MCQ
$RCOCl + 2M{e_2}NH \to A + M{e_2}\mathop {N{H_2}C{l^ - }}\limits^{ + \,\,\,\,\,\,\,\,\,\,\,\,\,\,} $ Here $A$ is
- ✓$RCON < \begin{array}{*{20}{c}} {Me} \\ {Me} \end{array}$
- B$RCON{H_2}$
- C$RCONHMe$
- D${(RCO)_2}NH$
$Me=$ Methyl.
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$Fe ^{2+} \rightarrow Fe ^{3+} + e ^{-} \quad E _{ Fe ^{3+} / Fe ^{2+}}=0.77 \,V$
$2 I ^{-} \rightarrow I _{2}+2 e ^{-} \quad E _{ I _{2} / I ^{-}}^{0}=0.54 \,V$
The standard electrode potential for the spontaneous reaction in the cell is $x \times 10^{-2} \,V 298$ $K$. The value of $x$ is .... (Nearest Integer)
A $4.0$ molar aqueous solution of $\mathrm{NaCl}$ is prepared and $500 \mathrm{~mL}$ of this solution is electrolysed. This leads to the evolution of chlorine gas at one of the electrodes (atomic mass: $\mathrm{Na}=23, \mathrm{Hg}=200 ; 1$ Faraday $=96500$ coulombs)
$1.$ The total number of moles of chlorine gas evolved is
$(A)$ $0.5$ $(B)$ $1.0$ $(C)$ $2.0$ $(D)$ $3.0$
$2.$ If the cathode is a $\mathrm{Hg}$ electrode, the maximum weight ( $\mathrm{g}$ ) of amalgam formed from this solution is
$(A)$ $200$ $(B)$ $225$ $(C)$ $400$ $(D)$ $446$
$3.$ The total charge (coulombs) required for complete electrolysis is
$(A)$ $24125$ $(B)$ $48250$ $(C)$ $96500$ $(D)$ $193000$
Give the answer question $1,2$ and $3.$
Set $1$ : $Zn(OH)_2(s)$ and $OH^-(aq)$
Set $2$ : $Zn(OH)_2(s)$ and $H_2O(l)$
Set $3$ : $Zn(OH)_2 (s)$ and $H^+(aq)$
Set $4$ : $Zn(OH)_2(s)$ and $NH_3(aq)$