Physical Chemistry 2.pdf - OER@AVU - African Virtual University
Physical Chemistry 2.pdf - OER@AVU - African Virtual University
Physical Chemistry 2.pdf - OER@AVU - African Virtual University
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<strong>African</strong> <strong>Virtual</strong> <strong>University</strong><br />
After the barrier is removed, the gases mix so that the total pressure is the sum of<br />
their partial pressure P = P A + P B . Gibbs energy is then given by<br />
G F inal = n A<br />
⎡ ° ⎛ PA ⎞ ⎤<br />
⎢µ<br />
A + RT ln<br />
⎝<br />
⎜<br />
P° ⎠<br />
⎟ ⎥<br />
⎣<br />
⎦<br />
+ nB µ ⎡ ° ⎛ PB ⎞ ⎤<br />
⎢ B + RT ln<br />
⎝<br />
⎜<br />
P° ⎠<br />
⎟ ⎥<br />
⎣<br />
⎦ (1.13)<br />
The change in Gibbs free energy on mixing is the difference between the initial free<br />
energy, G initial , and the final G final i.e.<br />
∆ mixG = nA RT ln P ⎛ A ⎞<br />
⎝<br />
⎜<br />
P° ⎠<br />
⎟ + nB RT ln P ⎛ B ⎞<br />
⎝<br />
⎜<br />
P° ⎠<br />
⎟<br />
(1.14)<br />
The may also be written in terms of mole fractions as<br />
since n i = x i n and P i /P = x i .<br />
1.7 What about the entropy of mix?<br />
(1.15)<br />
The entropy of mixing is derived from the thermodynamic expression that, − S =<br />
(∂G/∂T) P,n . It then follows from the equation (1.15) that the entropy of mixing is<br />
given by the expression<br />
∆ mix S = − ∂∆ mixG ⎛<br />
⎝<br />
⎜<br />
∂T<br />
⎞<br />
⎠<br />
⎟<br />
P ,T , nA , nB = − nR ( xA ln xA + xB ln xB )<br />
(1.16)<br />
From previous discussions in thermodynamics you will recall that Gibbs energy is<br />
related to enthalpy through the expression ΔG = ΔH – TΔS. For the mixing of two<br />
gases we can write that Δ mix G = Δ mix H – TΔ mix S, which gives<br />
Δ mix H= Δ mix G + TΔ mix S. (1.17)