For the pressure to remain the same, the temperature would double if the volume also doubled.
Decrease in pressure and volume.
There may have been some gas in the liquid, or maybe there was a decrease in pressure.
cos2(s)
If the volume is fixed, then doubling the absolute temperature will double the pressure.At 0° C, the absolute temperature is 273 K. Heat the gas to 273° C = 546 K.
The temperature of the water is 100 degrees celsius.
If a fixed sample of gas has a change of temperature pressure would increase.
pV = nRT ← General Gas Lawrearranging to solve the pressure gives us:p = nRT/Vdoubling the volume gives: p = nRT/2VThis means that the pressure will be halved.
Are you stating or asking ? If that's a statement, then it's an incorrect one. At constant temperature, the product of (pressure) x (volume) is constant. So, if the volume changed by a factor of 3, the pressure must also change by a factor of 3 ... the pressure must triple.
In a sample of air, an increase in temperature will result in an increase in the partial pressure of oxygen.
Decrease in pressure and volume.
There may have been some gas in the liquid, or maybe there was a decrease in pressure.
190 mm Hg
cos2(s)
liquid
temperature
If the volume is fixed, then doubling the absolute temperature will double the pressure.At 0° C, the absolute temperature is 273 K. Heat the gas to 273° C = 546 K.
The temperature of the water is 100 degrees celsius.