22. The First Law of Thermodynamics

PV Diagrams & Work

PV Diagrams

16 - Thermodynamics - PV diagram

A cylinder contains 0.0100 mol of helium at T = 27.0°C. (a) How much heat is needed to raise the temperature to 67.0°C while keeping the volume constant? Draw a pV-diagram for this process. (b) If instead the pressure of the helium is kept constant, how much heat is needed to raise the temperature from 27.0°C to 67.0°C? Draw a pV-diagram for this process. (c) What accounts for the difference between your answers to parts (a) and (b)? In which case is more heat required? What becomes of the additional heat? (d) If the gas is ideal, what is the change in its internal energy in part (a)? In part (b)? How do the two answers compare? Why?

Work and PV Diagrams

PV diagrams and work

Finding Value of V on Axis

PV Graph and First Law of Thermodynamics

A gas undergoes two processes. In the first, the volume remains constant at 0.200 m^3 and the pressure increases from 2.00 * 10^5 Pa to 5.00 * 10^5 Pa. The second process is a compression to a volume of 0.120 m^3 at a constant pressure of 5.00 * 10^5 Pa. (b) Find the total work done by the gas during both processes.

Two moles of an ideal gas are heated at constant pressure from T = 27°C to T = 107°C. (b) Calculate the work done by the gas

The pV-diagram in Fig. E19.13 shows a process abc involving 0.450 mol of an ideal gas.<img src="https://lightcat-files.s3.amazonaws.com/problem_images/28537634428e4ac9-XYZ.png" alt="" /> (c) How much heat had to be added during the process to increase the internal energy of the gas by 15,000 J?<img class="fr-dib" src="https://lightcat-files.s3.amazonaws.com/problem_images/9e2c73cf351fef61-1678286114148.jpg" style="width: 240px;">

Lesson 6 - Work Heat And PV Diagrams (Physics Tutor)

An ideal gas is taken from a to b on the pV-diagram shown in Fig. E19.15. During this process, 700 J of heat is added and the pressure doubles. <img src="https://lightcat-files.s3.amazonaws.com/problem_images/6dc3b4f9b4c4445b-PV%20XY.png" alt="" /> (c) How does the internal energy of the gas at a compare to the internal energy at b? Be specific and explain.<img class="fr-dib" src="https://lightcat-files.s3.amazonaws.com/problem_images/b8372dc60f833599-1678286197625.jpg" style="width: 226px;">

The process abc shown in the pV-diagram in Fig. E19.11 involves 0.0175 mol of an ideal gas. <img src="https://lightcat-files.s3.amazonaws.com/problem_images/59844642557910b3-JKL.png" alt="" /> (a) What was the lowest temperature the gas reached in this process? Where did it occur?<img class="fr-dib" src="https://lightcat-files.s3.amazonaws.com/problem_images/07cbefd8b90bab60-1678286050443.jpg" style="width: 251px;">

Thermodynamics and P-V Diagrams

Two moles of an ideal gas are heated at constant pressure from T = 27°C to T = 107°C. (a) Draw a pV-diagram for this process. (ANSWER IS )

Figure E19.8 shows a pV-diagram for an ideal gas in which its absolute temperature at b is one-fourth of its absolute temperature at a. <img src="https://lightcat-files.s3.amazonaws.com/problem_images/e1a0fb881af993b3-only%20a%20graph.png" alt="" /> (d) Did heat enter or leave the gas from a to b? How do you know? <img class="fr-dib" src="https://lightcat-files.s3.amazonaws.com/problem_images/f0725576d807aef3-1678285905457.jpg" style="width: 281px;">

A gas undergoes two processes. In the first, the volume remains constant at 0.200 m^3 and the pressure increases from 2.00 * 10^5 Pa to 5.00 * 10^5 Pa. The second process is a compression to a volume of 0.120 m^3 at a constant pressure of 5.00 * 10^5 Pa. (a) In a pV-diagram, show both processes. <ANSWER IS >

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