Interactive Self-Study Module: Fugacity of a Single Component
This module uses screencasts and interactive simulations to explain the driving force for single-component phase equilibrium. It then provides example problems to allow the user to test themselves. Your retention of material in this module will increase if you write down reasons for your answers to ConcepTests, questions in screencasts, and questions to answer before using interactive simulations, and you try to solve the example problems before watching the screencast solutions. We suggest reviewing the single-component phase equilibrium module before using the learning resources in the following order:
- Attempt to answer the multiple choice ConcepTest and solve the example problem before watching the screencasts or working with the simulations.
- Watch the screencasts that describe fugacity.
- Review important equations for fugacity of a single component.
- Use the interactive simulations to further understand the driving force for mass transfer.
- Try to solve the example problems before watching the solutions in the screencasts.
- Answer the ConcepTests.
- Look at the list of key points, but only after you try to list the key points yourself.
- Fugacity is used to determine the direction of mass transfer between phases and to determine when phases are in equilibrium.
- This module is intended for a thermodynamics course.
Before studying this module, you should be able to:
- Explain single-component phase equilibrium.
- Calculate the saturation pressure or temperature given Antoine constants
After studying this module, you should be able to:
- Calculate fugacity of a single-component ideal gas.
- Calculate the fugacity of a liquid or a solid.
- Calculate the fugacity of a non-ideal gas.
- Determine the direction of mass transfer between phases.
- Calculate the fugacity of a liquid or solid at high pressure using the Poynting correction.
- Explain the criteria for single-component phase equilibrium in terms of fugacity.
- Explain why the fugacity of a saturated liquid is close to the vapor pressure of the liquid.