Hey guys,(adsbygoogle = window.adsbygoogle || []).push({});

I'm working on calculating the enthalpy, entropy and internal energy of substances. treating them as an ideal gas. I wonder if I could be pointed in the right direction with some calculations.

Enthalpy change:

h_{2}-h_{1}=∫c_{p}dT+ ∫[v-T(∂v/∂T)_{P}]dP

At ideal gas the pressure integral goes to zero.

So we have just the integral of C_{p}with respect to T.

All correct so far?

Its with the entropy and internal energy where I get confused.

ds = (C_{p})dT - (∂v/∂T)_{P}dP

is there a way to simplify this further at ideal gas to make it easily calculated ?

I guess internal energy can be calculated from h using h = u + Pv.

Thanks very much

Look forward to any replies.

1. The problem statement, all variables and given/known data

2. Relevant equations

3. The attempt at a solution

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# Thermodynamics - ideal gas properties

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