if the temperature of a gas is raised but its volume is held constant what will happen to the pressure?

Answer 1

PV = nRT
Pressure*Volume = #_of_molecules*constant*temperature

So if the volume V, and the number of molecules n are fixed, increasing the temperature will cause an increase in pressure.

It's the principle used for pressure cookers: You heat up water to make steam. Since your cooker is closed the pressure inside rises. On old cookers, you have a removable cap; if you lift it while the water is boiling inside, steam will rush out until the pressure inside is the same as the pressure in your kitchen.

Answer 2

Yahoo search!: temperature of a gas is raised but its volume is held constant what will happen to the pressure -- and follow first link and read up on "pressure."

When you raise the temperature of a gas, the molecules gain energy. If the volume is not constrained, the molecules will get further apart -- i.e. the gas expands. But if you hold the volume constant, the molecules use the extra energy gained to hit the walls of the container with stronger force -- i.e. pressure increases.

Answer 3

Kinetic theory of gasses... Imagine the gas molecules as separate balls moving randomly. Their speed is proportional to their temperature. If you increase the temp without changing the enclosing volume, they will hit the interior surface at a higher velocity, hence with higher energy, hence higher force. Since the enclosing volume has not changed, the interior surface area has not changed. So an increase in force, with area acted upon remaining constant----> Increase in pressure

Answer 4

The equation that relates all of this information is PV=NRT, P being pressure, V being volume, n is number of moles, R is a constant, adn T is temp. B/c temp goes up and V is constant, pressure must increase

Answer 5

The pressure will increase.

Answer 6

The pressure will increase.

Answer 7

the pressure will rise