Question

The Boyle’s Law and the Gay-Lussac’s Law express experimental relationships between two of the three parameters characterizing the state of gas, the pressure, volume, and temperature, while the third is kept constant. For both laws state which parameters are variable and which is kept constant.

The Boyle’s Law and the Gay-Lussac’s Law are special cases of a more general relationship called the ideal gas law. State the ideal gas law. Why do we use the absolute temperature (temperature in kelvins) in the ideal gas law? Explain how using the Celsius scale would give nonsensical results.

Answer 1

In boyle's law the temperature is held constant. the boyle's law states that the volume of a gas is inversely proportional to the pressure at constant temperature.

In Gay-lussacs law the volume is kept constant .It states that the pressure of an ideal gas is directly proportional to the absolute temperature of the ideal gas at constant volume.

Ideal gas law- PV=nRT=it is an equation which shows the relationship between the parameters characterizing the state of an ideal gas

where P=pressure, V=volume, n=number of moles,R=gas constant, T= temperature in kelvin

we use absolute temperature( temperature in kelvins ) because in kelvin 0K is known as absolute zero which means at this point the energy is equal to zero and pressure and volume are in correlation with the energy.

The celcius scale would give nonsensical results due to two things

1) in celcius , there is a 0 degree, when caluclating the ideal gas equations, there will come zero in the denominator in place of T so that will give no value as anything divided by zero is infinity.

2) in celcius the negative value of temperatures may also give confusing results.