$Cr _{2} O _{7}^{2-}+14 H ^{+}+6 e ^{-} \rightarrow 2 Cr ^{3+}+7 H _{2} O$
The amount of $Cr ^{3+}$ obtained was $0.104\, g$. The
efficiency of the process(in\%) is
(Take : $F =96000\, C$, At. mass of chromium $=52$ )
Using stoichiometry; theoritically
$\frac{ n _{ e ^{\ominus}} used }{6}=$$\frac{ n _{ cr ^{+3}} \text {produced }}{2}$
$\Rightarrow n _{ cr ^{+3}}$ produced $=\frac{2}{6} \times \frac{8 \times 60 \times 2}{96000}$
$=\frac{0.02}{6}$
$\Rightarrow wt _{ cr ^{+3}}$ theoritically produced
$=\left(\frac{0.02}{6} \times 52\right) g$
$\Rightarrow \%$ efficiency $=\frac{0.104 g }{\left(\frac{0.02 \times 52}{6}\right) g } \times 100$
$=60 \%$
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$2$. $XeF_2 \xrightarrow{H_2O} $
$3$. $XeF_4 \xrightarrow{H_2O} $
$4$. $PbO_2 \xrightarrow{\Delta } $
$5$. $XeF_6 \xrightarrow{H_2O} $
In how many of the above processes, $O_2$ will be one of the products
Reason : Alcohols leading to conjugated alkenes are dehydrated to a greater extent
$CHC{l_3}\,\xrightarrow[{Zn/HCl\,\,(alc.)}]{{ +\, 2H}}$
$CHC{l_3}\,\xrightarrow[{Zn/HCl\,\,(aq)}]{{ + \,4H}}$
$CHC{l_3}\,\xrightarrow[{Zn/{H_2}O}]{{ + \,6H}}$