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 KO21s2 react with each mole of CO21g2. (b) Indicate the oxidation number for each atom involved in the reaction in part (a). What elements are being oxidized and reduced?

Key Concepts

Oxidation States

Oxidation states, or oxidation numbers, are a way to keep track of electrons in chemical reactions. They indicate the degree of oxidation of an atom in a compound, helping to identify which atoms are losing or gaining electrons. In the context of the reaction involving KO2 and CO2, determining the oxidation states of potassium, oxygen, and carbon is essential for identifying the elements that are oxidized and reduced.

Redox Reactions

Redox reactions, short for reduction-oxidation reactions, involve the transfer of electrons between two species. In these reactions, one species is oxidized (loses electrons) while another is reduced (gains electrons). Understanding the principles of redox reactions is crucial for analyzing the reaction between KO2 and CO2, as it allows us to determine which elements undergo oxidation and reduction.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the conservation of mass. It involves using balanced chemical equations to determine the proportions of substances involved. In the case of KO2 reacting with CO2, stoichiometry helps to quantify the amounts of each reactant and product, which is important for understanding the overall reaction and its implications in practical applications like oxygen masks.