Let us note that in a non-stationary problem, the isothermal surface is mobile in time.
The temperature field also allows a very important vector to be defined, whose use will be explained later on: temperature gradient.
Initially, we define this vector in a Cartesian system. Later on, we will see that it is quite easy to determine its components in other systems when the symmetries in a problem make that a pertinent option.
In a Cartesian system, this gradient is constructed by taking, for each of its components, the partial derivative of the temperature with respect to the relevant coordinate axis. In other words:
[1.2]
For other systems, it will be useful to refer to Appendix 2.
This mathematical operation is known to all physicists. With a minus sign, it is the derivation of a force from a potential.
We should note that in a stationary problem, this gradient is a vector attached to each point in space and fixed in time. In the case of a non-stationary problem, this gradient is a vector attached to each point in space and variable in time.
The temperature gradient possesses a fundamental property, which is demonstrated in Appendix 2: the gradient vector is normal at each point in space to the isothermal surface that passes through this point.
This property will be familiar to those who have studied electric fields.
1.2.2. Flow and density of flow
These two essential parameters will be used throughout this book.
Thermal flow Φ is the quantity of heat Q that passes a given surface in a unit of time:
[1.3]
This flow is expressed in Joules per second (J.s-1) or even better, in Watts (W).
Density of the thermal flow φ, which can be even greater, is the flow that passes through a unit of surface:
[1.4]
This flow density is expressed in Watt per m2 (W.m-2).
It is important not to confuse these two parameters, which also do not have the same units.
In this book, we will systematically note the flow with a capital Φ and the flow densities with a lowercase φ.
These flows and flow densities may not be uniform through a surface, which can also vary rapidly over time. We then deal with a definition on a differential basis, through small surface areas and with small time intervals.
Through a small surface d S:
[1.5]
[1.6]
The quantity of heat d2Q is measured on a small surface d S and on a small time interval d t, which becomes twice differential. The flow d Φ (t) becomes differential since it is the relationship of a twice differential quantity by a small surface d S at a given time t. The flow density φ is the relationship between two differential quantities, which remains finite (expressed in flow per unit of surface and time).
1.3. Relation to thermodynamics
We have already pointed out that when we talk about thermal science, thermodynamics is not far off. More precisely, it is its main principle.
Before the first principle, there was calorimetry.
We should be aware that each time that we draw up a balance for an environment, which will be particularly true in Chapter 4, we link a variation in temperature to an exchange of heat by a calorimetric operation.
1.3.1. Calorimetry
Calorimetry was, in fact, born before the first principle. We (mainly chemists) noted that the relative variations in temperature due to an exchange of what we had then designated as “heat”, depended on the mass m of the environments and a coefficient that is today denoted as the mass calorific capacity c. In other words, when a body transfers heat to another body, the relationship (with an obvious notation) is:
[1.7]
The minus sign indicates that one body is cooling and the other is heating.
This leads to the relationship between the quantity of heat Q given to a body and its rise in temperature ΔT (or the inverse in the case of cooling), which can be written as:
[1.8]
1.3.2. The first principle
Later on, Joule will demonstrate the equivalence of two forms of energy: work and heat.
His experiment can be reproduced on a daily basis. It is sufficient to turn a small paint mixer in water contained in a Thermos flask. Why a Thermos? So that the heat given to the water does not escape.
We measure the electrical energy provided to an engine for a certain time, with energy measuring the work “given” to the water. The heating of the water whose mass and calorific capacity are known measures the quantity of heat brought to the water. This quantity of heat can only come from the transformation of work provided through heat. In Joule’s era, heat was measured in calories.
One calorie raised the temperature of 1 gram of water by 1 degree Celsius. Work is evaluated in Joules. Modestly, this author only had a kilogram meter.
Hence, two conclusions will always be in the background of our study:
– qualitatively: work and heat are two equivalent and interchangeable forms of energy;
– quantitatively: the equivalence between a calorie and (today) a Joule is written as:
[1.9]
In principle, this is part of the repertoire of all high school pupils, but it is not a bad thing to give a reminder of it.
1.3.3. The second principle
This principle is about quality and reversibility. It is easy to transform work into heat. Simple friction is sufficient. This is what Joule experienced.
It is more complicated to transform heat into work. Several sources are required, at least one hot and one cold, and the temperature of the sources becomes important. Moreover, we never recover all the heat that we provide with the hot source in work. We always “throw” some into the cold source. This will be the large Carnot work, among others.
Those who have closely read the text at the end of our preamble will understand why. The blades of the mixer transform a “directed” energy into a chaotic thermal agitation. Chaos will also never spontaneously return to order.
All this comes from the genius (we defend our choice