Proving Ideal Gas Law: dU/dV and dH/dP at Constant T

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SUMMARY

The discussion focuses on proving the relationships (dU/dV)T=0 and (dH/dP)T=0 for an ideal gas. It establishes that, at constant temperature, the internal energy (U) does not change with volume (V), and the enthalpy (H) does not change with pressure (P). These conclusions are derived from the fundamental properties of ideal gases, specifically the ideal gas law and the definitions of internal energy and enthalpy.

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Hong1111
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how to prove that

(a)(dU/dV)T=0
(b)(dH/dP)T=0

for an ideal gas.
 
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The first step would be to post this in the homework section.
 

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