🫀anatomy and physiology ii review

key term - Henry's Law

Definition

Henry's Law states that at a constant temperature, the amount of gas that dissolves in a liquid is directly proportional to the partial pressure of that gas above the liquid. This principle is crucial in understanding how gases behave during breathing and gas exchange in the lungs, where the pressure of gases in the alveoli influences their solubility in blood and other fluids.

5 Must Know Facts For Your Next Test

  1. Henry's Law is expressed mathematically as C = kH * P, where C is the concentration of the gas in the liquid, kH is Henry's law constant, and P is the partial pressure of the gas.
  2. The solubility of different gases varies; for example, carbon dioxide is more soluble in water than oxygen due to its molecular properties.
  3. During inhalation, the partial pressure of oxygen increases in the alveoli, leading to greater diffusion into the blood as per Henry's Law.
  4. Conversely, during exhalation, the concentration of carbon dioxide in the alveoli rises, facilitating its release from blood into the lungs.
  5. Henry's Law helps explain why divers must be cautious with ascent; changes in pressure affect gas solubility, which can lead to decompression sickness.

Review Questions

  • How does Henry's Law explain the process of gas exchange in the lungs during inhalation?
    • During inhalation, oxygen enters the alveoli and its partial pressure increases. According to Henry's Law, this rise in partial pressure leads to greater amounts of oxygen dissolving into the blood. The higher concentration of dissolved oxygen in the blood enhances its transport to tissues where it is needed. This relationship illustrates how changes in pressure impact gas solubility and absorption during breathing.
  • Discuss how variations in temperature affect Henry's Law and gas solubility related to respiratory physiology.
    • Temperature plays a crucial role in Henry's Law as it can affect gas solubility. Generally, as temperature increases, the solubility of gases decreases. In respiratory physiology, this means that if body temperature rises due to exercise or fever, less oxygen and carbon dioxide can dissolve in blood plasma. Consequently, this may impact overall oxygen delivery to tissues and carbon dioxide removal during respiration.
  • Evaluate the implications of Henry's Law for understanding decompression sickness in divers.
    • Decompression sickness occurs when divers ascend too quickly, causing dissolved nitrogen to come out of solution too rapidly due to reduced ambient pressure. According to Henry's Law, as pressure decreases during ascent, nitrogen's solubility also decreases. If nitrogen bubbles form too quickly within tissues or bloodstream, it can lead to serious health issues. Understanding this principle allows divers to appreciate safe ascent rates and prevent potential injury from gas embolism.