Hyperbaric chambers, which provide high pressures (up to 6 atm) of either air or pure oxygen, are used to treat a variety of conditions, ranging from decompression sickness in deep-sea divers to carbon monoxide poisoning. Look up the solubility of O₂, N₂, CO, and CO₂ in water at standard temperature and pressure (1 atm, 25 °C). Explain how elevated pressures in a hyperbaric chamber be used to treat decompression sickness (excess N₂ in blood) and carbon monoxide poisoning. (Refer to Section 7.9 and Section 9.5)

Verified step by step guidance

1. Understand the concept of gas solubility: According to Henry's Law, the solubility of a gas in a liquid is directly proportional to the pressure of that gas above the liquid. This means that increasing the pressure of a gas will increase its solubility in a liquid.
2. Decompression sickness treatment: In decompression sickness, excess nitrogen (N₂) is dissolved in the blood due to high pressures experienced during deep-sea diving. When a diver ascends too quickly, the pressure decreases rapidly, causing nitrogen to form bubbles in the blood. By using a hyperbaric chamber, the pressure is increased, which helps dissolve the nitrogen back into the blood, allowing it to be safely eliminated from the body.
3. Carbon monoxide poisoning treatment: Carbon monoxide (CO) binds to hemoglobin in the blood more effectively than oxygen, reducing the blood's oxygen-carrying capacity. In a hyperbaric chamber, the pressure of oxygen is increased, which enhances the solubility of oxygen in the blood. This helps displace carbon monoxide from hemoglobin, allowing oxygen to bind instead and improving oxygen delivery to tissues.
4. Refer to Section 7.9: This section likely discusses gas solubility and the effects of pressure on solubility, providing a theoretical basis for understanding how hyperbaric chambers work.
5. Refer to Section 9.5: This section might cover specific applications of gas solubility principles, such as the treatment of decompression sickness and carbon monoxide poisoning, offering detailed explanations and examples.

Key Concepts

Henry's Law

Henry's Law states that the amount of gas that dissolves in a liquid is directly proportional to the partial pressure of that gas above the liquid. In the context of hyperbaric chambers, increasing the pressure allows more oxygen and nitrogen to dissolve in the blood, which is crucial for treating conditions like decompression sickness and carbon monoxide poisoning.

Decompression Sickness

Decompression sickness, also known as 'the bends,' occurs when nitrogen dissolved in the blood forms bubbles as pressure decreases during ascent from deep water. Hyperbaric treatment helps by increasing the pressure, allowing excess nitrogen to dissolve back into the blood, thus preventing bubble formation and alleviating symptoms.

Carbon Monoxide Poisoning

Carbon monoxide poisoning occurs when CO binds to hemoglobin in red blood cells more effectively than oxygen, reducing oxygen transport. Hyperbaric oxygen therapy increases the amount of dissolved oxygen in the blood, displacing carbon monoxide from hemoglobin and facilitating its elimination from the body, thereby improving oxygen delivery to tissues.