More. That is the only answer that is possible with the information provided. The ideal gas law states: PV=nRT. Solving for P gives: P=(nRT)/V. So you can see that if temperature and amount of gas are constant (R is always a constant), decreasing V will increase pressure and increasing V will decrease pressure. An easier formula derived from this one is P1V1=P2V2.
The gas takes on the size and shape of the container it's in. So if you make the volume of the container smaller (compress it) the volume of the gas is smaller as well. However, this comes at a higher pressure exerted, so there is no spontaneous mass creation.Well, by definition, compress means "to make smaller; to press or squeeze together; or to make something occupy a smaller space or volume." Therefore, the very word "compress" implies a decrease in volume. So if you wanted to know what happens when you compress a gas, you are squeezing it into a smaller space, or decreasing the volume.If you were to let the gas maintain a constant temperature as you compress it, then pressure would increase. If you were to let the gas maintain a constant pressure, then temperature would decrease.If you were to rephrase your question to "what happens to the volume of gas if put under pressure," then the gas' volume would decrease. For the temperature to remain constant and the pressure to increase, a gas must decrease in volume to occupy a smaller area.
17 l
Assuming it's a bag of gas at constant temperature, four times the volume by the relationship: P1V1 = P2V2
Air temperature and air pressure are inversely proportional. As temperature increases, air pressure decreases. This is best demonstrated in an enclosed vessel.
We usually apply the term compression to the act of squeezing a fluid to force it into a smaller volume or increase its pressure. The term applies to gases as well as fluids.
Here we consider a system as an open system .Now air forms the remaining system lwhich occupies remaining volume .;the considered system being small with respect to the volume enclosed by air ,there exists force exerted by air on this system in order to cover up the entire volume.----this is nothing but pressure
You cannot stretch a gas. If you extend the volume in which some gas is enclosed you are working against the difference in between the external atmospheric pressure and the internal pressure of the gas. As you increase the enclosed volume, the pressure inside there falls and you have to work harder.
DENSER MORE PRESSURE PRESSURE PRESSURE LOOK AT SCIENCE TEXT BOOK DONT CHEAT ON WIKI Water has more density than air.
The volume decreases (smaller,less)
For an enclosed gas (contained in a fixed volume), the pressure increases as temperature increases.Another way to picture this is that at higher temperatures, the gas molecules colliding with the walls of the container are more energetic, so the force exerted (pressure) is greater.
Kinetic theory explains the pressure that a gas exerts on the walls of its container. This describes elastic collisions between the atoms or molecules in the gas with the container's walls, which collectively exert a measureable pressure.
According to Boyle's law, the pressure of a gas depends on its volume, so if you lower the volume, the pressure increases.
Area enclosed by the PV (pressure-volume) and TS (temperature-entropy) diagrams shows the work done by the system.
If the temperature remains constant, decreasing the volume will increase the pressure.
because a ship has big volume and a coin has small volume hence the smaller the area the bigger the pressure,the smaller the area the big the volume
Boyle's Law, named after Robert Boyle, explains this phenomenon. This law states that the product of volume and pressure remains constant under constant temperature. Thus, a decrease in pressure will yield an increase in volume to compensate.
The force of the pressure put on the balloon is squeezed into smaller particles so the volume is smaller. :) From Jade Nicole White. X