The temperature, pressure, and volume of gases can be related by the ideal gas equation. PV = nRT where P is pressure, V is volume, n is moles, R is that ideal gas constant, and T is the temperature in Kelvin.
At constant pressure, temperature is proportional to volume of the gas.
At constant temperature, volume is inversely proportional to pressure.
The first one is the real relation between the volume and temperature of gases.
Remember that temperature is a measure of how fast the molecules are moving.
PV / T = nR, n is number of moles and R is the ideal gas constant, so if the amount of gas remains constant, the Pressure and Volume are inversely proportional and their product is directly proportional to the kelvin temperature.
The pressure and volume of a gas are indirectly proportional. If pressure goes down, volume goes up. If volume goes up, pressure goes down.
The pressure and temperature of a gas are directly proportional. If pressure increases, temperature increases. If pressure decreases, temperature decreases.
The volume and temperature are also directly proportional. As volume increases, temperature increases. As volume decreases, temperature decreases.
In case of an ideal gas, which follows all gas laws at all temperatures, pressure, volume and temperature are related by the universal gas law.
P V = n R T
where P =>pressure
V =>volume
n=>number of moles of a gas
R=>universal gas constant
T=>temperature
when temperature increases, volume of a gas also increases when pressure increases, volume of gas decreases and vice versa (when pressure is reduced, the volume of the gas increases)
Charles Law (also known as the law of volumes) describes how gases tend to expand or contract with temperature changes.If the temperature changes and the gas molecules and pressure remains the same then the volume will increase or decrease at the same rate that the temperature changes.Since the temperature doubled the volume will double to 6L.
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.
Gases Boyle's law states that the Volume of a given amount of gas at constant Temperature varies inversely proportional to Pressure. You have a given volume of gas, and you double its pressure keeping Temperature constant, the volume will reduce by half.
If the temperature increases, then the volume of the gases cannot stay the same. The pressure will keep building until it overcomes the integrity of the container its contained in and causes an explosion.
DecreasesApex (:
Yes, for gases if the volume is known
Charles Law (also known as the law of volumes) describes how gases tend to expand or contract with temperature changes.If the temperature changes and the gas molecules and pressure remains the same then the volume will increase or decrease at the same rate that the temperature changes.Since the temperature doubled the volume will double to 6L.
Gases are highly compressible. So they don't have definite volume and pressure. As volume is reduced for a given mass pressure increases. Also as temperature changes then at constant volume pressure changes considerably. Same way for a constant pressure temperature change brings a change in the volume. Moreover gasses do not have a free surface.
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.
no, it depends on pressure and temperature as well
gases have no shape,volume water has volume but no shape solids have shape and volume gases have the most intermolecular space solids have least inter molecular space <><><><><> Temperature and pressure.
Volume increases! If pressure is kept constant then temperature and volume are directly related to each other.(Charle's law). It states that:V1/T1 = V2/T2
Pressure and temperature. As pressure increases, volume decreases; as temperature increases, volume increases with it. At standard temperature and pressure (1 atm, 273 degrees Kelvin), one mole of a gas (6.022 x 1023 particles) has the volume of 22.4 liters.
Guy-lussac's law
The following variables are directly proportional: Temperature and Pressure Temperature and Volume These variables are inversely proportional: Pressure and Volume
Gases are highly compressible. So they don't have definite volume and pressure. As volume is reduced for a given mass pressure increases. Also as temperature changes then at constant volume pressure changes considerably. Same way for a constant pressure temperature change brings a change in the volume. Moreover gasses do not have a free surface.
The volume of gases decreases with temperature; extrapolating the volume/temperature relationship, it looked as if all gases would reach a volume of zero at approximately the same temperature, about minus 273 degrees centigrade.