Answer:
Kinetic energy increases.
Explanation:
In a solid, molecules do not have much room to move. They are very slow moving, which means that kinetic energy is low. In a liquid, molecules have more room to move. They are able to move faster than a solid, which means that kinetic energy is low.
From greatest to lowest kinetic energy:
gas, liquid, solid
Answer:the Boundary of an advancing mass of warm air, in particular the leading edge of the warm sector of a low-pressure system.
Explanation:
Answer:
No matter if you are on Earth, the moon or just chilling in space, your mass does not change. But your weight depends on the gravity force; you would weigh less on the moon than on Earth, and in space you would weigh almost nothing at all.
Answer: Gases are complicated. They're full of billions and billions of energetic gas molecules that can collide and possibly interact with each other. Since it's hard to exactly describe a real gas, people created the concept of an Ideal gas as an approximation that helps us model and predict the behavior of real gases. The term ideal gas refers to a hypothetical gas composed of molecules which follow a few rules:
Ideal gas molecules do not attract or repel each other. The only interaction between ideal gas molecules would be an elastic collision upon impact with each other or an elastic collision with the walls of the container. [What is an elastic collision?]
Ideal gas molecules themselves take up no volume. The gas takes up volume since the molecules expand into a large region of space, but the Ideal gas molecules are approximated as point particles that have no volume in and of themselves.
If this sounds too ideal to be true, you're right. There are no gases that are exactly ideal, but there are plenty of gases that are close enough that the concept of an ideal gas is an extremely useful approximation for many situations. In fact, for temperatures near room temperature and pressures near atmospheric pressure, many of the gases we care about are very nearly ideal.
If the pressure of the gas is too large (e.g. hundreds of times larger than atmospheric pressure), or the temperature is too low (e.g.
−
200
C
−200 Cminus, 200, start text, space, C, end text) there can be significant deviations from the ideal gas law.
Explanation:
