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If temperature remains constant throughout the reaction, then it is said to be isothermal. In a reversible reaction, the external pressure equals the internal pressure of the container, and the external pressure is increased or decreased in small increments. In a irreversible reaction, there is a noticeable difference between the external pressure and internal pressure.
Yes. Also, because in reversible reactions, you increase/decrease the pressure by small increments, that explains why we must use w=-nRTln(V2/V1) since pressure will not be constant. However, because in irreversible reactions, the external pressure remains constant, we use w=-PdeltaV because the external pressure is constant.
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