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Questions and Answers
What does Dalton's Law of Partial Pressures state about the total pressure of a mixture of gases?
What does Dalton's Law of Partial Pressures state about the total pressure of a mixture of gases?
- The total pressure is equal to the sum of the partial pressures of the individual gases. (correct)
- The total pressure is the product of the partial pressures.
- The total pressure is equal to the square root of the individual pressures.
- The total pressure is dependent on the specific gas that is present.
How is the partial pressure of a gas calculated?
How is the partial pressure of a gas calculated?
- By averaging the pressures of all the gases present in the mixture.
- By subtracting the atmospheric pressure from the total pressure.
- By multiplying the fractional concentration of the gas by the atmospheric pressure. (correct)
- By dividing the total pressure by the percentage of the gas.
What is the total atmospheric pressure at sea level expressed in mm-Hg?
What is the total atmospheric pressure at sea level expressed in mm-Hg?
- 800 mm-Hg
- 500 mm-Hg
- 760 mm-Hg (correct)
- 730 mm-Hg
What is the partial pressure of N2O in a 70% N2O/30% O2 mixture at sea level?
What is the partial pressure of N2O in a 70% N2O/30% O2 mixture at sea level?
What is the critical temperature of a substance defined as?
What is the critical temperature of a substance defined as?
If the atmospheric pressure is 550 mm-Hg, what is the partial pressure of O2 at this elevation?
If the atmospheric pressure is 550 mm-Hg, what is the partial pressure of O2 at this elevation?
What happens to the vapor pressure of a liquid as the temperature increases?
What happens to the vapor pressure of a liquid as the temperature increases?
What is the boiling point of a liquid defined as?
What is the boiling point of a liquid defined as?
What determines the boiling point of a liquid?
What determines the boiling point of a liquid?
Which gas law states that the total pressure of a gas mixture is the sum of the partial pressures?
Which gas law states that the total pressure of a gas mixture is the sum of the partial pressures?
What happens to the boiling point of a liquid as altitude increases?
What happens to the boiling point of a liquid as altitude increases?
If the saturated vapor pressure of Isoflurane is 240 mm Hg, what is its percent composition in a 760 mm Hg mixture of gases?
If the saturated vapor pressure of Isoflurane is 240 mm Hg, what is its percent composition in a 760 mm Hg mixture of gases?
What is vapor pressure a function of?
What is vapor pressure a function of?
In a mixture of gases, if the partial pressure of oxygen is 520 mm Hg and the total pressure is 760 mm Hg, what percent of the mixture is oxygen?
In a mixture of gases, if the partial pressure of oxygen is 520 mm Hg and the total pressure is 760 mm Hg, what percent of the mixture is oxygen?
Which of the following best describes saturated vapor pressure?
Which of the following best describes saturated vapor pressure?
What is the approximate vapor pressure of Desflurane at 20°C?
What is the approximate vapor pressure of Desflurane at 20°C?
What relationship does Gay Lussac’s Law describe between pressure and temperature at constant volume?
What relationship does Gay Lussac’s Law describe between pressure and temperature at constant volume?
What happens to the pressure in a N2O cylinder as it empties?
What happens to the pressure in a N2O cylinder as it empties?
At standard temperature and pressure, how much volume does one mole of a gas occupy according to Avogadro's hypothesis?
At standard temperature and pressure, how much volume does one mole of a gas occupy according to Avogadro's hypothesis?
What is the universal gas constant (R) in SI units?
What is the universal gas constant (R) in SI units?
What is the significance of the Bourdon’s gauge in a gas cylinder?
What is the significance of the Bourdon’s gauge in a gas cylinder?
Under what conditions can a gas liquefy according to the critical temperature concept?
Under what conditions can a gas liquefy according to the critical temperature concept?
What occurs during an adiabatic process involving a compressed gas?
What occurs during an adiabatic process involving a compressed gas?
What effect does the Joule-Thompson effect describe when a compressed gas escapes into space?
What effect does the Joule-Thompson effect describe when a compressed gas escapes into space?
What happens to flow in a tube when it becomes turbulent?
What happens to flow in a tube when it becomes turbulent?
How do you calculate the amount of dissolved O2 in the blood?
How do you calculate the amount of dissolved O2 in the blood?
Which law describes the relationship between gas solubility and partial pressure at a constant temperature?
Which law describes the relationship between gas solubility and partial pressure at a constant temperature?
What is the significance of Reynolds number in fluid dynamics?
What is the significance of Reynolds number in fluid dynamics?
What factor does NOT contribute to turbulent flow in a tube?
What factor does NOT contribute to turbulent flow in a tube?
If the partial pressure of O2 increases from 100 mm Hg to 500 mm Hg, how much does the amount of dissolved O2 in the blood increase?
If the partial pressure of O2 increases from 100 mm Hg to 500 mm Hg, how much does the amount of dissolved O2 in the blood increase?
What is the approximate solubility of carbon dioxide in blood according to Henry's Law?
What is the approximate solubility of carbon dioxide in blood according to Henry's Law?
Which of the following statements about Poiseuille's Law is true?
Which of the following statements about Poiseuille's Law is true?
How much dissolved oxygen is present in 100 mL of blood when PaO2 is 100 mm Hg?
How much dissolved oxygen is present in 100 mL of blood when PaO2 is 100 mm Hg?
If the fraction of inspired oxygen (FiO2) is 40%, what is the estimated PaO2?
If the fraction of inspired oxygen (FiO2) is 40%, what is the estimated PaO2?
According to Henry's Law, how much CO2 is dissolved in 100 mL of blood when PaCO2 is 50 mm Hg?
According to Henry's Law, how much CO2 is dissolved in 100 mL of blood when PaCO2 is 50 mm Hg?
Using Boyle's Law, if the service pressure of an E size cylinder is 2000 psig and the volume is approximately 5 Liters, what is the final volume (V2) after using gas?
Using Boyle's Law, if the service pressure of an E size cylinder is 2000 psig and the volume is approximately 5 Liters, what is the final volume (V2) after using gas?
What happens to the intrapulmonary pressure during expiration?
What happens to the intrapulmonary pressure during expiration?
According to Charles's Law, what happens to the volume of the gas in an inflatable cuff when it is heated?
According to Charles's Law, what happens to the volume of the gas in an inflatable cuff when it is heated?
How long will an E type full oxygen cylinder last if 3 liters of O2 are used per minute?
How long will an E type full oxygen cylinder last if 3 liters of O2 are used per minute?
Which clinical application involves Boyle's Law related to intrapulmonary pressure changes?
Which clinical application involves Boyle's Law related to intrapulmonary pressure changes?
Study Notes
Vapor Pressure and Saturation
- Vapor pressure is a function of temperature; it indicates the pressure where gaseous and liquid states are in equilibrium.
- Saturated vapor pressure reflects the pressure at which a liquid boils, balancing atmospheric pressure.
- Boiling point increases with atmospheric pressure; it decreases at higher altitudes due to lower atmospheric pressure.
Dalton’s Law of Partial Pressures
- Total pressure of a gas mixture equals the sum of the partial pressures of its individual gases.
- Partial pressure can be calculated using the formula: Partial Pressure = Percent Fraction × Atmospheric Pressure.
- Example: At sea level, O2 has a partial pressure of 160 mm Hg (21%); N2 has 600 mm Hg (79%).
Clinical Applications of Dalton’s Law
- In a 70% N2O and 30% O2 mixture at sea level (760 mm Hg):
- Partial pressure of N2O: 70% × 760 mm Hg = 532 mm Hg.
- Partial pressure of O2: 30% × 760 mm Hg = 228 mm Hg.
- In mountains with a Patm of 550 mm Hg:
- Partial pressure of O2: 21% × 550 mm Hg = 116 mm Hg.
Vapor Pressure and Critical Temperature
- Vapor pressure signifies a liquid’s tendency to evaporate, influenced by temperature.
- Critical temperature is the maximum temperature a substance can exist as a liquid; above this, it is gaseous regardless of pressure.
Gas Laws and Their Clinical Implications
- Henry’s Law: Gas solubility in a solution is directly proportional to the partial pressure of the gas.
- O2 dissolved in blood: 0.003 mL/dL/mm Hg; CO2: 0.067 mL/dL/mm Hg.
- Example of calculation: At PaO2 of 300 mm Hg, dissolved O2 = 300 × 0.003 = 0.9 mL O2/100 mL blood.
- Boyle's Law: At constant temperature, gas volume is inversely proportional to pressure.
- Example with an E size cylinder:
- If P1 = 2000 psig and V1 = 5 L, the remaining volume can be calculated with P2V2 = P1V1.
- Example with an E size cylinder:
- Charles’s Law: At constant pressure, gas volume is directly proportional to temperature.
- Example: An inflatable cuff expands with increased temperature during sterilization.
- Gay-Lussac’s Law: At constant volume, pressure of gas is directly proportional to temperature.
- Important for gas storage safety to prevent explosions.
Avogadro’s Hypothesis and Ideal Gas Law
- Avogadro’s number is 6.022 × 10²³; one mole of gas occupies 22.4 liters at STP.
- Ideal gas equation: PV = nRT, where R is the universal gas constant.
Gas Cylinder Considerations
- Gases liquefy under sufficient pressure below the critical temperature.
- Adiabatic processes can lead to temperature increases that pose ignition risks.
- The Joule-Thompson effect indicates cooling during adiabatic expansion as gas escapes.
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Description
Test your understanding of saturated vapor pressure and its relationship with temperature. Explore how vapor pressure interacts with liquid and gas states and the impact of boiling points. This quiz will help clarify key concepts in thermodynamics.
