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Electrochemical Series

Select the st...

Question

Select the strongest reducing agent from amongst the substances involved in the following half-reactions.
$C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q) + 1.36 V$
$B r_{2} (g) + 2 e^{-} \to 2 B r^{-} (a q) + 1.09 V$
$S n_{2 +} + 2 e^{-} \to S n - 0.14 V$

A

C l^{-}

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B

B r^{-}

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C

S n

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D

S n^{2 +}

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Solution

The correct option is A $C l^{-}$
The strongest reducing agent should have the lowest reduction potential.
The reduction potential increases in the following order,
${C l}^{-} < {B r}^{-} < {S n}^{2 +} < S n$
Therefore, ${C l}^{-}$ is the strongest reducing agent.

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Similar questions

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 (s)} + 2 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) + 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.

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:

Q. A solution containing equimolar amounts of

N i C l_{2}

S n B r_{2}

is electrolysed using a 9V battery and graphite electrodes. What are the first products formed?
Half reaction

N i^{2 +} (a q) + 2 e^{-} \to N i (s)

Standard reduction potential (V) -0.236
Half reaction

S n^{2 +} (a q) + 2 e^{-} \to S n (s)

Standard reduction potential (V) -0.141

B r_{2} (a q) + 2 e^{-} \to 2 B r^{-} (a q)

Standard reduction potential (V) 1.077
Half reaction

C l_{2} (a q) + 2 e^{-} \to 2 C l^{-} (a q)

Standard reduction potential (V) 1.360

Q. The reaction,

2 B r^{-} (a q) + S n^{2 +} (a q) \to B r_{2} (1) + S n (s)

with the standard potentials,

E_{S n}^{\circ} = - 0.114 V, E_{B r_{2}}^{\circ} = + 1.09 V

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