Arri asked:
According to the ideal gas law, the number of moles would need to increase as the temperature decreases and it would need to decrease if the temperature increases. Why is this? Wouldn’t temperature rise if there are more moles since there will be more “bumping” going on? Also, if it’s not too much to ask, can someone give an example to help my understanding of this concept? Thanks in advance!
According to the ideal gas law, the number of moles would need to increase as the temperature decreases and it would need to decrease if the temperature increases. Why is this? Wouldn’t temperature rise if there are more moles since there will be more “bumping” going on? Also, if it’s not too much to ask, can someone give an example to help my understanding of this concept? Thanks in advance!
{ 1 comment… read it below or add one }
The Ideal gas law is PV = nRT.
If the number of moles increases and the temperature stays the same, then for the same volume the pressure will increase. However to ensure that the pressure is constant the temperature must be reduced. This reduces the amount of kinetic energy that the gas particles have, so for the same volume, the pressure will be the same.
Also if the temperature increases and the number of moles stays the same then the particles have more kinetic energy so the pressure will be increased assuming the volume is constant. The number of moles must then be decreased to accomodate the increase in kinetic energy.