- A$\ce{Hs}$
- B$\ce{Mt}$
- ✓$\ce{Ds}$
- D$\ce{Sg}$
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$\begin{array}{*{20}{c}}
O \\
{||} \\
{C{H_3} - C{H_2} - C - C{H_2} - C{H_2}}
\end{array}$
$\begin{array}{*{20}{c}}
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,O} \\
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,||} \\
{C{H_3} - C{H_2} - C{H_2} - C - N{H_2}}
\end{array}$


$MnCl _2+ K _2 S _2 O _8+ H _2 O \longrightarrow KMnO _4+ H _2 SO _4+ HCl$ (equation not balanced).
Few drops of concentrated $HCl$ were added to this solution and gently warmed. Further, oxalic acid ( $225 mg$ ) was added in portions till the colour of the permanganate ion disappeared. The quantity of $MnCl _2$ (in $mg$ ) present in the initial solution is. . . . . . . . . (Atomic weights in $g mol ^{-1}: Mn =55, Cl =35.5$ )
| Metal | $Li$ | $Na$ | $K$ | $Mg$ | $Cu$ | $Ag$ | $Fe$ | $Pt$ | $W$ |
| $\phi( eV )$ | $2.4$ | $2.3$ | $2.2$ | $3.7$ | $4.8$ | $4.3$ | $4.7$ | $6.3$ | $4.75$ |
