Chapter 5, Problem 161IP

In the presence of nitric acid, UO²⁺ undergoes a redox process. It is converted to UO₂²⁺ and nitric oxide (NO) gas is produced according to the following unbalanced equation:

${\text{H}}^{\text{+}}\left(aq\right)+{\text{ NO}}_{\text{3}}{}^{-}(aq)+{\text{ UO}}^{\text{2+}}(aq)\to \text{ NO}\left(g\right)+{\text{UO}}_{\text{2}}{}^{\text{2 +}}\left(aq\right)+{\text{H}}_{\text{2}}\text{O}\left(l\right)$

If 2.55 × 10² mL NO(g) is isolated at 29°C and 1.5 atm, what amount (moles) of UO²⁺ was used in the reaction? (Hint: Balance the reaction by the oxidation states method.)