Question #44120

An acidified aqueous solution of $\ce{K2Cr2O7}$ reacts with $\ce{H2O2}$ in the presence of diethyl ether at $273\text{ K}$ to yield a deep blue colored compound $\mathbf{X}$, which is extracted into the organic layer. Consider two other compounds: $\mathbf{Y}$ is sodium tetrathionate ($\ce{Na2S4O6}$) and $\mathbf{Z}$ is tribromooctaoxide ($\ce{Br3O8}$). Let $p$ be the actual oxidation state of the central metal atom in $\mathbf{X}$, $q$ be the number of peroxy linkages ($\ce{-O-O-}$) present in one molecule of $\mathbf{X}$, $r$ be the magnitude of the difference between the highest and lowest formal oxidation states of the sulfur atoms in $\mathbf{Y}$, and $s$ be the average oxidation state of the bromine atoms in $\mathbf{Z}$. Evaluate the expression: $\Omega = (p \times q) + r + 3s$.