Partial Pressure in Gases
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Questions and Answers

What is the total pressure of gases in a given mixture?

  • The average pressure of the gases
  • The sum of individual pressures of all gases (correct)
  • The pressure of the most abundant gas
  • The pressure of the gas with the highest solubility

    • How is the partial pressure of a specific gas determined?

  • By dividing its concentration by the total volume
  • By using its fractional concentration multiplied by the total pressure (correct)
  • By subtracting its pressure from the atmospheric pressure
  • By adding the gas's concentration to the atmospheric pressure

    • What is the value of partial pressure of O2 at sea level in dry inspired air?

  • 47 mm Hg
  • 160 mm Hg (correct)
  • 99.33 mm Hg
  • 150 mm Hg

    • What happens to partial pressure of inspired oxygen, PIO2, when at a higher elevation?

    <p>It decreases due to lower atmospheric pressure</p> Signup and view all the answers

    What will occur to PIO2 when receiving supplemental oxygen at an FIO2 of 80%?

    <p>PIO2 will increase dramatically</p> Signup and view all the answers

    What does Henry's Law state regarding the concentration of a gas in a liquid?

    <p>It is equal to the partial pressure of the gas times its solubility</p> Signup and view all the answers

    What factors affect the partial pressure of gases in the alveoli?

    <p>Temperature and humidity levels</p> Signup and view all the answers

    What is the formula to calculate the partial pressure of inspired oxygen in humidified air?

    <p>PIO2 = (Patm - PH2O) x FIO2</p> Signup and view all the answers

    Why is the concentration of a gas in solution solely due to dissolved gas considered?

    <p>Because only dissolved gases contribute to blood oxygen levels</p> Signup and view all the answers

    What does the term 'partial pressure' refer to?

    <p>The pressure a single gas exerts in a mixture of gases.</p> Signup and view all the answers

    Which gas is the most abundant in Earth's atmosphere?

    <p>Nitrogen</p> Signup and view all the answers

    What is the average atmospheric pressure at sea level?

    <p>760 mmHg</p> Signup and view all the answers

    Which law states that in a mixture of gases, the total pressure is equal to the sum of the partial pressures of each gas?

    <p>Dalton's Law</p> Signup and view all the answers

    What percentage of oxygen is typically present in the air?

    <p>21%</p> Signup and view all the answers

    Which of the following is NOT a factor affecting the partial pressures of gases?

    <p>Density of the gas</p> Signup and view all the answers

    What physical process governs gas exchange between the lung and blood?

    <p>Diffusion</p> Signup and view all the answers

    How does the motion of gas molecules relate to gas pressure?

    <p>It is proportional to the pressure exerted by gases.</p> Signup and view all the answers

    Which statement correctly describes bulk flow in relation to gas exchange?

    <p>Bulk flow involves the transportation of gases within the lungs to the gas exchange surfaces.</p> Signup and view all the answers

    What factors would affect the partial pressure of inspired oxygen?

    <p>Altitude and temperature</p> Signup and view all the answers

    Study Notes

    Partial Pressure

    • The pressure a single gas exerts in a mixture of gases
    • Atmospheric pressure = Barometric pressure
    • Most abundant gas in our atmosphere: nitrogen
    • % of Oxygen in air: 21%
    • Average atmospheric pressure at sea level: 760 mmHg

    Calculating Partial Pressure

    • Partial pressure of a specific gas: Px = Patm x Fx (Px = partial pressure of a gas in mmHg, Patm = atmospheric pressure, Fx = fractional concentration of gas)
    • For air: Patm = PN2 + PO2 + PH2O + PCO2

    Calculation of PO2 and PIO2

    • PO2 = Patm x FO2 = 760 mm Hg x 0.21 = 160 mm Hg
    • PIO2 = (Patm – PH2O) x FIO2 = (760 mm Hg - 47 mm Hg) x 0.21 = 150 mm Hg

    Thought Experiments on PIO2

    • Lower at the top of Mt. Humphrey’s compared to Phoenix because Patm is lower at high elevation, FIO2 doesn’t change
    • Higher when receiving supplemental oxygen (increasing the FI02 to 80%) through a non-rebreathing mask because FIO2 increased, Patm is unchanged

    Concentrations of Dissolved Gases

    • Equilibrium reached when Px (gas) = Px (liquid)
    • Henry’s Law: Concentration of a GAS (in liquid) = Px x solubility
    • Concentration of a gas in solution is ONLY due to dissolved gas, not relevant if bound, e.g.to hemoglobin, or chemically modified, e.g.into HCO3-

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    Lecture 20: Gas Exchange PDF

    Description

    This quiz covers the concept of partial pressure in mixtures of gases, focusing on its calculation and implications in different environments. It discusses atmospheric pressure, contributions of individual gases, and thought experiments related to oxygen concentration at varying elevations and conditions. Test your understanding of these essential principles in gas behavior.

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