a) Write a balanced equation for this reaction. work. Oxidized? How many liters of exhaled air can react with 8.50 g K02, assuming each liter of air contains 0.0520 g C02? g
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
![**Title: Understanding the Role of Potassium Superoxide in Breathing Apparatus**
**Text:**
Potassium superoxide (KO₂) is utilized in self-contained breathing equipment by firefighters. It reacts with carbon dioxide in exhaled air to form potassium carbonate and oxygen gas. Below are the essential components and reactions involved:
**Questions:**
a) **Write a balanced equation for this reaction.**
b) **What is the oxidation number of oxygen in potassium superoxide (KO₂)? Show your work.**
c) **Solve for the oxidation numbers of each element. Which element is being reduced? Oxidized?**
d) **How many liters of exhaled air can react with 8.50 g of KO₂, assuming each liter of air contains 0.0520 g of CO₂?**
**Balanced Equation and Calculation:**
\[ \text{4 KO}_2(s) + 2 \text{CO}_2(g) \rightarrow 2 \text{K}_2\text{CO}_3(s) + 3 \text{O}_2(g) \]
The handwritten notes indicate:
- Starting mass of KO₂: 8.5 g
- Mass of CO₂ in air per liter: 0.0520 g
**Explanation:**
1. **Balanced Equation:** The given reaction shows the process of KO₂ reacting with CO₂ to produce K₂CO₃ and O₂. This is effectively capturing CO₂ and releasing O₂, making it useful for rebreathers.
2. **Oxidation Numbers:**
- Oxygen in KO₂ typically has an unusual oxidation state that needs to be calculated.
- Identifying which elements are oxidized and reduced involves analyzing these oxidation states.
3. **Application in Breathing Apparatus:**
- By reacting with exhaled CO₂, KO₂ supports life in enclosed environments by generating oxygen.
- Understanding the stoichiometry of the reaction is key to determining the efficiency and capacity of the breathing equipment.
This educational exercise combines real-world application with chemical theory, offering insights into both practical and theoretical aspects of chemistry.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F23f54c76-b762-419b-8fbe-ee40e7662c11%2F6fd345ea-efff-4661-8fbf-a004d072d658%2Fpvaot5r_processed.jpeg&w=3840&q=75)
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 3 images
