Saturated Vapor Pressure Quiz

Podcast Beta

Play an AI-generated podcast conversation about this lesson

Questions and Answers

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?

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?

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?

532 mm-Hg Signup and view all the answers

What is the critical temperature of a substance defined as?

The highest temperature at which it can exist as a liquid. Signup and view all the answers

If the atmospheric pressure is 550 mm-Hg, what is the partial pressure of O2 at this elevation?

116 mm-Hg Signup and view all the answers

What happens to the vapor pressure of a liquid as the temperature increases?

Vapor pressure increases with temperature. Signup and view all the answers

What is the boiling point of a liquid defined as?

The temperature where vapor pressure equals atmospheric pressure. Signup and view all the answers

What determines the boiling point of a liquid?

The saturated vapor pressure equal to atmospheric pressure Signup and view all the answers

Which gas law states that the total pressure of a gas mixture is the sum of the partial pressures?

Dalton's Law of Partial Pressures Signup and view all the answers

What happens to the boiling point of a liquid as altitude increases?

It decreases Signup and view all the answers

If the saturated vapor pressure of Isoflurane is 240 mm Hg, what is its percent composition in a 760 mm Hg mixture of gases?

31.6% Signup and view all the answers

What is vapor pressure a function of?

Temperature only Signup and view all the answers

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?

68.4% Signup and view all the answers

Which of the following best describes saturated vapor pressure?

The pressure at which vapor and liquid coexist in a closed system Signup and view all the answers

What is the approximate vapor pressure of Desflurane at 20°C?

669 mm Hg Signup and view all the answers

What relationship does Gay Lussac’s Law describe between pressure and temperature at constant volume?

Pressure is directly proportional to temperature. Signup and view all the answers

What happens to the pressure in a N2O cylinder as it empties?

The pressure decreases even if liquid N2O is present. Signup and view all the answers

At standard temperature and pressure, how much volume does one mole of a gas occupy according to Avogadro's hypothesis?

22.4 liters Signup and view all the answers

What is the universal gas constant (R) in SI units?

1.987 J/degree/mole Signup and view all the answers

What is the significance of the Bourdon’s gauge in a gas cylinder?

It serves as a content gauge for the amount of gas. Signup and view all the answers

Under what conditions can a gas liquefy according to the critical temperature concept?

At low temperatures with sufficient pressure applied. Signup and view all the answers

What occurs during an adiabatic process involving a compressed gas?

The temperature rises rapidly without heat gain. Signup and view all the answers

What effect does the Joule-Thompson effect describe when a compressed gas escapes into space?

Cooling occurs during the escape. Signup and view all the answers

What happens to flow in a tube when it becomes turbulent?

Resistance to flow increases Signup and view all the answers

How do you calculate the amount of dissolved O2 in the blood?

Multiply the partial pressure of O2 by 0.003 Signup and view all the answers

Which law describes the relationship between gas solubility and partial pressure at a constant temperature?

Henry's Law Signup and view all the answers

What is the significance of Reynolds number in fluid dynamics?

It indicates whether flow is laminar or turbulent Signup and view all the answers

What factor does NOT contribute to turbulent flow in a tube?

Smooth interior surface of the tube Signup and view all the answers

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?

1.5 mL O2/100 mL blood Signup and view all the answers

What is the approximate solubility of carbon dioxide in blood according to Henry's Law?

0.067 ml/dL/mmHg Signup and view all the answers

Which of the following statements about Poiseuille's Law is true?

It includes factors such as diameter and viscosity. Signup and view all the answers

How much dissolved oxygen is present in 100 mL of blood when PaO2 is 100 mm Hg?

0.3 mL O2/100 mL blood Signup and view all the answers

If the fraction of inspired oxygen (FiO2) is 40%, what is the estimated PaO2?

200 mm Hg Signup and view all the answers

According to Henry's Law, how much CO2 is dissolved in 100 mL of blood when PaCO2 is 50 mm Hg?

3.35 mL CO2/100 mL blood Signup and view all the answers

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?

665 Liters Signup and view all the answers

What happens to the intrapulmonary pressure during expiration?

Increases and volume decreases Signup and view all the answers

According to Charles's Law, what happens to the volume of the gas in an inflatable cuff when it is heated?

Volume increases Signup and view all the answers

How long will an E type full oxygen cylinder last if 3 liters of O2 are used per minute?

220 minutes Signup and view all the answers

Which clinical application involves Boyle's Law related to intrapulmonary pressure changes?

Inflation of an Ambu bag Signup and view all the answers

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.
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.

Studying That Suits You

Use AI to generate personalized quizzes and flashcards to suit your learning preferences.

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.