|Apr24-12, 12:28 AM||#1|
Thermodynamics: Internal Energy and Enthalpy
H = U+ pV
pV = nRT
H= U+ nRT
H= H (T)
I dont understand the transition from U+ nRT to H (T)
Can someone explain this?
I get that H = U + pV
But how is H= U+ nR
|Apr24-12, 02:14 AM||#2|
For a monoatomic ideal gas, U=(3/2) PV. Hence, H=(5/2) PV=(5/2) nRT
Which shows that H for an ideal gas is a function of T alone ,i.e, H=H(T).
Of course it is also function of n since it is extensive quantity. However, this dependence is easy to get rid of by defining h=H/n which is an intensive quantity.
|Apr24-12, 10:12 PM||#3|
thank you...that clears it up!
|enthalpy, internal energy|
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