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Redox Reactions

Which of the ...

Question

Which of the following is an example of oxidation?

{S n}^{+ 2} - 2 e^{-} \to {S n}^{+ 4}

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{F e}^{+ 3} + e^{-} \to {F e}^{+ 2}

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{C l}_{2} + 2 e^{-} \to 2 C l^{-}

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None of the above

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Solution

The correct option is B ${S n}^{+ 2} - 2 e^{-} \to {S n}^{+ 4}$
Oxidation is the loss of electrons or an increase in oxidation state by a molecule, atom, or ion.
Therefore, ${S n}^{+ 2} - 2 e^{-} \to {S n}^{+ 4}$ is an example of oxidation.

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Similar questions

F e^{+ 2} + 2 e \to F e; E^{o} = 0.44 V

F e^{+ 3} + 1 e \to F e^{+ 2}; E^{o} = + 0.77 V

S n^{+ 4} + 2 e \to S n^{+ 2}; E^{o} = + 0.13 V

I_{2} + 2 e \to 2 I; E^{o} = + 0.54 V

C r^{3 +} + 3 e \to C r; E^{o} = 0.74 V

F e^{2 +} + 2 e^{-} \to F e (- 0.44 V)

N i^{2 +} + 2 e^{-} \to N i (- 0.25 V)

S n^{2 +} + 2 e^{-} \to S n (- 0.14 V)

F e^{3 +} + e^{-} \to F e^{2 +} (+ 0.77 V)

E^{0}

I_{2} (g) + 2 e^{-} \to 2 I^{-} (a q); E^{0} = + 0.54 V

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

F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{0} = + 0.76 V

C e^{4 +} (a q) + e^{-} \to C e^{3 +} (a q); E^{0} = + 1.60 V

S n^{4 +} (a q) + 2 e^{-} \to S n^{2 +} (a q); E^{0} = + 0.15 V

E^{\circ}

I_{2} + 2 e^{-} \to 2 I^{-}; E^{\circ} = + 0.54 v o l t

C l_{2} + 2 e^{-} \to 2 C l^{-}; E^{\circ} = + 1.36 v o l t

F e^{2 +} + e^{-} \to F e^{2 +}; E^{\circ} = + 0.76 v o l t

C e^{4 +} + e^{-} \to C e^{3 +}; E^{\circ} = + 1.60 v o l t

S n^{4 +} + 2 e^{-} \to S n^{2 +}; E^{\circ} = + 0.15 v o l t

F e^{3 +}

C e^{3 +}

I_{2}

K C l

F e C l_{3}

S n C l_{2}

S n^{4 +} + 2 e^{-} \to S n^{2 +}

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