Chapter 10: Problem 72
Helium is mixed with oxygen gas for deep-sea divers. Calculate the percent by volume of oxygen gas in the mixture if the diver has to submerge to a depth where the total pressure is \(5.2 \mathrm{~atm}\). The partial pressure of oxygen is maintained at \(0.20 \mathrm{~atm}\) at this depth.
Short Answer
Expert verified
The percent by volume of oxygen is approximately 3.85%.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Partial Pressure: Essential Understanding
In the world of gases, the term "partial pressure" refers to the pressure exerted by a single type of gas within a mixture of gases. Imagine each gas in the mixture behaving as if it occupies the entire volume on its own. Dalton's Law of Partial Pressures shines a light on this concept. It's a fundamental principle which states that the total pressure of a mixture is simply the sum of the partial pressures of its individual gases.
For example, if you have a total pressure of 5.2 atm in a gas mixture and know that oxygen contributes a partial pressure of 0.20 atm, then the rest of the gases must together contribute 5.0 atm to maintain this total. This principle is essential in calculating gas behaviors in various scientific and practical scenarios, such as medical oxygen delivery systems and deep-sea diving.
Understanding partial pressures can significantly help when dealing with many real-life applications involving gases. These considerations ensure that safety and effectiveness are prioritized, especially in critical situations.
Gas Mixtures: Safe and Scientific
A gas mixture is simply a combination of two or more gases. Each gas contributes individually to the collective properties of the mixture, such as its pressure, volume, and temperature. Gaseous interactions are often predictable due to established laws like Dalton’s Law, making it easier to manage specific requirements.
In practical applications, such as with deep-sea diving, gas mixtures are engineered to prioritize safety. Different gases like helium and oxygen are blended for divers to breathe safely under high pressure. Oxygen must be regulated to avoid toxicity, while helium is added to reduce nitrogen's narcotic effects at depth.
Engineers and scientists meticulously calculate the proportions of gases within a mixture to ensure that the partial pressures of each component remain within safe and effective limits. These calculations safeguard divers from potential hazards, thereby highlighting the importance of understanding gas mixtures.
Deep-Sea Diving: A Delicate Balance
Deep-sea diving requires careful planning and understanding of gas laws to ensure diver safety. At great depths, the pressure increases significantly, causing a corresponding increase in the partial pressures of the gases being breathed.
For divers, maintaining the appropriate partial pressures of oxygen is crucial. Oxygen contributes to vital bodily functions, but too much of it at a high pressure can lead to oxygen toxicity, which poses a serious risk to divers. By managing the gas mixtures properly—like including helium to desaturate nitrogen and control oxygen levels—the risk of negative physiological effects can be minimized.
Therefore, deep-sea diving highlights the practical application of Dalton's Law of Partial Pressures. Divers depend on this knowledge to manage their breathing mixtures, ensuring each dive is safe and efficient. By adhering to this delicate balance, both safety and success can be achieved during undersea adventures.
Understanding these principles allows for careful preparation and successful dives that both protect divers' health and enhance their underwater experience.
