_{2} + 2 e^{-}$ $E^{⊖} = - 0.54 V$ ;

Which of the following statements is/are correct ?

For the reaction

$N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)$

Q. The equilibrium constant for the reaction,

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)

k

, then the equilibrium constant for the equilibrium

2 N H_{3} (g) ⇌ N_{2} (g) + 3 H_{2} (g)

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