The solubility product of ${\mathrm{Ag}}_2{\mathrm{CO}}_3$ and ${\mathrm{FeCO}}_3$ in water at $25°\mathrm{C}$ are $4\times {10}^{-12}$ and $2.5\times {10}^{-11}$, respectively. If ${\mathrm{S}}_1$ and ${\mathrm{S}}_2$ are their solubilities in water, respectively when dissolved separately, then ${\mathrm{S}}_1/{\mathrm{S}}_2$ is:

${\mathrm{K}}_{\mathrm{sp}}\left(\mathrm{SnS}\right)={10}^{-25}$
${\mathrm{K}}_{\mathrm{SP}}\left(\mathrm{ZnS}\right)=1.6\times {10}^{-24}$

To a solution containing $0.01{\mathrm{MSn}}^{2+}$ and $0.2{\mathrm{MZn}}^{2+},{\mathrm{S}}^{2-}$ is added gradually. Without changing the volume of solution. Which of the following is correct?

Consider the following reversible reaction at  equilibrium, $2{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{g}\right)}\rightleftharpoons 2{\mathrm{H}}_{2\left(\mathrm{g}\right)}+{\mathrm{O}}_{2\left(\mathrm{g}\right)};\mathrm{\Delta H}=241.7\mathrm{kJ}$

Which one of the following changes in conditions will lead to maximum decomposition of H₂O(g)?