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

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Identify the chemical reaction: 4 KO_2 + 2 CO_2 \(\rightarrow\) 2 K_2CO_3 + 3 O_2.

Determine the oxidation number of each element in the reactants: K in KO_2 is +1, O in KO_2 is -1/2, C in CO_2 is +4, and O in CO_2 is -2.

Determine the oxidation number of each element in the products: K in K_2CO_3 is +1, C in K_2CO_3 is +4, O in K_2CO_3 is -2, and O_2 is 0.

Compare the oxidation numbers of each element in the reactants and products to identify changes: O in KO_2 changes from -1/2 to 0, indicating oxidation, and O in CO_2 changes from -2 to -2, indicating no change.

Conclude which elements are oxidized and reduced: Oxygen in KO_2 is oxidized, and no element is reduced as there is no decrease in oxidation number.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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.

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Textbook Question

Chlorine dioxide gas 1ClO22 is used as a commercial bleachingagent. It bleaches materials by oxidizing them. In thecourse of these reactions, the ClO2 is itself reduced. (b) Why do you think that ClO2 is reduced so readily?

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Textbook Question

Federal regulations set an upper limit of 50 parts per million (ppm) of NH₃ in the air in a work environment [that is, 50 molecules of NH₃(g) for every million molecules in the air]. Air from a manufacturing operation was drawn through a solution containing 1.00⨉10² mL of 0.0105 M HCl. The NH₃ reacts with HCl according to: NH₃₍aq) + HCl(aq) → NH₄Cl(aq). After drawing air through the acid solution for 10.0 min at a rate of 10.0 L/min, the acid was titrated. The remaining acid needed 13.1 mL of 0.0588 M NaOH to reach the equivalence point. (a) How many grams of NH₃ were drawn into the acid solution?

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