answersLogoWhite

0

Gauge pressure = absolute pressure - atmospheric pressure.

Atmospheric pressure (at sea level) is generally taken to be 101.325kPa.

so the answer is (C) = 448.955 kPa

User Avatar

Wiki User

13y ago

Still curious? Ask our experts.

Chat with our AI personalities

ViviVivi
Your ride-or-die bestie who's seen you through every high and low.
Chat with Vivi
DevinDevin
I've poured enough drinks to know that people don't always want advice—they just want to talk.
Chat with Devin
LaoLao
The path is yours to walk; I am only here to hold up a mirror.
Chat with Lao
More answers

The gauge pressure is the difference between the absolute pressure and atmospheric pressure. If atmospheric pressure is approximately 101.3 kPa, then the gauge pressure would be 448.980 kPa (550.280 kPa - 101.3 kPa).

User Avatar

AnswerBot

10mo ago
User Avatar

The gauge pressure would be 448.955 kPa.

User Avatar

Wiki User

10y ago
User Avatar

448.995 kPa

User Avatar

Wiki User

12y ago
User Avatar

Add your answer:

Earn +20 pts
Q: If the absolute pressure of gas is 550.280 kPa it's gage pressure is?
Write your answer...
Submit
Still have questions?
magnify glass
imp
Continue Learning about Natural Sciences

If a gas has a gage pressure of 206 kPa its absolute pressure is?

The absolute pressure can be calculated by adding the atmospheric pressure to the gauge pressure. If the atmospheric pressure is 101.3 kPa, then the absolute pressure of the gas would be 206 kPa + 101.3 kPa = 307.3 kPa.


With respect to gages Boyle's law shows the relationship between?

Boyle's Law says that PV is constant for ideal gas at a constant temperature. The pressure used should be the absolute pressure, not the gage pressure. Ge the absolute pressure should be obtained using : P = PG + PE where PG = gage pressure ( kPag , psig, etc. ) PE = barometric pressure ( kPaa, psia, etc. ) P = absolute pressure ( kPaa , psia, etc. ) ( PG + PE ) ( V ) = Constant for constant temperature The g in kPag and in psig indicates gage pressure.


If a certain amount of gas fills a 1.0 liter container and exerts a pressure on the walls of 2.0 Nm2 at 20 degrees celsius what would the pressure theoretically be at absolute zero?

At absolute zero, the gas molecules stop moving, hence no pressure is exerted by the gas. This is known as absolute zero pressure.


Whose law states that the volume of a gas varies inversely with the absolute pressure as long?

Boyle's law.


What would the volume and pressure of an ideal gas be at absolute zero temperature IF an ideal gas actually existed?

At absolute zero temperature, an ideal gas would theoretically have zero volume and zero pressure. This is because at absolute zero, the kinetic energy of gas particles would be minimal, causing them to come to a complete stop and occupy no volume. Since pressure is the result of gas particles colliding with the walls of their container, zero particle movement would result in zero pressure.