Potassium superoxide,KO₂, is often used in oxygen masks (such as those used by firefighters) because KO₂ reacts with CO₂ to release molecular oxygen. Experiments indicate that 2 mol of KO₂ (s) react with each mole of CO2(g).

(a) The products of the reaction are K₂CO₃(s) and O₂(g).Write a balanced equation for the reaction between KO₂(s) and CO₂(g).

(b) Indicate the oxidation number for each atom involved in the reaction in part (a). What elements are being oxidized and reduced?

(c)What mass of KO₂(s) is needed to consume 18.0 g CO₂(g)? What mass of O₂(g) is produced during this reaction?