Chemistry - Redox Reactions Question with Solution | TestHub

Equal volumes of $\mathrm{NO}$ and $\mathrm{N}{\mathrm{O}}_2$ mean equal moles; take 1 mol each. Electrons gained = $1x3$ ($\mathrm{N}{\mathrm{O}}_3^{-}$ $\to$ $\mathrm{NO}$) + $1x1$ ($\mathrm{N}{\mathrm{O}}_3^{-}$ $\to$ $\mathrm{N}{\mathrm{O}}_2$) = 4; each Ag loses only 1 ${\mathrm{e}}^{-}$ (Ag $\to$ $\mathrm{A}{\mathrm{g}}^{+}$), so X = 4. Nitrate used: 2 as oxidant + 4 locked in $4AgN{\mathrm{O}}_3$ = 6, so Y = 6. The balanced equation is 4Ag + $6HN{\mathrm{O}}_3$ $\to$ $4AgN{\mathrm{O}}_3$ + $\mathrm{NO}$ + $\mathrm{N}{\mathrm{O}}_2$ + $3{\mathrm{H}}_2\mathrm{O}$.