Energy is transferred or moves from one object or place to another. This is what we refer to when we say that energy "flows". For example, when a burner on your stove is hot, the heat (thermal) energy flows or is transferred from the burner to a pan, or the room, or maybe even your hand. Another example is when a moving object, such as a cue ball, strikes a none moving object, the eight ball, causing the eight ball to move. Thus some of the energy of the cue ball (kinetic energy) is transferred to the eight ball. As you can see there are different forms of energy...two are described above. To further complicate things energy changes form and this contributes to the idea of energy flow. Here is an example of energy flowing through a system by transfer and transformation. The chemical energy stored in natural gas is transformed into thermal energy when the gas burns in a stove burner. The thermal energy of the burning gas is transfered to the pan and transfered again to the water inside the pan. As the water in the pan gets hotter and begins to boil, the steam causes the lid on the pan to move (rattle about as the pan of water is rapidly boiling). Since the lid is moving, it has kinetic energy. Energy flowed in this example as it moved from the gas to the pan to the water to the lid. Several changes we required for energy to flow through this system. Energy changed form (transformed) from chemical energy to thermal energy to kinetic energy. Keep in mind that I left a few things out...like the electomagnetic energy also released when the gas burned and the fact that thermal energy is also is best understood in terms of moving particles.
an action or device that has an input of energy in order to do work and have a useful output.
example:
clapping hands (to make noise)
mechanical energy(input), (then) sound energy (useful output) + thermal energy (waste output)
Energy flows from the greatest concentration of energy to lower concentrations of energy. This causes entropy to increase. This flow from greater to lower concentrations is true for thermal energy, radiant energy, heat energy, energy of all types. This continues until entropy is maximum.
You can store energy by doing work. And if you have energy in your body (or a system) you can do work using the energy.
When heat is added to or is absorbed by a system, its internal energy increases. The amount of external work a system can do essentially refers to the amount of energy it can transfer to something else. So when internal energy increases, so does the external work done by the system.
work done on the system: when a surrounding does work on the system the total energy increases so work done is positive..........
It helps to think of work as "transfer of energy". If you do energy on a system, its energy content increases. If the system does work on something else, the system's energy content decreases.
Assuming you are talking about a closed system, it is the difference in energy transferred to or from the system as work and HEAT.
Energy is the potential to do some work. If there is work done on a system, this work done is stored as potential energy of the system. If the system in motion, it should have kinetic energy. Hence total energy of the system PE+KE
You can store energy by doing work. And if you have energy in your body (or a system) you can do work using the energy.
When heat is added to or is absorbed by a system, its internal energy increases. The amount of external work a system can do essentially refers to the amount of energy it can transfer to something else. So when internal energy increases, so does the external work done by the system.
work done on the system: when a surrounding does work on the system the total energy increases so work done is positive..........
It helps to think of work as "transfer of energy". If you do energy on a system, its energy content increases. If the system does work on something else, the system's energy content decreases.
If work is done adiabatically on a system, the internal energy will increase. This is because adiabatic processes do not involve the exchange of heat with the surroundings, so any work done on the system will directly contribute to an increase in its internal energy.
Assuming you are talking about a closed system, it is the difference in energy transferred to or from the system as work and HEAT.
remains constant From Rafaelrz. When a simple closed system does work and no heat is added, the temperature of the system will drop. This is because the work is done at the expense of his internal energy, which is thermal energy.
Energy
Usually the "thermal energy" will increase since work ON the system adds energy. Thermal energy is really not the best term though. A much better term in thermodynamics would be ENTHALPY.
Physics. the capacity to do work; the property of a system that diminishes when the system does work on any other system, by an amount equal to the work so done; potential energy. Symbol: E e= mc2
If the internal energy of the system increases the temperature will increase.