entropy is greater the more possible arrangements for energy there are, which increases as the molecules become more mobile, so entropy is high in a gas, lower in a liquid, and lowest in a solid.
Gas, the actual values vary with temperature and pressure.
The entropy of H20 gas at standard atmospheric pressure is about 7.35 kj/kg*k and H20 liquid at 1 atmosphere is about 1.3 kj/kg*k.
because the particles have more freedom of movement in a liquid than they do in a solid.
Gas has the most, Liquid in the middle, and solid has the least
Gas has more entropy.
Gas
Gas
A+
A gas has the highest entropy.
Gas
Solid to liquid
Vapors always have more entropy than liquids of the same substance at the same temperature, because the number of energy states accessible to molecules in the vapor phase is much greater than in the liquid phase.
The products becoming more spread out.
It happens because, even in the same compound, atoms/molecules in different phases have different types of behaviour. For example, unlike solids, liquid and gas molecules can 'flow' around.
Entropy is a measure of the disorder or randomness in a system. The phase of matter with the highest entropy is generally considered to be the gas phase, as the particles in a gas have the highest degree of freedom and randomness compared to liquids and solids.
The transition of water (or of anything) from the liquid phase to the gas phase does constitute an increase in entropy.
Gas
The gas phase. That is true of any substance. Gases, because they are free to move about the entire volume of any container have much more entropy than either liquid or solids (and liquids have more than solids). The more ways the atoms are free to move around, the more entropy they have.
Solid to liquid
Vapors always have more entropy than liquids of the same substance at the same temperature, because the number of energy states accessible to molecules in the vapor phase is much greater than in the liquid phase.
Liquid may change into a vapor below the liquid's boiling point (or solid into vapor below the freezing point, think shrinking ice-cubes). This is a very difficult phenomanon the explain. The second law of thermodynamics explains that at every moment, the ammount of randomness of all matter in the universe is increasing. This randomness is called entropy. Entropy is a property of matter. The greater the number of locations and positions any given atom may randomly occupy at any given time, the greater that atom's entropy. This is to say that the molecules in a liquid would prefer to be in the vapor phase because it would increase their entropy. However, they're held down in the liquid phase because of the inter-molecular forces they experience between one another. If their temperature were higher, they would have enough energy (velocity) to escape the liquid phase. Luckily, at a given temperature, not every molecule has the same kinetic energy. There is actually a distribution of velocities (Maxwell-Boltzman distribution). The molecules having a high velocity manage to escape the intermolecular forces of the liquid phase and escape into the vapor phase. The higher energy molecules escaping the liquid phase decreases the average molecular velocity and causes the liquid temperature to decrease. This is why you feel cold after you get out of the shower. Your body heat is transferred to the water molecules which then evaporate The closer a liquid is to its boiling point, the greater the number of molecules there are that have enough kinetic energy to overcome the intermolecular forces and escape into the vapor phase, thus the higher the rate of evaporation.
Liquid phase: liquid water
The products becoming more spread out.
The liquid phase is preferable for drinks and solvents.
This phase is a liquid.
yes it is transition from the liquid phase to gas phase