1

### AIPMT 2011 Mains

A solution contains Fe2+, Fe3+ and I$-$ ions. This solution was treated with iodine at 35oC. Eo for Fe3+/Fe2+ is + 0.77 V and Eo for I2/2I$-$ = 0.536 V.
The favourable redox reaction is
A
I2 will be reduced to I$-$
B
there will be no redox reaction
C
I$-$ will be oxidised to I2
D
Fe2+ will be oxidised to Fe3+

## Explanation

Since the reduction potential of Fe3+/Fe2+ is greater than that of I2 /I , Fe3+ will be reduced and I will be oxidised.

2Fe3+ + 2I $\to$ 2Fe2+ + I2
2

### AIPMT 2011 Prelims

The electrode potentials for Cu2+(aq) + e$-$ $\to$ Cu+(aq)
and Cu+(aq) + e$-$ $\to$ Cu(s) are + 0.15 V and + 0.50 V respectively.

The value of Eocu2+/cu will be
A
0.500 V
B
0.325 V
C
0.650 V
D
0.150 V

## Explanation

Cu2+(aq) + e$-$ $\to$ Cu+(aq) ; E1o = 0.15 V

Cu+(aq) + e$-$ $\to$ Cu(s) ; E2o = 0.50 V

Cu2+ + 2e $\to$ Cu ; Eo = ?

$\Delta$Go = $\Delta$G1° + $\Delta$G2°

$\Rightarrow$ – nFE° = – n1FE1° – n2FE2°

$\Rightarrow$ Eo = ${{1 \times 0.15 + 1 \times 0.50} \over 2}$ = 0.325 V
3

### AIPMT 2011 Prelims

Standard electrode potential for Sn4+/Sn2+ couple is + 0.15 V and that for the Cr3+/Cr couple is $-$ 0.74 V. These two couples in their standard state are connected to make a cell. The cell potential will be
A
+ 1.19 V
B
+ 0.89 V
C
+ 0.18 V
D
+ 1.83 V

## Explanation

Sn4+/Sn2+ = 0.15 V

Cr3+/Cr = –0.74 V

cell = E°cathode – E°anode

= 0.15 – (– 0.74) = 0.15 + 0.74 = 0.89 V
4

### AIPMT 2011 Prelims

Standard electrode potential of three metals X, Y and Z are $-$1.2 V, + 0.5 V and $-$ 3.0 V respectively. The reducing power of these metals will be
A
Y > Z > X
B
Y > X > Z
C
Z > X > Y
D
X > Y > Z

## Explanation

As the electrode potential drops, reducing power increases.

So, Z (–3.0 V) > X (–1.2 V) > Y (+ 0.5 V)