Question

Oxygen masks for producing \(\mathrm{O}_{2}\) in emergency situations contain potassium superoxide, \(\mathrm{KO}_{2}\). It reacts with \(\mathrm{CO}_{2}\) and \(\mathrm{H}_{2} \mathrm{O}\) in exhaled air to produce oxygen: $$ 4 \mathrm{KO}_{2}(s)+2 \mathrm{H}_{2} \mathrm{O}(g)+4 \mathrm{CO}_{2}(g) \longrightarrow 4 \mathrm{KHCO}_{3}(s)+3 \mathrm{O}_{2}(g) $$

Short answer

Also, what is the stoichiometry of the reaction? Answer: The reactants in this chemical equation are potassium superoxide (4 moles of KO2), water (2 moles of H2O), and carbon dioxide (4 moles of CO2). The products of the reaction are potassium bicarbonate (4 moles of KHCO3) and oxygen (3 moles of O2). The stoichiometry of this reaction states that for every 4 moles of KO2, 2 moles of H2O, and 4 moles of CO2, the reaction will produce 4 moles of KHCO3 and 3 moles of O2.

Step-by-step solution

Understand the chemical equation

The given balanced chemical equation represents a reaction between potassium superoxide (KO2), carbon dioxide (CO2), and water (H2O) to produce potassium bicarbonate (KHCO3) and oxygen (O2). It is crucial to identify the reactants and products in this equation. Reactants: - 4 moles of potassium superoxide (KO2) - 2 moles of water (H2O) - 4 moles of carbon dioxide (CO2) Products: - 4 moles of potassium bicarbonate (KHCO3) - 3 moles of oxygen (O2)

Analyze the reaction conditions

Ensure to notice the given states of the substances in the reaction: - Potassium superoxide (KO2) is in solid state (s) - Water (H2O) is in gaseous state (g) - Carbon dioxide (CO2) is in gaseous state (g) - Potassium bicarbonate (KHCO3) is in solid state (s) - Oxygen (O2) is in gaseous state (g)

Understand the stoichiometry

Observe the coefficients in the balanced chemical equation, which indicate the stoichiometric amounts, or the ratios between the number of moles of reactants and products: - For every 4 moles of potassium superoxide (KO2), 2 moles of water (H2O) and 4 moles of carbon dioxide (CO2) are needed to produce 4 moles of potassium bicarbonate (KHCO3) and 3 moles of oxygen (O2). This stoichiometry helps to determine how much of each reactant is needed to produce a desired amount of the product. For instance, if you only have 2 moles of KO2, you would need 1 mole of H2O and 2 moles of CO2 to produce 2 moles of KHCO3 and 1.5 moles of O2.

Visualization of the reaction

To help visualize the reaction, you can view it as follows: 4 KO2 (s) + 2 H2O (g) + 4 CO2 (g) → 4 KHCO3 (s) + 3 O2 (g) - Potassium superoxide reacts with water and carbon dioxide. - When the solid KO2 reacts with gaseous H2O and gaseous CO2, it forms solid KHCO3. In this process, gaseous oxygen is released, which can be used for breathing in emergency situations.

Key concepts

Potassium Superoxide

Potassium Superoxide, \(\mathrm{KO}_{2}\), is a fascinating compound, especially due to its unique use in chemical oxygen generators. It stands out because it reacts with the carbon dioxide (CO₂) in exhaled air to produce oxygen (O₂), a process that is highly valuable in confined environments such as submarines, space capsules, and oxygen masks used in emergencies. Potassium superoxide is a bright yellow solid that is sensitive to moisture and must be handled with care.

This compound is part of a group known as metal superoxides, featuring oxygen molecules that have one extra electron, which contributes to their ability to engage in redox reactions. When it comes in contact with water and carbon dioxide, it reacts to release oxygen and form potassium bicarbonate as a byproduct.

The ability of \(\mathrm{KO}_{2}\) to release oxygen efficiently makes it indispensable in terms of providing life-support oxygen in sealed environments. This not only highlights its practicality but also underscores the ingenuity of chemical engineering in optimizing safety equipment.

Stoichiometry

Stoichiometry is a vital concept in chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. This is beautifully illustrated in the reaction involving potassium superoxide (KO₂), water (H₂O), and carbon dioxide (CO₂).

The balanced chemical equation for this reaction is:
\[4 \mathrm{KO}_{2}(s)+2 \mathrm{H}_{2} \mathrm{O}(g)+4 \mathrm{CO}_{2}(g) \longrightarrow 4 \mathrm{KHCO}_{3}(s)+3 \mathrm{O}_{2}(g)\]

In this equation:

• 4 moles of \(\mathrm{KO}_{2}\) are needed.
• 2 moles of \(\mathrm{H}_{2} \mathrm{O}\) are required.
• 4 moles of \(\mathrm{CO}_{2}\) must be present.

These reactants yield 4 moles of potassium bicarbonate and 3 moles of oxygen.

Understanding these molar ratios, or coefficients, allows chemists to calculate how much of each substance is required or produced. This is crucial in practical applications like creating oxygen masks, ensuring the correct amount of each component is included to generate the needed oxygen under emergency conditions. An example of stoichiometry in action: if you have 1 mole of \(\mathrm{KO}_{2}\), you could determine you need 0.5 moles of water and carbon dioxide each to form 1 mole of potassium bicarbonate and 0.75 moles of oxygen.

Oxygen Generation

Oxygen Generation through chemical reactions is a clever and crucial process. In emergency scenarios or sealed environments, such as submarines or space stations, generating a continuous supply of oxygen can be life-saving. This is effectively achieved by using compounds like potassium superoxide, \(\mathrm{KO}_{2}\).

When \(\mathrm{KO}_{2}\) reacts with \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{CO}_{2}\), it produces \(\mathrm{O}_{2}\), which is necessary for breathing. The process not only adds oxygen to the atmosphere but also removes carbon dioxide, making it doubly effective.

Using the balanced reaction:
\[4 \mathrm{KO}_{2}(s)+2 \mathrm{H}_{2} \mathrm{O}(g)+4 \mathrm{CO}_{2}(g) \longrightarrow 4 \mathrm{KHCO}_{3}(s)+3 \mathrm{O}_{2}(g)\]

This reaction cleans the air by converting accumulated carbon dioxide into solid potassium bicarbonate and simultaneously replenishes it with breathable oxygen. This dual action is particularly beneficial in emergency equipment such as oxygen masks and represents a powerful chemical solution to real-world challenges.