- A$[Fe(CO)_5]$
- B$[Cr(CN)_6]^{-3}$
- ✓$[Mn_2(CO)_{10}]$
- D$[Fe(CN)_6]^{-4}$
$\mathrm{m}-2=0$
$\mathrm{m}=+2$
$\left(\mathrm{NH}_{3}\right)_{2} \Rightarrow$ Diammine
$\mathrm{Cl} \Rightarrow$ Chlorido.
$\mathrm{NO}_{2} \Rightarrow \mathrm{Nitrito}-\mathrm{N}$
So, IUPAC NAME:
diamminechloridonitrito-N-platinum(II)
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$Mg\left( s \right) + \mathop {2A{g^ + }}\limits_{(0.0001\,M)} \to \mathop {M{g^{ + 2}}}\limits_{\left( {0.100\,M} \right)} + 2Ag\left( s \right)$
If $E_{cell}^o = 3.17\,V$

$\mathrm{Cr}_2 \mathrm{O}_7{ }^{2-}+14 \mathrm{H}^{+}+6 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cr}^{3+}+7 \mathrm{H}_2 \mathrm{O}, \mathrm{E}^{\circ}=1.33 \mathrm{~V}$
$\mathrm{Fe}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightarrow \mathrm{Fe} \mathrm{E}^{\circ}=-0.04 \mathrm{~V}$
$\mathrm{Ni}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightarrow \mathrm{Ni} \mathrm{E}^{\circ}=-0.25 \mathrm{~V}$
$\mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Ag} \mathrm{E}^{\circ}=0.80 \mathrm{~V}$
$\mathrm{Au}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightarrow \mathrm{Au} \mathrm{E}^{\circ}=1.40 \mathrm{~V}$
Consider the given electrochemical reactions, The number of metal$(s)$ which will be oxidized be $\mathrm{Cr}_2 \mathrm{O}_7{ }^{2-}$, in aqueous solution is. . . . . .
$\underset{{{C}_{3}}{{H}_{6}}C{{l}_{2}}}{\mathop{A}}\,\,\xrightarrow[2.\,\,{{H}^{+}}\,\,(\min d)]{\begin{smallmatrix}
1\,.\,\,alcoholic\,\,KOH\,/\,\Delta \\
followed\,\,by\,\,NaN{{H}_{2}}\,/\,\Delta
\end{smallmatrix}}$ $B\,\xrightarrow[{{H}_{2}}{{O}_{2}}/\overset{\Theta }{\mathop{O}}\,H]{{{B}_{2}}{{H}_{6}}}C$
$A\,\xrightarrow{aq.\,\,KOH\,(excess)}C$