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$CO(g) + H_2O(g) \rightleftharpoons CO_2(g) + H_2(g)$, at a given temperature, the equilibrium amount of $CO_2(g)$ can be increased by
${{C}_{6}}{{H}_{6}}+C{{H}_{3}}CH=C{{H}_{2}}\xrightarrow[heat]{{{H}_{3}}P{{O}_{4}}}A\xrightarrow[2.\,{{H}_{3}}{{O}^{+}},heat]{1.\,{{O}_{2}},heat}B+C$
The products $(B)$ and $(C)$ are
$Fe ^{2+}( aq )+ S ^{2-}( aq ) \rightleftharpoons FeS ( s )$
When equal volumes of $0.06 M Fe ^{2+}( aq )$ and $0.2 M S ^{2-}( aq )$ solutions are mixed, the equilibrium concentration of $Fe ^{2+}$ (aq) is found to be $Y \times 10^{-17} M$. The value of $Y$ is. . . . .
$[Fe(CN)_6]^{4-} \rightarrow [Fe(CN)_6]^{3-} + e^{-1}\, ;$ $ E^o = -0.35\, V$
$Fe^{2+} \rightarrow Fe^{3+} + e^{-1}\ ;$ $E^o = -0.77\, V$