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In a closed system the pressure is directly proportional to the temperature (Gay-Lussac law).At higher temperature the volume tend to increase but in a container the volume is limited.
In a container the volume remain constant but the pressure increase.
A gas will expand to fill up any volume available to it. Think of rigid containers that will not change shape or volume. If you have 10 completely empty containers that can be connected. Inside each is a vacuum. Place some gas in the first container. It completely fills the container and creates some pressure. Connect a second container and some of the gas leaves the first container, but not all of the gas. The gas will completely fill both containers, but creating less pressure. Continue connecting containers, and the same appens every time. The gas completely fills every container that is connected and the pressure 'adjusts' on its own to reach a new equilibrium pressure.
Because the pressure increases The real answer is: Charles's Law. He found that if you increase the temperature of a constant pressure the volume increases also.
0.783 g of hydrogen gas is placed in an container of volume 657 mL at a temperature of 342 K. What is the pressure in atm?
it would change the pressure exerted by the gas in the container.
False. Gases in a container take the shape of the container. The volume of a gas increases with temperature and inversely with pressure, except when in a closed container where volume remains the same as the volume of the container and the temperature and pressure will vary.
If temperature increases, either the volume or the pressure must increase. Since you have limited the volume by closing the container, pressure must increase.
In a closed system the pressure is directly proportional to the temperature (Gay-Lussac law).At higher temperature the volume tend to increase but in a container the volume is limited.
If the volume of a container of air is reduced by one half the partial pressure of the oxygen with in the container will be doubled. If the volume of a container of gas is reduced, the pressure inside the container will increase.
The mass of the gass, the volume of the container holding the gas, and the temperature of the gass. If you have a container of gas, the greater the mass of the gas, the more molecules there are in the container, and this leads to greater pressure. If you have a fixed mass of gas, changing the volume of the container holding the gas will cause the pressure to change. Increasing the volume of the container decreases the pressure. Decreasing the volume of the container increases the pressure. If you increase the temperature of a gas without changing its mass or volume, pressure increases.
In a container the volume remain constant but the pressure increase.
A gas will expand to fill up any volume available to it. Think of rigid containers that will not change shape or volume. If you have 10 completely empty containers that can be connected. Inside each is a vacuum. Place some gas in the first container. It completely fills the container and creates some pressure. Connect a second container and some of the gas leaves the first container, but not all of the gas. The gas will completely fill both containers, but creating less pressure. Continue connecting containers, and the same appens every time. The gas completely fills every container that is connected and the pressure 'adjusts' on its own to reach a new equilibrium pressure.
Increasing the temperature of a gas will increase it's pressure ONLY if the volume is held constant.
If the volume stays the same, the pressure will decrease.
The pressure of the gas increase.
The pressure increases. Hopefully, the container is strong enough to withstand the increased pressure. If there is a weakness in the container, gas will escape as a leak.