The Relationship Between Temperature and Pressure of an Ideal Gas

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Temperature can change without altering pressure or the number of molecules in an ideal gas, as demonstrated by Charles' Law. This law states that if pressure and composition remain constant, an increase in temperature necessitates an increase in volume. Conversely, a decrease in temperature requires a decrease in volume to maintain constant pressure. The relationship is encapsulated in the equation PV = nRT, where volume adjustments allow for temperature changes at constant pressure. Understanding this principle is crucial for applications involving isobaric processes in gases.
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can temperature be changed without changing pressure as well as number of molecules for an ideal gas?
 
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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?

PV = nRT

If pressure and composition are constant

\frac{P}{nR}V = \kappa V = T

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.
 

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