A. only at low pressures and large volumes.
B. only at high temperatures.
C. only at large volumes and large pressures.
D. at all pressures and volumes.
2007-04-25 17:33:01 · 5 answers · asked by 11111111111111111111111111111111 1 in Science & Mathematics ➔ Physics
A. only at low P and Large V.
Really, it the answer should be at low pressures and low densities. The closer the gas particles get together the more they interact and affect each other. That's why the pressure has to be low (means the particles are not being compressed) and the volume has to be high (that part isn't really true as I said above). A is the best answer, but not really the correct one.
2007-04-25 17:36:46 · answer #1 · answered by yamaguchi 2 · 1⤊ 0⤋
I would say A. The ideal gas law is that, only for ideal situations of around room temperature, low pressure, and large volumes. The ideal gas law is nothing more than a limiting case of a much more complicated gas law.
2007-04-25 17:39:08 · answer #2 · answered by msi_cord 7 · 0⤊ 0⤋
Probably, C, because physics teacher said that as temperature of gas increases the more likely it is going to be like an ideal gas, but I'm not sure.
2014-02-17 01:18:16 · answer #3 · answered by Anonymous · 0⤊ 0⤋
At all pressures and volume.
2007-04-25 17:36:27 · answer #4 · answered by Faisal R 3 · 0⤊ 0⤋
D
2007-04-25 17:38:55 · answer #5 · answered by Alandi 3 · 0⤊ 0⤋