the energy of the universe if constant; same as law of conservation of energy
See Law of Conservation of Energy.
One of the two Laws of Thermodynamics which states that the amount of matter and energy in a system remains constant. Matter is transformed to energy and vice versa. Neither matter not energy can be destroyed nor be produced from zero.
the change in internal energy of a system is the difference between the heat taken in by the system and the work done by the system (see equation 13.1)
Essentially a restatement of energy conservation, it states that the change in the internal energy of a system is equal to the heat added plus the work done on the system.
The fact, based on irrefutable observations, that energy is never created or destroyed, but may be converted from one form to another, e.g., electricity to light. Also called the Law of Conservation of Energy. (See also Second Law of Thermodynamics.)
In any physical or chemical change, no detectable amount of energy is created or destroyed, but in these processes energy can be changed from one form to another; you cannot get more energy out of something than you put in; in terms of energy quantity, you cannot get something for nothing (there is no free lunch). This law does not apply to nuclear changes, in which energy can be produced from small amounts of matter. See also second law of thermodynamics.
A statement of the relationship between the internal energy of a system and the heat and work transferred from the system to its surroundings, or vice versa: Esys = q + w.
The total amount of energy in the universe remains constant; more energy cannot be created and existing energy cannot be destroyed; energy can only undergo conversion from one form to another.
the fundamental principle of physics that the total energy of an isolated system is constant despite internal changes
A statement of the conservation of energy for thermodynamic systems. The fundamental form requires that the heat absorbed by the system serve either to raise the internal energy of the system or to do work on the environment.
a law stating that the energy of the universe is constant.
States that energy is conserved; that is, it is neither created nor destroyed under normal conditions.
Energy can neither be created nor destroyed in the Universe but it can be converted from one form to another. Also called the Law of Conservation of Energy
The amount of work done on or by a system is equal to the amount of energy transferred to or from the system.( 010)
Energy can neither be created or destroyed.
the law of physics that states that the heat absorbed by a system either raises the internal energy of the system or does work on the environment
the total amount of energy and mass in the universe is constant; energy and mass can be neither created nor destroyed.
After the initial creation of the universe ex nihilo, no matter or energy can be created or destroyed. [See Second Law of Thermodynamics.
The law of conservation of energy, which states that energy is neither created nor destroyed, but merely transformed from one state to another or converted to or from matter.
Energy cannot be created or destroyed; it can only be converted from one form to another. For example, the potential chemical energy in coal can be converted in thermal energy.
Energy is neither created nor destroyed; it changes from one form to another.
Energy cannot be created or destroyed, but only transformed from one form to another. The process of transformation of energy is never totally efficient, and some energy is always converted into heat.
States that energy cannot be created or destroyed, but only changed from one form to another. First Law efficiency measures the fraction of energy supplied to a device or process that it delivers in its output. Also called the law of conservation of energy.
The total internal energy of an isolated system is constant. If a thermodynamic system is not isolated, its internal energy may change because of two distinguishable macroscopic processes: working (a force exerted through a distance) and heating ( energy exchange by virtue of a temperature difference between the system and its surroundings). The first law may be written where is the rate of heating and is the rate of working on the system. For a simple system in which working is solely a consequence of volume changes, the rate of working is given by where is pressure and is volume, provided volume changes at a sufficiently slow rate (quasi- static process) that the pressure is approximately uniform.
The first law of thermodynamics is an expression of the universal law of conservation of energy, and identifies heat transfer as a form of energy transfer.