A system gains 1500 J of heat, while the internal energy of...

A system gains $1500 \mathrm{~J}$ of heat, while the internal energy of the system increases by $4500 \mathrm{~J}$ and the volume decreases by $0.010 \mathrm{~m}^{3}$. Assume the pressure is constant and find its value.

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Key Concepts

First Law of Thermodynamics

This principle states that energy is conserved, and it expresses the relationship between the change in internal energy of a system, the heat added to the system, and the work done by (or on) the system. In thermodynamic processes, the overall energy change can be tracked by accounting for both heat transfer and work, which provides a foundational framework for analyzing energy interactions in thermal systems.

Work in Constant Pressure Processes

In processes where the pressure remains constant, the work done by or on the system is directly related to the change in volume. Specifically, the work is calculated as the product of the constant pressure and the change in volume. This relationship simplifies the analysis of energy transfer when the system undergoes expansion or compression under a fixed pressure environment.

Thermodynamic Sign Conventions

Understanding sign conventions is crucial because it determines how the work and heat terms are treated in energy equations. Typically, heat added to the system is taken as positive and work done by the system is considered positive, while work done on the system is negative (or vice versa, depending on the convention used). Clear interpretation of these signs helps in correctly applying the first law and in solving problems related to energy changes in a system.

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