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WWCY
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- Homework Statement
- The equation of state for some gas is ##P(V-b) = RT)## (V is the volume occupied by a mole of gas), show that the internal energy of this gas is a function of temperature only.
My work leads to the wrong answer, some assistance in pointing out my mistake is greatly appreciated!
- Relevant Equations
- Real gas equations
My work was as follows:
The first law states ##dU = TdS - PdV##, and thus
$$p =- (\partial U/\partial V)| _S$$
$$U = -RT \ln(V-b) + f(S)$$
To determine ##f(S)##, I reasoned that in the ideal gas limit of ##b = 0##, ##U## should take the form of the ideal gas' molar internal energy ##\frac{3}{2} RT##. So I set ##b = 0## and compare the expressions for energy in the ideal gas limit to obtain
$$f(S) = \frac{3}{2}RT + RT \ln (V)$$
However, inserting this into the internal energy expression for the real gas gives
$$U = \frac{3}{2}RT + RT \ln \big(\frac{V}{V-b} \big)$$
which doesn't seem to be independent of V.
What have I done incorrectly?
The first law states ##dU = TdS - PdV##, and thus
$$p =- (\partial U/\partial V)| _S$$
$$U = -RT \ln(V-b) + f(S)$$
To determine ##f(S)##, I reasoned that in the ideal gas limit of ##b = 0##, ##U## should take the form of the ideal gas' molar internal energy ##\frac{3}{2} RT##. So I set ##b = 0## and compare the expressions for energy in the ideal gas limit to obtain
$$f(S) = \frac{3}{2}RT + RT \ln (V)$$
However, inserting this into the internal energy expression for the real gas gives
$$U = \frac{3}{2}RT + RT \ln \big(\frac{V}{V-b} \big)$$
which doesn't seem to be independent of V.
What have I done incorrectly?
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