Question

Energy is conserved. This means that in any system, _________. a) energy is constantly recycled b) total energy input equals total energy output c) light energy is released to replace the original input of solar energy d) high-quality energy input equals high-quality energy output

Answer 1

The law of conservation of energy states that the total energy of an isolated system remains constant. Regardless of energy transformations, the total energy of the system does not change.

Step-by-step explanation:

The law of conservation of energy states that the total energy of an isolated system remains constant. While energy may be transformed from one form to another, the total amount of energy does not change.

For example, consider a roller coaster. As it goes up a hill, its potential energy increases, and as it goes down the hill, its potential energy is converted to kinetic energy. Regardless of these energy transformations, the total energy of the roller coaster remains constant.

Therefore, the correct answer to the question is b) total energy input equals total energy output.

Answer 2

b) total energy input equals total energy output

Step-by-step explanation:

The first law of thermodynamics is a generalization of the conservation of energy in thermal processes. It is based on Joule's conclusion that heat and energy are equivalent. But to get there you have to get around some traps along the way.

From Joule's conclusion we might be tempted to call heat "internal" energy associated with temperature. We could then add heat to the potential and kinetic energies of a system, and call this sum the total energy, which is what it would conserve. In fact, this solution works well for a wide variety of phenomena, including Joule's experiments. Problems arise with the idea of ​​heat "content" of a system. For example, when a solid is heated to its melting point, an additional "heat input" causes the melting but without increasing the temperature. With this simple experiment we see that simply considering the thermal energy measured only by a temperature increase as part of the total energy of a system will not give a complete general law.

Instead of "heat," we can use the concept of internal energy, that is, an energy in the system that can take forms not directly related to temperature. We can then use the word "heat" to refer only to a transfer of energy between a system and its environment. Similarly, the term work will not be used to describe something contained in the system, but describes a transfer of energy from one system to another. Heat and work are, therefore, two ways in which energy is transferred, not energies.

In an isolated system, that is, a system that does not exchange matter or energy with its surroundings, the total energy must remain constant. If the system exchanges energy with its environment but not matter (what is called a closed system), it can do so only in two ways: a transfer of energy either in the form of work done on or by the system, either in the form of heat to or from the system. In the event that there is energy transfer, the change in the energy of the system must be equal to the net energy gained or lost by the environment.