One of the common commercial bleaching agents is chlorine dioxide gas (ClO₂). It bleaches materials by oxidizing them while ClO₂ itself is reduced. ClO₂ can be prepared by the reaction of chlorine and sodium chlorite:

Cl₂(g) + 2 NaClO₂(s) → 2 ClO₂(g) + 2 NaCl(s)

What is the mass of ClO₂ that can be prepared when 18.6 g of NaClO₂ is allowed to react with 3.00 L of chlorine gas at a pressure of 2.2 atm at 23°C?