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Electrochemical Series

Redox reactio...

Question

Redox reactions play a pivotal role in chemistry and biology. The values of standard redox potential $(E^{o})$ of two half-cell reactions decide which way the reaction is expected to proceed. $A$ simple example is a Daniel cell in which zinc goes into solution and copper gets deposited. Given below are a set of half-cell reactions (acidic medium) along with their $E^{o} (V$ with respect to normal hydrogen electrode) values.

$I_{2} + 2 e^{-} \to 2 I^{-}; E^{o} = 0.54$
$C l_{2} + 2 e^{-} \to 2 C l^{-}; E^{o} = 1.36$
$M n^{3 +} + e^{-} \to M n^{2 +}; E^{o} = 1.50$
$F e^{3 +} + e^{-} \to F e^{2 +}; E^{o} = 0.77$
$O_{2} + 4 H^{+} + 4 e^{-} \to 2 H_{2} O; E^{o} = 1.23$

Among the following, identify the correct statement.

A

C

hloride ion is oxidized by

O_{2}

.

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B

F e^{2 +}

is oxidized by iodine.

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C

Iodide ion is oxidized by chlorine.

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D

M n^{2 +}

is oxidized by chlorine.

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Solution

The correct option is A Iodide ion is oxidized by chlorine.
(A) Oxide ion is oxidized by chlorine as the SRP of chlorine is higher than the SRP of oxygen.
(B) Iodide ion is oxidized by $F e^{3 +}$ as the SRP of $F e^{2 +}$ is higher than that of iodine.
(C) Iodide ion is oxidized by chlorine as the SRP of chlorine is higher than that of iodine.
(D) Chloride ion is oxidized by $M n^{3 +}$ as the SRP of $M n^{3 +}$ is higher than that of chlorine.

Option C is correct.

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Similar questions

Q. This question and the following one were a part of a linked comprehension in the (IIT-JEE, 2008) exam.

Redox reactions play a pivotal role in chemistry and biology. The values of standard redox potential

(E_{⊖})

of two half cell reactions decided which way the reaction is expected to proceed. A simple example is a Daniell cell in which zinc goes into solution and copper gets deposited. Given below are a set of half cell reactions (acidic medium) along with their

E_{⊖}

(V with respect to normal hydrogen electrode) values. Using this data, obtain correct explanations for the follwing questions.

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

C l_{2} + 2 e^{-} \to 2 C I_{⊖}; E^{⊖} = 1.36

M n^{3 +} + e^{-} \to M n^{2 +}; E^{⊖} = 1.50

F e^{3 +} + e^{-} \to F e^{2 +}; E^{⊖} = 0.77

O_{2} + 4 H^{⨁} + 4 e^{-} \to 2 H_{2} I; E^{⊖} = 1.23

Among the following, identify the correct statement.

Q. Redox reactions play a pivotal role in chemistry and biology. The values of standard redox potential

(E_{⊖})

of two half cell reactions decided which way the reaction is expected to proceed. A simple example is a Daniell cell in which zinc goes into solution and copper gets deposited. Given below are a set of half cell reactions (acidic medium) along with their

E_{⊖}

(V with respect to normal hydrogen electrode) values. Using this data, obtain correct explanations for the following question

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

C l_{2} + 2 e^{-} \to 2 C l^{⊖}; E^{⊖} = 1.36

M n^{3 +} + e^{-} \to M n^{2 +}; E^{⊖} = 1.50

F e^{3 +} + e^{-} \to F e^{2 +}; E^{⊖} = 0.77

O_{2} + 4 H^{⨁} + 4 e^{-} \to 2 H_{2} O; E^{⊖} = 1.23

F e^{3 +}

M n^{3 +}

is not stable in acid solution because

Redox reactions play a pivotal role in chemistry and biology. The values of standard redox potential $(E_{⊖})$ of two half cell reactions decided which way the reaction is expected to proceed. A simple example is a Daniell cell in which zinc goes into solution and copper gets deposited. Given below are a set of half cell reactions (acidic medium) along with their $E_{⊖}$ (V with respect to normal hydrogen electrode) values. Using this data, obtain correct explanations for the following question
$I_{2} + 2 e^{-} \to 2 I^{⊖}; E^{⊖} = 0.54$
$C l_{2} + 2 e^{-} \to 2 C l^{⊖}; E^{⊖} = 1.36$
$M n^{3 +} + e^{-} \to M n^{2 +}; E^{⊖} = 1.50$
$F e^{3 +} + e^{-} \to F e^{2 +}; E^{⊖} = 0.77$
$O_{2} + 4 H^{⨁} + 4 e^{-} \to 2 H_{2} O; E^{⊖} = 1.23$

While $F e^{3 +}$ is stable, $M n^{3 +}$ is not stable in acid solution because

This question and the following one were a part of a linked comprehension in the (IIT-JEE, 2008) exam.

Redox reactions play a pivotal role in chemistry and biology. The values of standard redox potential $(E_{⊖})$ of two half cell reactions decided which way the reaction is expected to proceed. A simple example is a Daniell cell in which zinc goes into solution and copper gets deposited. Given below are a set of half cell reactions (acidic medium) along with their $E_{⊖}$ (V with respect to normal hydrogen electrode) values. Using this data, obtain correct explanations for the follwing questions.
$I_{2} + 2 e^{-} \to 2 I_{⊖}; E^{⊖} = 0.54$
$C l_{2} + 2 e^{-} \to 2 C I_{⊖}; E^{⊖} = 1.36$
$M n^{3 +} + e^{-} \to M n^{2 +}; E^{⊖} = 1.50$
$F e^{3 +} + e^{-} \to F e^{2 +}; E^{⊖} = 0.77$
$O_{2} + 4 H^{⨁} + 4 e^{-} \to 2 H_{2} I; E^{⊖} = 1.23$

Among the following, identify the correct statement.

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