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<h2>Heat</h2>
<p>In <a data-page="42" href="https://app.ulearngo.com/tutorials/work-energy-energy-resources/">Work, Energy, and Energy Resources</a>, we defined work as force times distance and learned that work done on an object changes its kinetic energy. We also saw in <a data-page="93" href="https://app.ulearngo.com/tutorials/temperature-kinetic-theory-gas-laws/">Temperature, Kinetic Theory, and the Gas Laws</a> that temperature is proportional to the (average) kinetic energy of atoms and molecules. We say that a thermal system has a certain internal energy: its internal energy is higher if the temperature is higher. If two objects at different temperatures are brought in contact with each other, energy is transferred from the hotter to the colder object until equilibrium is reached and the bodies reach thermal equilibrium (i.e., they are at the same temperature). No work is done by either object, because no force acts through a distance. The transfer of energy is caused by the temperature difference, and ceases once the temperatures are equal. These observations lead to the following definition of <strong>heat</strong>: Heat is the spontaneous transfer of energy due to a temperature difference.</p>
<p>As noted in <a data-page="93" href="https://app.ulearngo.com/tutorials/temperature-kinetic-theory-gas-laws/">Temperature, Kinetic Theory, and the Gas Laws</a>, heat is often confused with temperature. For example, we may say the heat was unbearable, when we actually mean that the temperature was high. Heat is a form of energy, whereas temperature is not. The misconception arises because we are sensitive to the flow of heat, rather than the temperature.</p>
<p>Owing to the fact that heat is a form of energy, it has the SI unit of <em>joule</em> (J). The <em>calorie</em> (cal) is a common unit of energy, defined as the energy needed to change the temperature of 1.00 g of water by \(1\text{.00ºC}\) —specifically, between \(\text{14}\text{.5ºC}\) and \(\text{15}\text{.5ºC}\), since there is a slight temperature dependence. Perhaps the most common unit of heat is the <strong>kilocalorie</strong> (kcal), which is the energy needed to change the temperature of 1.00 kg of water by \(1\text{.}\text{00ºC}\). Since mass is most often specified in kilograms, kilocalorie is commonly used. Food calories (given the notation Cal, and sometimes called “big calorie”) are actually kilocalories (\(1\phantom{\rule{0.25em}{0ex}}\text{kilocalorie}\phantom{\rule{0.25em}{0ex}}\text{=}\phantom{\rule{0.25em}{0ex}}\text{1000 calories}\)), a fact not easily determined from package labeling.</p>
<div class="fig_container" id="navlink_id862880"><img alt="In figure a there is a soft drink can and an ice cube placed on a surface at a distance from each other. The temperatures of the can and the ice cube are T one and T two, respectively, where T one is not equal to T two. In figure b, the soft drink can and the ice cube are placed in contact on the surface. The temperature of both is T prime. " src="https://data.ulearngo.com/assets/f51bbf7a-c3cf-4cd9-951c-138cf3578ee4"/>
<p class="fig_caption">In figure (a) the soft drink and the ice have different temperatures, \({T}_{1}\) and \({T}_{2}\), and are not in thermal equilibrium. In figure (b), when the soft drink and ice are allowed to interact, energy is transferred until they reach the same temperature \(T\prime \), achieving equilibrium. Heat transfer occurs due to the difference in temperatures. In fact, since the soft drink and ice are both in contact with the surrounding air and bench, the equilibrium temperature will be the same for both.</p>
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Physics is a science discipline concerned with the nature and properties of matter and energy. Physics topics include mechanics, heat, light and radiation, sound, electricity, magnetism, the structure of atoms, and so on.

Physics

Heat

Discover the principles of heat and learn about the various methods of heat transfer, including conduction, convection, and radiation, as well as the mechanics of latent heat and temperature change in this tutorial.


Heat

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