The Relationship Between Temperature and Pressure of an Ideal Gas

Click For Summary

Discussion Overview

The discussion revolves around the relationship between temperature and pressure in the context of an ideal gas, specifically exploring whether temperature can be altered without affecting pressure or the number of molecules present. The scope includes theoretical considerations and references to gas laws.

Discussion Character

  • Technical explanation
  • Conceptual clarification
  • Debate/contested

Main Points Raised

  • One participant questions whether it is possible to change temperature without also changing pressure or the number of molecules in an ideal gas.
  • Another participant references the isobaric process, suggesting that temperature can change while pressure remains constant.
  • A third participant presents the ideal gas law (PV = nRT) to argue that if pressure and the number of molecules are constant, temperature can be expressed in terms of volume, indicating that temperature can change with volume adjustments.
  • A later reply elaborates that temperature can increase while pressure remains constant if the volume increases, and conversely, temperature can decrease while pressure remains constant if the volume decreases.

Areas of Agreement / Disagreement

Participants present multiple viewpoints regarding the relationship between temperature, pressure, and volume in ideal gases, indicating that there is no consensus on the initial question posed.

Contextual Notes

The discussion relies on the assumptions of ideal gas behavior and does not address potential limitations or conditions under which these relationships hold true.

factfinder
Messages
8
Reaction score
0
can temperature be changed without changing pressure as well as number of molecules for an ideal gas?
 
Science news on Phys.org


See isobaric (constant pressure) process for a gas.
 


factfinder said:
can temperature be changed without changing pressure as well as number of molecules for an ideal gas?

[itex]PV = nRT[/itex]

If pressure and composition are constant

[itex]\frac{P}{nR}V = \kappa V = T[/itex]

This is Charles law.
 


As stated in the above equation, the temperature of a set number of molecules can increase while the pressure remains constant, just so long as the volume of the molecules increases. Or you can say just the opposite, the the temperature of a set number of molecules can decrease while the pressure remains constant, just so long as the volume decreases.
 

Similar threads

Undergrad Movable Wall in an Adiabatic System: Same Final Temperature?
  • · Replies 8 ·
Replies
8
Views
2K
Undergrad Why pressure stays the same when doubling both volume and temperature?
  • · Replies 35 ·
2
Replies
35
Views
6K
Undergrad How to calculate the mass of gas in a tank?
  • · Replies 109 ·
4
Replies
109
Views
9K
Undergrad Compressing gas with piston: reasons for temperature increase?
  • · Replies 5 ·
Replies
5
Views
4K
High School Extrapolation of relationship of temperature and volume for gas
  • · Replies 7 ·
Replies
7
Views
3K
Undergrad Focus Problem for Entropy Change in Irreversible Adiabatic Process
  • · Replies 60 ·
3
Replies
60
Views
11K
Undergrad Derivation of ideal gas heat capacity relationship
  • · Replies 6 ·
Replies
6
Views
2K
Undergrad Why is estimation of ##\frac{Pv}{RT}=1+BP+CP^2+...## interesting?
  • · Replies 2 ·
Replies
2
Views
2K
High School How the temperature of the Earth's surface affects the air pressure above it
  • · Replies 7 ·
Replies
7
Views
3K
High School Ideal gas formula not working?
  • · Replies 14 ·
Replies
14
Views
2K