You can't compare pressure with volume. Presumably, somebody was talking about something being greater AT constant pressure, compared to constant volume.
high
At a constant temperature, the volume and the pressure are inversely proportional, that it, the greater the volume, the lesser the pressure on the gas, and viceversa.
At a constant temperature, the volume and the pressure are inversely proportional, that it, the greater the volume, the lesser the pressure on the gas, and viceversa.
The volume is constant. The pressure will increase.The volume is constant. The pressure will increase.
One is for constant pressure, the other is for constant volume. These are not the same; for example, if the pressure is maintained constant, and the gas is heated, the volume changes.
The pressure is now higher.
Ideal gas Law PV = nRT where P is pressure V is volume n is moles R is a constant of 8.31 and T is temperature so if u multiply PV with T constant, that leaves nR, therefore you will always get mole of the air multiplied with 8.31
Pressure. An isochore represents constant volume, while an isobar represents constant pressure.
At constant temperature p.V=constant, so pressure INcreases when decreasing the volume.
In general, the pressure of a gas increases with increasing temperature, assuming volume remains constant (according to Gay-Lussac's Law). This is because as temperature increases, gas molecules gain more kinetic energy and collide with the container walls more frequently and with greater force, resulting in increased pressure.
Volume & pressure are inversely proportionate, if temperature stays constant volume would decrease at a factor proporionate to the increase in pressure.
When the temperature of a gas is constant and the pressure decreases, the volume will increase. This is described by Boyle's Law, which states that at constant temperature, the pressure and volume of a gas are inversely proportional to each other.