Ideal Gas Laws: Understanding Pressure, Temperature, and Specific Volume, Lecture notes of Thermodynamics

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Presented by: John Lester D. Mones

Objectives

At the end of this course, the learners will be able to:

• discuss the ideal gas laws;
• solve problems involving ideal gas laws; and
• explain the processes of ideal gases.

• Boyle, Charles, and Gay-Lussac observed that pressure of gases is inversely proportional to their volume, and the volume of a gas is proportional to its temperature 𝐏 = 𝐑

Where: P - absolute pressure T - absolute temperature v - specific volume R – gas constant

• The gas constant R is different for each gas and is determined from: 𝑹 =

(kJ/kg∙K or kPa∙m 3 /kg∙K) Where: Ru – universal gas constant M – molar mass / molecular wt.

• What is the mass of 3 kmol of diatomic nitrogen

compressed in a tank?

• What is the gas constant of a gas with the molar mass of

32 g/mol?

• The ideal-gas equation of state can be written in several different forms: 𝐏𝐕 = 𝐦𝐑𝐓 𝐏𝐕 = 𝐍𝐑 𝐮

Where: vത – molar specific volume

• The properties of an ideal gas at two different states are

related to each other by:

𝟏

𝟏

𝟏

𝟐

𝟐

𝟐

• At a pressure of 405 kPa, the volume of a gas is 6. 00 cm 3 . Assuming the temperature remains constant, at what pressure will the new volume be 4. 00 cm 3 ?
• A gas with a volume of 4. 0 L at a pressure of 205 kPa is allowed to expand to a volume of 12. 0 L. What is the pressure in the container if the temperature remains constant?

• The gas constant R is different for each gas and is determined from: 𝑹 =

(kJ/kg∙K or kPa∙m 3 /kg∙K) Where: Ru – universal gas constant M – molar mass / molecular wt.

• Isobaric

- this is a process where the pressure of the system is kept

constant

• Isochoric

- this is a process where the volume of the system is kept

constant.

• Adiabatic

- This is a process where no heat is being added or

removed from the system.

- no heat transfer (or heat flow) happening in a system.

- Q = 0