- ABr2/FeBr3, KMnO4, HNO3/H2SO4
- BKMnO4, Br2/FeBr3, HNO3
- CHNO3, Br2/FeBr3, KMnO4
- DHNO3, KMnO4, Br2/FeBr3
Explanation:

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$Zn^{2+} + 2e^-$ $\longrightarrow$ $Zn (s) ; E^o = -0.76\,V$
$Ca^{2+} + 2e^-$ $\longrightarrow$ $Ca (s) ; E^o = -2.87\,V$
$Mg^{2+} + 2e^-$ $\longrightarrow$ $Mg (s) ; E^o = -2.36\,V$
$Ni^{2+} + 2e^-$ $\longrightarrow$ $Ni (s) ; E^o = -0.25\,V$
The reducing power of the metals increases in the order

$A$. They exhibit high enthalpy of atomization as the d-subshell is full.
$B$. $\mathrm{Zn}$ and $\mathrm{Cd}$ do not show variable oxidation state while $\mathrm{Hg}$ shows $+\mathrm{I}$ and + $II.$
$C$. Compounds of $\mathrm{Zn}, \mathrm{Cd}$ and $\mathrm{Hg}$ are paramagnetic in nature.
$D$. $\mathrm{Zn}, \mathrm{Cd}$ and $\mathrm{Hg}$ are called soft metals.
Choose the most appropriate from the options given below:
$CH_2OH-CHOH-CH_2OH$ $\xrightarrow{{KHS{O_4}/\Delta }}(X)\mathop {\xrightarrow{{{{({C_2}{H_5}O)}_3}Al}}}\limits_\Delta (Y)$
$(Y)$ will be: