Our teacher just told us to always do it in terms of the temperature remaining constant.
So if the pressure increases, for the temperature, and therefore kinetic energy, to remain constant, the volume must fall. Potential energy decreases and so the internal energy decreases.
This was posted from The Student Room's Android App on my GT-S5360
Volume doesn't affect internal energy. The internal energy is the sum of both potential and kinetic. As volume decreases/ pressure increases the loss in potential energy is converted to kinetic energy. If decreasing the volume of a gas made the internal energy lower you would be destroying energy, and this isn't what happen. Am I missing something?
Volume doesn't affect internal energy. The internal energy is the sum of both potential and kinetic. As volume decreases/ pressure increases the loss in potential energy is converted to kinetic energy. If decreasing the volume of a gas made the internal energy lower you would be destroying energy, and this isn't what happen. Am I missing something?
I agree with you here, I think they are getting Volume and Mass muddled up, by decreasing volume you are increasing the mass per m^3 so the pressure increases. By decreasing mass you are decreasing binding enery (g485) e=mc^2
This is going to sound very stupid, but what exactly is an ideal gas?
It's a concept used to describe a gas, the term ideal is used as certain assumptions are made. However at standard temperature and pressure most gases behave as an ideal gas.