Thermal energy and temperature are closely related but distinct concepts in thermodynamics.
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Thermal Energy: This refers to the total kinetic energy of all the particles in an object due to their motion and interactions. It depends on the mass of the object, the type of substance, and the amount of particle motion. Thermal energy can change based on factors such as heat transfer, phase changes, or varying particle movements.
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Temperature: This is a measure of the average kinetic energy of the particles in a substance. It provides an indication of how hot or cold an object is and is a scale for quantifying thermal energy. Temperature is typically measured in degrees Celsius (°C), Kelvin (K), or Fahrenheit (°F).
Relationship:
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Temperature vs. Thermal Energy: While temperature gives an average measure of the kinetic energy of particles, thermal energy is the sum of all kinetic energies of the particles in a substance. Thus, two objects can have the same temperature but different thermal energies if their masses are different (for example, a small pot of water and a large pot of water at the same temperature).
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Higher Temperature Indicates Higher Thermal Energy: Generally, as the temperature of an object increases, its thermal energy increases as well, assuming the object remains in the same phase (solid, liquid, gas).
In summary, while temperature and thermal energy are related, they are not the same thing; temperature measures the average energy of particles, while thermal energy is the total energy due to all the particles in a system.
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