An isobaric process is a thermodynamic process in which the pressure of the system remains constant. During this process, any heat added to the system can result in a change in volume and temperature, but the pressure does not change.
The work done by the system in an isobaric process can be expressed with the following equation:
\[ W = P \Delta V \]
Where:
- \( W \) is the work done by the system,
- \( P \) is the constant pressure,
- \( \Delta V \) is the change in volume of the system.
Additionally, using the first law of thermodynamics, we can express the change in internal energy (\( \Delta U \)) and the heat added to the system (\( Q \)) as follows:
\[ Q = \Delta U + W \]
In an isobaric process, we often relate the heat transfer to temperature change:
\[ Q = nC_P \Delta T \]
Where:
- \( n \) is the number of moles of the gas,
- \( C_P \) is the molar heat capacity at constant pressure,
- \( \Delta T \) is the change in temperature.
In summary, during an isobaric process, the pressure remains constant while the system can expand or contract, leading to heat transfer that results in temperature change.
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