the total number of molecules in each phase stays constant
Static equilibrium refers to a system at rest where all forces are balanced, while dynamic equilibrium refers to a system in motion where the rate of change is constant. In static equilibrium, objects are stationary, while in dynamic equilibrium, objects are moving at a constant speed and direction.
The temperature at which the rate of evaporation equals the rate of condensation is known as the equilibrium vapor pressure. At this temperature, the vapor pressure of a liquid is equal to the external pressure, leading to a dynamic equilibrium between the liquid and vapor phases.
The two kinds of equilibrium are static equilibrium, where an object is at rest with no linear or angular acceleration, and dynamic equilibrium, where an object is moving at a constant velocity with no linear or angular acceleration.
A fan moving with uniform angular speed is in dynamic equilibrium. This is because even though the fan is rotating at a constant rate, there are still forces acting on it to keep it moving in a circular path, such as air resistance and friction.
An object in dynamic equilibrium has equal and opposite forces acting on it, resulting in no net acceleration. This means the object is either at rest or moving at a constant velocity. In this state, the object's internal and external forces are balanced, allowing it to remain in equilibrium.
reactants are turning into products. products are turning into reactants.
the total number of molecules in each phase stays constant
The two types of equilibrium are static equilibrium and dynamic equilibrium. Static equilibrium is when an object is at rest, while dynamic equilibrium is when an object is moving at a constant velocity with no acceleration. Static equilibrium involves balanced forces in all directions, while dynamic equilibrium involves balanced forces with movement.
On a phase diagram, the conditions of pressure and temperature at which two phases coexist in equilibrium are represented by a line. This line is called the phase boundary or phase equilibrium line. It separates the regions where the two phases exist in equilibrium from the region where only one phase is present.
The triple point on a phase diagram represents the temperature and pressure conditions at which all three phases of a substance (solid, liquid, and gas) coexist in equilibrium. At the triple point, the substance can exist in a state where all three phases are present simultaneously. This point is unique for each substance and is a precise combination of temperature and pressure.
the total number of molecules in each phase stays constant
Two phases are at equilibrium when the rate of their interconversion is equal in both directions. This means that the amount of substance transitioning from one phase to another is the same in both directions, resulting in a stable balance between the phases.
By a line separating the phases
Equilibrium is referred to as dynamic because in a system at equilibrium, the forward and reverse reactions are occurring at the same rate. This means that while it appears that there is no net change in the concentrations of reactants and products, molecules are constantly being converted back and forth between the two states.
The maximum number of phases that can be in mutual equilibrium is three.
Dynamic equilibrium is important because it indicates that a reaction has stabilized.
semi-circular canals for dynamic equilibrium and vestibule for static equilibrium