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Describe the Zeroth Law of Thermodynamics
The "zeroth law" states that if two systems are at the same time in thermal equilibrium with a third system, they are in thermal equilibrium with each other.
If A and C are in thermal equilibrium with B, then A is in thermal equilibrium with C. Practically this means that all three are at the same temperature, and it forms the basis for comparison of temperatures. It is so named because it logically precedes the First and Second Laws of Thermodynamics.
There are underlying ideas about heat associated with the zeroth law of thermodynamics, and one of those ideas was expressed by Maxwell as "All heat is of the same kind." If A is in thermal equilibrium with B, then every unit of internal energy that passes from A to B is balanced by the same amount of energy passing from B to A. This is true even if the atomic masses in A are different from those in B, and even if the amount of energy per unit mass in A is different because the material has a different specific heat. This implies that there is a measurable property that can be considered to be the same for A and B, a property upon which heat transfer depends. That property is called temperature.
Сформулируйте вопросы на английском языке и дайте ответы на них. Что такое внутренняя энергия?
What is the Internal Energy?
The internal energy of a system is identified with the random, disordered motion of molecules; the internal energy in a system includes potential and kinetic energy. This is contrast to external energy which is a function of the sample with respect to the outside environment (e.g. kinetic energy if the sample is moving or potential energy if the sample is at a height from the ground). The symbol for Internal Energy Change is ΔU.
Energy on a smaller scale:
Internal energy includes energy on a microscopic scale
It is the sum of all the microscopic energies such as:
translational kinetic energy
vibrational and rotational kinetic energy
potential energy from intermolecular forces
Internal Energy Change Equations ΔU = Q+W, where Q is heat and W is work.
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What is Heat?
The degree of hotness or coldness of a body or environment.
A measure of the warmth or coldness of an object or substance with reference to some standard value.
A measure of the average kinetic energy of the particles in a sample of matter, expressed in terms of units or degrees designated on a standard scale.
A measure of the ability of a substance, or more generally of any physical system, to transfer heat energy to another physical system.
Any of various standardized numerical measures of this ability, such as the Kelvin, Fahrenheit, and Celsius scale
The quantity of energy transferred as heat is a scalar expressed in an energy unit such as the joule (J), with a sign that is customarily positive when a transfer adds to the energy of a system. It can be measured by calorimetry.
Heat gained is equal to heat lost
Heat never flows from a cooler body to a hotter body of its own accord
Heat can never be taken from a reservoir without something else happening to the system