- #1
korneld
- 22
- 0
Hi,
I have a question about the ideal gas law.
I have been under the impression that if volume goes down then pressure and temperature go up. But, if you look at the equation T=PV/nR, it seems that if volume, say, doubles, pressure will be halved and vice-versa. While that makes sense, it also leaves the temperature constant. Doesn’t that conflict with real life observations?
Thank you,
Kory
I have a question about the ideal gas law.
I have been under the impression that if volume goes down then pressure and temperature go up. But, if you look at the equation T=PV/nR, it seems that if volume, say, doubles, pressure will be halved and vice-versa. While that makes sense, it also leaves the temperature constant. Doesn’t that conflict with real life observations?
Thank you,
Kory