- A${V^{ + 3}}$
- B$M{n^{ + 3}}$
- ✓$F{e^{ + 3}}$
- D$C{u^{ + 2}}$
|
S. No. |
Outer configu-ration |
No. of unpaired $e^-$ |
Colour of ion |
Magnetic moment |
|
${V^{ + 3}}$ |
$3{d^2}$ |
$2$ |
Green |
$2.76$ |
|
$M{n^{ + 3}}$ |
$3{d^4}$ |
$4$ |
Violet |
$1.9$ |
|
$F{e^{ + 3}}$ |
$3{d^5}$ |
$5$ |
Yellow |
$5.96$ |
|
$C{u^{ + 2}}$ |
$3{d^9}$ |
$1$ |
Blue |
$1.9$ |
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$\frac{2}{3} Al_2O_3 \rightarrow \frac{4}{3} Al + O_2,\,$ $\Delta G = +966\,kJ\,mol$
The potential difference needed for electrolytic reduction of $Al_2O_3$ at $500^o C$ is at least ...... $V$.

$X \left| X ^{2+}(0.001 M ) \| Y ^{2+}(0.01 M )\right| Y$
is $.......\times 10^{-2} V$ (Nearest integer).
Given: $E _{ x ^{2+} \mid x }^0=-2.36\,V$
$E _{ Y ^{3+} \mid Y }^0=+0.36\,V$
$\frac{2.303\,RT }{ F }=0.06\,V$
(At. No. $Ti = 22, Cr = 24, Co = 27, Zn = 30$ )
