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Thermodynamics tells us that ΔT is proportional to ΔE, so what's the problem?
You need to combine 0, 1 and 2.
Simply, we can say that in an isothermal processT = constanthttps://en.m.wikipedia.org/wiki/Isothermal_processExample
Only some portion of the energy of an object is manifested as its temperature.
Quote from: hamdani yusuf on 21/08/2024 09:43:08Only some portion of the energy of an object is manifested as its temperature.Note the conventional use of Δ.
(Specific) heat capacity. Assuming no phase change, of course.
Over the humanly survivable temperature and pressure range, say -40 to + 150F and 14.5 psi, the curve looks flat enough to me.
Heat capacity and entropy share the same units because they are both derived from the fundamental relationship between energy and temperature in thermodynamic processes.### Units of Heat Capacity- **Heat Capacity (C)** is defined as the amount of heat required to change the temperature of a substance by one degree. Mathematically, it is expressed as: \[ C = \frac{Q}{\Delta T} \] where \( Q \) is the heat added, and \( \Delta T \) is the temperature change. Since \( Q \) is measured in joules (J) and \( \Delta T \) in kelvins (K), the unit of heat capacity is joules per kelvin (J/K).### Units of Entropy- **Entropy (S)** is a measure of the disorder or randomness of a system. In thermodynamics, it is related to the amount of heat exchanged in a reversible process at a constant temperature. The change in entropy is given by: \[ \Delta S = \frac{Q_{\text{rev}}}{T} \] where \( Q_{\text{rev}} \) is the reversible heat exchange, and \( T \) is the absolute temperature. Here, \( Q_{\text{rev}} \) is in joules (J), and \( T \) is in kelvins (K), making the unit of entropy also joules per kelvin (J/K).### Why They Share the Same UnitsBoth heat capacity and entropy involve the relationship between energy (heat) and temperature. The similarity in units arises because both quantities describe how energy (measured in joules) is distributed with respect to temperature (measured in kelvins):1. **Heat Capacity** measures how much energy is needed to change the temperature of a substance, indicating the energy absorption efficiency.2. **Entropy** measures how energy is distributed at a specific temperature, representing the disorder or randomness of the system.Although they describe different physical concepts?heat capacity deals with energy absorption, while entropy deals with energy distribution?they both fundamentally relate energy to temperature, leading to the same units (J/K).
BC was talking about heating a room in his house because it was uncomfortably cold.
Over the humanly survivable temperature and pressure range, say -40 to + 150F and 14.5 psi, the curve looks flat enough to me. And IIRC the special air in your room was an ideal gas.
Anyway, apropos setting fire to something with light beam, you are adding energy to the target by irradiating it with electromagnetic radiation. What isn't scattered or reflected either induces a chemical change or just heats the target.Thermodynamics tells us that ΔT is proportional to ΔE, so what's the problem?I spent many happy years measuring ΔT induced by x- and γ-rays absorbed in carbon and water - it's how we define radiation dose.