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Redox Reactions and Couple

Is the reacti...

Question

Is the reaction, $2 A l + 3 F e^{2 +} ⇌ 2 A l^{3 +} + 2 F e$ possible?

A

No, because standard oxidation potential of

A l < F e

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B

Yes, because standard oxidation potential of

A l > F e

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C

Cannot be predicted

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D

Yes, because aluminium is a strong oxidising agent

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Solution

The correct option is C Yes, because standard oxidation potential of $A l > F e$
Yes, the reaction is possible because the reduction potential of Al is more ( - 1.66 V) than that of Fe (-0.41 V),
so, oxidation of Al and reduction of Fe will takes place.

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Similar questions

Q. Given the standard oxidation potentials:

E_{F e (s) / F e^{2 +} (a q)}^{0} = 0.44 V

E_{F e^{2 +} (a q) / F e^{3 +} (a q)}^{0} = - 0.77 V

The standard EMF of the given reaction will be:

F e (s) + 2 F e^{3 +} (a q) \to 3 F e^{2 +} (a q)

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:

Q. The standard formation reaction for aluminium oxide is

4 A l (s) + 6 O (g) \to 2 A l_{2} O_{3} (s)

. This statement is false because:

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. Aluminium is much more reactive than iron because its standard reduction potential is higher than iron. Still, aluminium is less easily corroded than iron because :

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