Equilibrium: Heat energy
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physics & chemistry
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published 28/07/2008
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level : Advanced
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SummaryHeat is energy flowing from a high temperature object to a low temperature object. When the two objects are at the same temperature, there is no net flow of energy or heat. That is why a covered cup of coffee will not be colder than or warmer than the room temperature after it has been in there for a few hours. This phenomenon is known as equilibrium. In this example, we deal with the flow of energy. Equilibria happen in phase transitions. For example, if the temperature in a system containing a mixture of ice and water is uniformly 273.15 K, the net amount of ice formed and the melt will be zero. The amount of liquid water will also remain constant, if no vapor escape from the system.
Table of Contents
- Chemical equilibrium.
- Beginning of reaction.
- Haber process.
- Static equilibrium.
- Dynamic equilibrium.
- Heterogeneous equilibria.
- Manipulating the equilibrium law.
- Application of equilibrium constant.
- Reaction quotient (Q).
- Solving equilibrium problems.
- Le Chatelier's principle.
- The effect of change in concentration.
- Addition of solvent to an equilibrium system in solution.
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