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Heat and Temperature
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Heat corresponds to the energy possessed by the atoms in a body, which can be interpreted as the oscillation they perform around their equilibrium point.
A measure of this energy is the body's temperature. If heat is supplied to a body, its temperature increases proportionally. The proportionality constant, which we call heat capacity, is in itself a function of the temperature.
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Mechanisms
Iframe
Heat and temperature are fundamental concepts in thermodynamics that represent different physical quantities. Heat is the energy transferred between systems or objects due to a temperature difference, flowing from hotter to cooler objects until thermal equilibrium is reached. It is measured in joules, calories, or British Thermal Units and is considered a path function, meaning it depends on the process of energy transfer. Heat can be transferred through conduction, convection, or radiation.
Temperature, on the other hand, is a measure of the average kinetic energy of the particles in a substance, indicating how hot or cold an object is. It is measured in degrees Celsius, Kelvin, or Fahrenheit, with Kelvin being the SI unit used in scientific contexts. Temperature is a state function, depending only on the current state of the system and not on the process used to reach that state. It determines the direction of heat flow, as heat moves from regions of higher temperature to lower temperature.
Mechanisms
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Microscopic heat
Description
Heat is nothing more than energy at a microscopic level.
In the case of a gas, it corresponds primarily to the kinetic energy of its molecules.
In liquids and solids, we must take into account the attraction between atoms, which is where potential energy comes into play. Therefore, in these cases, heat corresponds to the energy that particles have and with which they oscillate around the equilibrium point defined by the surrounding particles.
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Heat
Description
Heat is associated with elements like fire, which causes the temperature of water to rise. The process of heating generates movement, indicating that heat is related to mechanical energy. Even the handle of a pot gets heated, and our bodies are capable of perceiving that temperature. Moreover, fire emits radiation that heats up objects that are exposed to it.
From this, we can infer that by transferring heat, we can raise the temperature of an object, and that the generation of movement is associated with energy.
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Temperature
Description
Temperature is a measure of the energy contained within an object and is associated with the oscillations of molecules/atoms in solids and liquids, and with the movement of these particles in gases and liquids.
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Model
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Parameters
Variables
Calculations
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Calculations
Calculations
Variable 
Given Calculate 
Target : Equation To be used 
Equations
$ \Delta Q = C \Delta T $
DQ = C * DT
$ \Delta Q = Q_f - Q_i $
DQ = Q_f - Q_i
$ \Delta T = T_f- T_i$
DT = T_f - T_i
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Temperature Difference (Kelvin)
Equation
If a system is initially at ($$) and then is at the temperature in final state ($T_f$), the difference will be:
| $ \Delta T = T_f- T_i$ |
The temperature difference is independent of whether these values are in degrees Celsius or Kelvin.
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Heat difference
Equation
If a body initially has an amount of heat the initial heat ($Q_i$) and subsequently has an amount of heat the final heat ($Q_f$) ($Q_f > Q_i$), heat has been transferred to the body the heat difference ($\Delta Q$). Conversely, if ($Q_f < Q_i$), the body has released heat.
| $ \Delta Q = Q_f - Q_i $ |
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Caloric content
Equation
When the heat supplied to liquid or solid ($\Delta Q$) is added to a body, we observe a proportional increase of the temperature variation in a liquid or solid ($\Delta T$). Therefore, we can introduce a proportionality constant the heat capacity ($C$), known as heat capacity, which establishes the following relationship:
| $ \Delta Q = C \Delta T $ |
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