If the internal energy (temperature) of a system increased, it could be due to

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To understand what can raise the internal energy (or temperature) of a system, recall the first law of thermodynamics: ΔU = Q − W, where Q is heat added to the system and W is work done by the system on the surroundings (positive when the system does work).

Option 1: 'heat was added to the system as heat' — When heat is transferred into the system (Q > 0), this adds energy to the system, increasing its internal energy and typically its temperature, assuming no phase change that absorbs heat without raising temperature. This aligns with the convention that positive heat input raises U.

Option 2: 'work was done to the system by the environment' — This phrasing describes the surroundings doing work on the system, which corresponds to W being negative from the system’s perspective (or equivalently, W_on_system > 0). In the ΔU = Q − W convention, a positive work input to the system (i.e., W negative for the system) effectively increases U, so the internal energy rises when the environment compresses or otherwise does work on the system.

If we consider the standard sign convention, both adding heat to the system and having the environment do work on the system are mechanisms that increase U. Conversely, removing heat (Q < 0) or the system doing work on the surroundings (W > 0) would decrease internal energy.

In summary, option 1 correctly describes a common mechanism for increasing internal energy, and option 2 correctly describes another mechanism (work done on the system). There are no other options provided to evaluate, so both listed possibilities are valid explanations for an increase in internal energy.

CLMTGR5001_002_2025_3 - Dynamics of Climate Variability and Chan PRACTICE QUIZ: Week 3 Lecture 2.2

If the internal energy (temperature) of a system increased, it could be due to

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