Robert Boyle
Pressure, volume, temperature & the amount of gas.
Yes, it does affect the volume. The relationship between them can be explained by the equation pV=nRT (pressure x volume = number of moles of gas x molar gas constant x temperature). Therefore, there is a direct proportionality between temperature and volume. If the temperature doubles, so does the volume.
The product of pressure and volume. Does PV = nRT look familiar? (:
directly proportional to the Kelvin temperature
When pressure double, the volume halves. However this is only true if the number of molecules and the temperature are both in a constant state.
Avogadro stated that two samples of ideal gases at the same temperature, pressure, and volume contain the same number of molecules.
Pressure, volume, temperature & the amount of gas.
Yes, it does affect the volume. The relationship between them can be explained by the equation pV=nRT (pressure x volume = number of moles of gas x molar gas constant x temperature). Therefore, there is a direct proportionality between temperature and volume. If the temperature doubles, so does the volume.
Mass, temperature, time, distance, and volume can all have number values.
The volume decrease.
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 doubled.
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 temperature and pressure.
The temperature and pressure.
Then the specific volume varies directly with temperature.
If the volume is constant, the density does not change with temperature. With increasing temperature there is still the same number of molecules confined to the same volume of space, so no difference in density.