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What would you do to the volume of a gas to reduce its pressure to one quarter of the original value?
Wiki User
∙ 8y ago
You could increase its volume or cool it or both.
Wiki User
∙ 8y ago
Wiki User
∙ 8y agoIncrease it by 4 times.
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What is difference between compressibility factor and super compressibility factor?
An ideal gas will have a volume that is inversely proportional to the pressure (assuming constant temperature). For example, if you double the pressure, the volume will be reduced to 1/2 the original volume. For real gases, the behavior is usually somewhat different. In some cases, if you double the pressure, the volume will reduce to LESS than 1/2 the original volume. This is due to the attraction between the molecules, and this phenomenon is called "supercompressibility".
What would happen to the volume of the gas inside the cylinder if you reduce the kelvin temperature to half its original value while holding the pressure constant?
according to the ideal gas equation , volume will be four time of initial value.
What happens to the pressure of a gas if the volume of gas is tripled at a constant temperature?
The pressure is reduced to one third of the original pressure. The pressure will stay the same you are only changing the volume
How can we reduce pressure?
Pressure in a glass can be reduced by either decreasing the amount of the gas in a finite space, or by increasing the volume of the finite space.
How do you increase the pressure of gas?
decreasing the volume available for the gas or increasing its temperature
According to ideal gas eqation if pressure is double to initial pressure then what happens to the volume?
It would be half of the original volume. As you reduce the volume the pressure would increase and at half the original volume the pressure would be doubled.
What is difference between compressibility factor and super compressibility factor?
An ideal gas will have a volume that is inversely proportional to the pressure (assuming constant temperature). For example, if you double the pressure, the volume will be reduced to 1/2 the original volume. For real gases, the behavior is usually somewhat different. In some cases, if you double the pressure, the volume will reduce to LESS than 1/2 the original volume. This is due to the attraction between the molecules, and this phenomenon is called "supercompressibility".
What change in volume would cause the pressure of an enclosed bag to be reduced to one quarter of its original value?
Assuming it's a bag of gas at constant temperature, four times the volume by the relationship: P1V1 = P2V2
What will the pressure inside the container become if the piston is moved to the 1.80 L rm L mark while the temperature of the gas is kept constant?
This problem can be solved with the ideal gas law. The original pressure and volume of the container are proportional the final pressure and volume of the container. The original pressure was 1 atmosphere and the original volume was 1 liter. If the final volume is 1.8 liters, then the final pressure is 0.55 atmospheres.
What would happen to the volume of the gas inside the cylinder if you reduce the kelvin temperature to half its original value while holding the pressure constant?
according to the ideal gas equation , volume will be four time of initial value.
What is Charles law and boyles law?
BOYLES LAW The relationship between volume and pressure. Remember that the law assumes the temperature to be constant. or V1 = original volume V2 = new volume P1 = original pressure P2 = new pressure CHARLES LAW The relationship between temperature and volume. Remember that the law assumes that the pressure remains constant. V1 = original volume T1 = original absolute temperature V2 = new volume T2 = new absolute temperature P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature IDEAL GAS LAW P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature Answer BOYLES LAW The relationship between volume and pressure. Remember that the law assumes the temperature to be constant. or V1 = original volume V2 = new volume P1 = original pressure P2 = new pressure CHARLES LAW The relationship between temperature and volume. Remember that the law assumes that the pressure remains constant. V1 = original volume T1 = original absolute temperature V2 = new volume T2 = new absolute temperature P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature IDEAL GAS LAW P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature
What happen to the pressure of a gas if the volume of the gas is tripled of a constant temperature?
The pressure is reduced to one third of the original pressure. The pressure will stay the same you are only changing the volume
What happens to the pressure of a gas if the volume of gas is tripled at a constant temperature?
The pressure is reduced to one third of the original pressure. The pressure will stay the same you are only changing the volume
How do you increase the volume of gas?
To increase the volume of a gas * reduce the pressure, or * increase the temperature, or * add more gas
If the pressure on a gas increases four fold what happens to its volume?
The volume, in this case, will reduce by a factor of 4 (i.e., to 1/4 of its previous volume).
If the pressure of a gas in a container is 10psi what will the pressure be in the volume of the container is reduced to one-half of its original size?
20psi
How can we reduce pressure?
Pressure in a glass can be reduced by either decreasing the amount of the gas in a finite space, or by increasing the volume of the finite space.
