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Answered 2010-11-05 01:44:46

If you increase the temperature of a fluid, the pressure in the container increases.

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If the contents in the container are gaseous, then the pressure will increase as temperature increases. The pressure will decrease as temperature decreases.

Answer The pressure increases when the temperature rises.

Since the container cannot expand, the pressure will increase because the increase in temperature increases the kinetic energy of the gas particles, resulting in the particles hitting the inside walls of the container more frequently.

The pressure of a gas increases with an increase in temperature.

the pressure increases, as more matter added to a container with a constant temperature will just bunch everything toghether tighter.

Either the volume or the pressure of the gas will increase.

Assuming you haven't put any more gas in the container, the pressure will go down. Usually, the reason the volume of the container gets larger is that you put more gas in the container and the gas pressure in the container seeks to equalize with the pressure outside it.

If you decrease the volume of the container, the pressure rises, and vice versa.

If the volume stays the same, and temperature goes up, pressure goes up.

The pressure decreases. If the temperature were to decrease enough it is possible for the gas to become a liquid or solid, but that would require a large change in temperature, assuming the container starts at room temperature.

In that case, the pressure increases. Specifically, the pressure will be proportional to the absolute temperature.

According to the Ideal gas law, pV=nRT where p = absolute pressure and T = absolute temperature Therefore, the temperature increases if the pressure increases.

The pressure will increase. Temperature is the measure of the average kinetic energy in a substance. So if temperature is increased, the particles of the substance will move faster. This will result in more collisions on the wall of the container, or in other words, higher pressure. To visualize this with the ideal gas law, take a look at the equation: PV = nRT P: pressure V: volume n: number of moles of gas R: a constant T: temperature You can see that if all variables were kept the same, and temperature was increased, pressure would also have to increase. Temperature and pressure are therefore directly related. Hope this helps!

By Charles law, at constant volume the pressure is directly proportional to the temperature. Hence fall in pressure

If the gas is in an inclosed container, the pressure will increase. If it is free to expand, it will have a greater volume.

Assuming the volume is kept constant, the pressure will also decrease in this case.