- ✓$CrO_2Cl_2$ and $MnO_4^-$
- B$MnO_2$
- C$[Fe(CN)_6)]^{3-}$ and $[Co(CN)_6]^{3-}$
- D$MnO$
$Ni ( CO )_4 \Rightarrow 28+4 \times 2=36$
$(i)$ $V ( CO )_6 \Rightarrow 23+2 \times 6=35$
$(ii)$ $Cr ( CO )_5 \Rightarrow 24+2 \times 5=34$
$(iii)$ $Cu ( CO )_3 \Rightarrow 29+2 \times 3=35$
$(iv)$ $Mn ( CO )_5 \Rightarrow 25+2 \times 5=35$
$(v)$ $Fe ( CO )_5 \Rightarrow 26+2 \times 5=36$
$(vi)$ $\left[ Co ( CO )_3\right]^{3-} \Rightarrow 27+3+2 \times 3=36$
$(vii)$ $\left[ Cr ( CO )_4\right]^{4-} \Rightarrow 24+4+2 \times 4=36$
$(viii)$ $\left[\operatorname{Ir}( CO )_3\right] \Rightarrow 77+2 \times 3=83$
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$X\xrightarrow[{(2)\,\,drydistillation}]{{(1)\,Ca{{(OH)}_2}}}Y$
$Y$ is


$'B'$ is
$\frac{2}{3} Al_2 O_3 \rightarrow \frac{4}{3} Al + O_2$
$\Delta _rG = + 960\, kJ\, mol^{-1}$
The potential difference needed for the electrolytic reduction of aluminium oxide $(Al_2O_3)$ at $500^oC$ is at least ........ $V$.