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How to prove that (a)(dU/dV)T=0 (b)(dH/dP)T=0 for an ideal gas. Where U is internal energy per unit mass, V is volume, T is temperature (which is held constant for above 2 question), H is the enthalpy per unit mass, and P is the pressure. I found this in a thermodynamics textbook. This is...

how to prove that (a)(dU/dV)T=0 (b)(dH/dP)T=0 for an ideal gas.

Oh sorry... What I am trying to ask is, how to prove that (a)(dU/dV)T=0 (b)(dH/dP)T=0 for an ideal gas.

For an ideal gas, how to prove that: (a) its internal energy does not change with volume at constant temperature (b) its enthalpy does not change with pressure at constant temperature Thanks.