a. phase diagram - A phase diagram is a graph showing how phases are affected by changes in temperature or pressure.
b. triple point - The triple point is the temperature and pressure at which all three phases exist simultaneously.
c. kinetic energy - Kinetic energy is the energy of motion, represented as K.E. = 1/2 mv^2, where m is mass, and v is the velocity of the particle in motion.
d. temperature - Temperature is an indicator of average kinetic energy.
e. phase equilibrium - Phase equilibrium is the state achieved when the exchange of molecules between two phases occurs at the same rate.
f. Kinetic Molecular Theory - Kinetic Molecular Theory is the theory that attempts to explain gas behavior at the molecular level.
g. evaporation - Evaporation is a dynamic situation when the number of molecules leaving the liquid is greater than the number returning.
A phase diagram is a graphical representation that illustrates how the phases of a substance are influenced by changes in temperature and pressure. It provides valuable insights into the conditions under which a substance exists as a solid, liquid, or gas. The triple point, designated as the temperature and pressure at which all three phases coexist in equilibrium, serves as a reference point for phase transitions.
Kinetic energy, a fundamental concept in thermodynamics, represents the energy associated with the motion of particles. Temperature, on the other hand, is a measure of the average kinetic energy of particles in a system. According to the Kinetic Molecular Theory, which aims to explain gas behavior at the molecular level, particles in gases are in constant motion, and their behavior can be understood through principles such as temperature and kinetic energy.
Phase equilibrium occurs when the exchange of molecules between two phases, such as liquid and vapor, transpires at the same rate, establishing a dynamic balance. Evaporation, a process in which molecules leave a liquid and enter the vapor phase, is a manifestation of kinetic energy, specifically when the number of molecules leaving the liquid surpasses those returning.