- A$\left[ Ni \left( NH _3\right)_6\right]^{2+}$
- ✓$Ni ( CO )_4$
- C$\left[ Ni ( CN )_4\right]^{2-}$
- D$\left[ P ( CN )_4\right]^{2-}$
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$1.$ $P$ and $Q$, respectively, are the sodium salts of
$(A)$ hypochlorus and chloric acids
$(B)$ hypochlorus and chlorus acids
$(C)$ chloric and perchloric acids
$(D)$ chloric and hypochlorus acids
$2.$ $R , S$ and $T$, respectively, are
$(A)$ $SO _2 Cl _2, PCl _5$ and $H _3 PO _4$
$(B)$ $SO _2 Cl _2, PCl _3$ and $H _3 PO _3$
$(C)$ $SOCl _2, PCl _3$ and $H _3 PO _2$
$(D)$ $SOCl _2, PCl _5$ and $H _3 PO _4$
Give the answer question $1$ and $2.$
Maleic anhydride can be prepared by :
$[ R =$ gas constant, $F =$ Faraday constant, $T =$ Temperature $]$
$(A)$ For the reaction, $M (s)+2 H ^{+}(a q) \rightarrow H _2(g)+ M ^{2+}(a q)$, if $\frac{ dE _{c o l l}}{ dT }=\frac{ R }{ F }$, then the entropy change of the reaction is $R$ (assume that entropy and internal energy changes are temperature independent).
$(B)$ The cell reaction, $Pt (s) \mid H _2(g, 1$ bar $)\left| H ^{+}(a q, 0.01 M ) \| H ^{+}(a q, 0.1 M )\right| H _2(g, 1 bar ) \mid Pt (s)$, is an entropy driven process.
$(C)$ For racemization of an optically active compound, $\Delta S >0$.
$(D)$ $\Delta S >0$, for $\left[ Ni \left( H _2 O \right)_6\right]^{2+}+3$ en $\rightarrow\left[ Ni ( en )_3\right]^{2+}+6 H _2 O$ (where en $=$ ethylenediamine).