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Richie Smash
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Hello, I would like to know, why is the volume of gas produced during phase change significantly more than the original volume of the liquid being used? Say water changing phase at 1atm.
Is there a way to show that ?Khashishi said:Gas molecules don't necessarily have more kinetic energy than liquid
The equipartition theorem states that the average energy in a mode is ##\frac{1}{2} kT##. So, the energy per degree of freedom is the same for a gas and liquid at equilibrium. But, if you want a complete answer, you need to know how many modes there are.BvU said:Is there a way to show that ?
The volume of a gas increases during a phase change because the molecules of the gas are able to move more freely and are less constrained by intermolecular forces. This allows the molecules to spread out and take up more space, resulting in an increase in volume.
The expansion of a gas during a phase change is caused by an increase in the average kinetic energy of the gas molecules. As the temperature increases, the molecules gain more energy and move faster, leading to an increase in volume.
During a phase transition, such as from a liquid to a gas, the volume of the gas increases significantly. This is because the molecules are transitioning from a more compact liquid phase to a more spread out gaseous phase, resulting in an increase in volume.
When a gas undergoes a phase change to become a liquid, the molecules lose a significant amount of kinetic energy and are forced to come closer together due to intermolecular forces. This results in a decrease in volume as the molecules become more tightly packed.
According to Boyle's Law, the volume of a gas is inversely proportional to the pressure exerted on it. During a phase change, there may be a change in pressure due to a change in temperature or external factors, which can also impact the volume of the gas. As pressure increases, the volume of the gas decreases and vice versa.