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Chapter 13: Problem 50

Respiratory problems are treated with devices that deliver air with a higher partial pressure of \(\mathrm{O}_{2}\) than normal air. Why?

Short Answer

Expert verified
Higher partial pressure of \(\mathrm{O}_{2}\) improves oxygen absorption by the bloodstream, aiding those with respiratory issues.

Step by step solution

01

- Understand Partial Pressure

Partial pressure is the pressure that a single component of a mixture of gases contributes to the total pressure of the mixture. For oxygen, its partial pressure is an important factor in how it is absorbed into the bloodstream.
02

- Role of \(\mathrm{O}_{2}\)

Oxygen is essential for cellular respiration, which is the process cells use to produce energy. In individuals with respiratory problems, the efficiency of oxygen exchange in the lungs may be compromised.
03

- Effect of Higher Partial Pressure of \(\mathrm{O}_{2}\)

Increasing the partial pressure of \(\mathrm{O}_{2}\) in the air can enhance the rate at which oxygen dissolves in the blood. This is due to the principles of gas exchange, where gases diffuse from areas of higher partial pressure to areas of lower partial pressure.
04

- Improved Oxygen Delivery

By delivering air with a higher partial pressure of \(\mathrm{O}_{2}\), these devices facilitate a greater uptake of oxygen by the bloodstream, improving oxygen availability to tissues and aiding in the respiratory process for those with compromised lung function.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Gas Laws in Respiratory Therapy
Gas laws play a crucial role in respiratory therapy, particularly in understanding how oxygen is delivered and utilized by the body. Let's break it down:
  • Partial Pressure: This concept explains the contribution of a single gas in a mixture to the overall pressure. In medicine, understanding partial pressure is essential for grasping how oxygen moves from the lungs into the blood.
  • Boyle's Law: It states that the pressure of a gas is inversely proportional to its volume. This is seen in how we breathe. When our lungs expand, the pressure inside drops, allowing air to flow in.
  • Henry's Law: It tells us that the amount of gas dissolved in a liquid is proportional to its partial pressure. Thus, increasing the partial pressure of oxygen in inhaled air increases the amount dissolved in our blood.
Understanding these gas laws helps respiratory therapists optimize oxygen delivery to patients with compromised lung function.
Oxygen Exchange in Lungs
Oxygen exchange in the lungs is a pivotal process for maintaining life. It happens in these steps:
  • Inhalation: Air enters the lungs, filling alveoli, tiny air sacs where gas exchange occurs. This air contains a higher partial pressure of oxygen compared to the blood in the pulmonary capillaries.
  • Diffusion: Oxygen diffuses from alveoli into the blood because it moves from areas of higher partial pressure to areas of lower partial pressure, as stated by Fick's Law of Diffusion.
  • Binding to Hemoglobin: Once in the blood, oxygen binds to hemoglobin molecules in red blood cells, facilitating transport throughout the body.
  • Exhalation: Carbon dioxide, a waste product of cellular respiration, is exhaled out of the lungs following a similar diffusion process in reverse.
Enhancing the partial pressure of oxygen can improve this process, especially in patients with respiratory issues, ensuring tissues receive the oxygen needed for proper function.
Cellular Respiration
Cellular respiration is the process by which cells produce energy from oxygen and glucose. Here are the key stages:
  • Glycolysis: This anaerobic process occurs in the cytoplasm and breaks down glucose into pyruvate, producing a small amount of energy (ATP).
  • Krebs Cycle: Also known as the Citric Acid Cycle, this takes place in the mitochondria, where pyruvate is further broken down, generating electron carriers and more ATP.
  • Electron Transport Chain: The final stage occurs in the mitochondrial membrane. Here, electrons from carrier molecules are used to create a proton gradient that drives the production of a large amount of ATP.
Oxygen plays a critical role, especially in the electron transport chain, where it acts as the final electron acceptor. Without sufficient oxygen, cells cannot efficiently produce the energy needed for survival, highlighting the importance of oxygen therapy.

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Most popular questions from this chapter

A pharmaceutical preparation made with ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) is contaminated with methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right) .\) A sample of vapor above the liquid mixture contains a \(97 / 1\) mass ratio of \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\) to \(\mathrm{CH}_{3} \mathrm{OH}\). What is the mass ratio of these alcohols in the liquid mixture? At the temperature of the liquid mixture, the vapor pressures of \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\) and \(\mathrm{CH}_{3} \mathrm{OH}\) are 60.5 torr and 126.0 torr, respectively.

A small protein has a molar mass of \(1.50 \times 10^{4} \mathrm{~g} / \mathrm{mol}\). What is the osmotic pressure exerted at \(24.0^{\circ} \mathrm{C}\) by \(25.0 \mathrm{~mL}\) of an aqueous solution that contains \(37.5 \mathrm{mg}\) of the protein?

The freezing point of benzene is \(5.5^{\circ} \mathrm{C}\). What is the freezing point of a solution of \(5.00 \mathrm{~g}\) of naphthalene \(\left(\mathrm{C}_{10} \mathrm{H}_{8}\right)\) in \(444 \mathrm{~g}\) of benzene \(\left(K_{\mathrm{f}}\right.\) of benzene \(\left.=4.90^{\circ} \mathrm{C} / \mathrm{m}\right) ?\)

Pyridine (right) is an essential portion of many biologically active compounds, such as nicotine and vitamin \(\mathrm{B}_{6}\). Like ammonia, it has a nitrogen with a lone pair, which makes it act as a weak base. Because it is miscible in a wide range of solvents, from water to benzene, pyridine is one of the most important bases and solvents in organic syntheses. Account for its solubility behavior in terms of intermolecular forces.

Wastewater from a cement factory contains \(0.25 \mathrm{~g}\) of \(\mathrm{Ca}^{2+}\) ions and \(0.056 \mathrm{~g}\) of \(\mathrm{Mg}^{2+}\) ions per \(100.0 \mathrm{~L}\) of solution. The solution density is \(1.001 \mathrm{~g} / \mathrm{mL}\). Calculate the \(\mathrm{Ca}^{2+}\) and \(\mathrm{Mg}^{2+}\) concentrations in ppm (by mass).
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