Physical Chemistry: Estimating ΔG of an Ideal Gas

AI Thread Summary
To estimate ΔG for one mole of an ideal gas increasing pressure from 1.00 atm to 11.0 atm at 25.0°C, the relevant equation is ΔG = nRTln(Pf/Pi). The discussion highlights that the problem does not specify whether the gas is monatomic or diatomic, which raises questions about the applicability of certain equations. Although the heat capacity (C(p,m)) is not provided, it is noted that ΔH can still be calculated. The participants confirm that the equation for ΔG is valid for this isothermal process involving an ideal gas. Overall, the focus is on clarifying the necessary parameters and equations for the calculation.
Nick_273
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Homework Statement


Estimate ΔG for the process where one mol of ideal gas is subjected to an increase in
pressure from 1.00 atm to 11.0 atm at 25.0°C.


Homework Equations


ΔG=ΔH-TΔS
ΔH=C(p,m)(Tf-Ti


The Attempt at a Solution


Seems straight forward, but it seems i am not given enough information to complete the problem. I need C(p,m)? It does say estimate. Does that mean that i only need to imply that the Gibbs free energy will be possitive, negative, or 0?

If you can help me clarify the problem that would be greatly appreciated!

Thanks.
 
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Does the problem say whether the ideal gas is monatomic or diatomic?
 
No, it does not. Does this equation apply?

ΔG = nRTln(Pf/Pi)

I found it in my notes but can't find it anywhere in the text.
 
Oh, for this case, you can actually still calculate ΔH even though you do not know the heat capacity of the gas.
 
Hi Nick_273! :smile:

Nick_273 said:
No, it does not. Does this equation apply?

ΔG = nRTln(Pf/Pi)

I found it in my notes but can't find it anywhere in the text.

Yep, it applies (for an isothermal process on an ideal gas).
 

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