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Electrochemical Cells, Galvanic Cells

The value of ...

Question

The value of E for elements are as follows:
$F e^{+ 2} + 2 e \to F e; E^{o} = 0.44 V$
$F e^{+ 3} + 1 e \to F e^{+ 2}; E^{o} = + 0.77 V$
$S n^{+ 4} + 2 e \to S n^{+ 2}; E^{o} = + 0.13 V$
$I_{2} + 2 e \to 2 I; E^{o} = + 0.54 V$
$C r^{3 +} + 3 e \to C r; E^{o} = 0.74 V$
Based on the above data correct statements are:

A

Strongest reducing agent is

C r^{3 +}

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B

Strongest oxidising agent is

F e^{3 +}

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C

S n^{+ 4}

can oxidise

I

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D

S n^{+ 3}

can oxidise

I

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Solution

The correct options are
A Strongest oxidising agent is $F e^{3 +}$
D $S n^{+ 3}$ can oxidise $I$
As $F e^{+ 3}$ have highest reduction potential so it is strongest oxidising agent among all.
Also, according to given values $S n^{+ 3}$ can oxidise iodide ion.

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Similar questions

Given: $F e_{(s)} \to F e^{2 +} + 2 e^{-}; E^{o} = + 0.44 V$

$P b_{(s)} \to P b^{2 +} + 2 e^{-}; E^{o} = + 0.13 V$

$A g^{+} e^{-} \to A g; E^{o} = + 0.8 V$

$C u^{2 +} 2 e^{-} \to C u; E^{o} = + 0.34 V$

Which of the following metals will oxidise iron?

a) $A g$

b) $C u$

c) $P b$

d) None of these

Q. The standard reduction potentials at 298K for the following half cell reaction are given below:

Z n^{2 +} (a q) + 2 e^{-} ⇌ Z n (s); E^{o} = - 0.762 V

C r^{3 +} (a q) + 3 e^{-} ⇌ C r (s); E^{o} = + 0.762 V

2 H^{+} (a q) + 2 e^{-} ⇌ H_{2} (g); E^{o} = + 0.00 V

F e^{3 +} (a q) + e^{-} ⇌ F e^{2 +} (a q); E^{o} = + 0.770 V

Based on the above reactions, select the strongest reducing agent?

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. Given standard electrode potentials :

{F e}^{3 +} + {3 e}^{-} ⟶ F e; E^{o} = - 0.036 v o l t

{F e}^{2 +} + {2 e}^{-} ⟶ F e; E^{o} = - 0.440 v o l t

The standard electrode potential

E^{o}

{F e}^{3 +} + e^{-} ⟶ {F e}^{2 +}

Q. Given standerd electrode potentials

F e^{2 +} + 2 e^{-}

⟶

F e; E^{o} = - 0.440 V

F e^{3 +} + 3 e^{-}

⟶

F e; E^{o} = - 0.036 V

The standard electrode potential

(E^{o}

F e^{3 +} + e^{-}

\to

F e^{2 +}

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