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If expression 5.68 is correct, it must be extensive: Increasing both NA and NB by a common factor while holding all intensive variables fixed should increase G by the same factor. Show that expression 5.68 has this property. Show that it would not have this property had we not added the term proportional to In NA!.

Short Answer

Expert verified

Therefore,

G'=xGG'xG

Step by step solution

01

Given information

Increasing both NA and NB by a common factor while holding all intensive variables fixed should increase G by the same factor.

02

Explanation

The Gibbs free energy for a pure solvent is calculated as follows:

G=NAμ0+NBf-NBkTlnNA+NBkTlnNB-NBkT(1)

We can show that G is an extensive quantity by replacing NAwithxNAandNBwithxNBwhile keeping the intensive quantities constant:

G'=xNAμ0+xNBf-xNBkTlnxNA+xNBkTlnxNB-xNBkT(2)

By using ln(AB)=ln(A)+ln(B), we have

xNBkTlnxNA=xNBkTlnNA+ln(x)xNBkTlnxNB=xNBkTlnNB+ln(x)

Equation (2) will become

G'=xNAμ0+xNBf-xNBkTlnNA+xNBkTlnNB-xNBkTG'=xNAμ0+NBf-NBkTlnNA+NBkTlnNB-NBkTG'=xG

This means Gibbs energy is extensive quantity

03

Explanation

The Gibbs free energy will be: if the term lnNB!is not included to equation (1).

G=NAμ0+NBf-NBkTlnNA

Replace NAwithxNAandNBwithxNB

G'=xNAμ0+xNBf-NBkTlnxNA

By using ln(AB)=ln(A)+ln(B)

G=xNAμ0+xNBf-NBkTlnNA-NBkTln(x)xGG'xG

Hence, Gibbs free energy will not be extensive.

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Most popular questions from this chapter

Let the system be one mole of argon gas at room temperature and atmospheric pressure. Compute the total energy (kinetic only, neglecting atomic rest energies), entropy, enthalpy, Helmholtz free energy, and Gibbs free energy. Express all answers in SI units.

What happens when you spread salt crystals over an icy sidewalk? Why is this procedure rarely used in very cold climates?

Suppose that a hydrogen fuel cell, as described in the text, is to be operated at 75°Cand atmospheric pressure. We wish to estimate the maximum electrical work done by the cell, using only the room temperature data at the back of this book. It is convenient to first establish a zero-point for each of the three substances, H2,O2,andH2O. Let us take Gfor both H2andO2to be zero at 25°C, so that G for a mole of H2Ois -237KJat 25°C.

(a) Using these conventions, estimate the Gibbs free energy of a mole of H2at 75°C. Repeat for O2andH2O.

(b) Using the results of part (a), calculate the maximum electrical work done by the cell at 75°C, for one mole of hydrogen fuel. Compare to the ideal performance of the cell at25°C.

Suppose you have a liquid (say, water) in equilibrium with its gas phase, inside some closed container. You then pump in an inert gas (say, air), thus raising the pressure exerted on the liquid. What happens?

(a) For the liquid to remain in diffusive equilibrium with its gas phase, the chemical potentials of each must change by the same amount: dμl=dμg Use this fact and equation 5.40 to derive a differential equation for the equilibrium vapour pressure, Pv as a function of the total pressure P. (Treat the gases as ideal, and assume that none of the inert gas dissolves in the liquid.)

(b) Solve the differential equation to obtain

Pv(P)-PvPv=eP-PvV/NkT

where the ratio V/N in the exponent is that of the liquid. (The term Pv(Pv) is just the vapour pressure in the absence of the inert gas.) Thus, the presence of the inert gas leads to a slight increase in the vapour pressure: It causes more of the liquid to evaporate.

(c) Calculate the percent increase in vapour pressure when air at atmospheric pressure is added to a system of water and water vapour in equilibrium at 25°C. Argue more generally that the increase in vapour pressure due to the presence of an inert gas will be negligible except under extreme conditions.

By subtracting μNfrom localid="1648229964064" U,H,F,orG,one can obtain four new thermodynamic potentials. Of the four, the most useful is the grand free energy (or grand potential),

ΦU-TS-μN.

(a) Derive the thermodynamic identity for Φ, and the related formulas for the partial derivatives ofΦwith respect toT,V, and μN

(b) Prove that, for a system in thermal and diffusive equilibrium (with a reservoir that can supply both energy and particles), Φtends to decrease.

(c) Prove thatϕ=-PV.

(d) As a simple application, let the system be a single proton, which can be "occupied" either by a single electron (making a hydrogen atom, with energy -13.6eV) or by none (with energy zero). Neglect the excited states of the atom and the two spin states of the electron, so that both the occupied and unoccupied states of the proton have zero entropy. Suppose that this proton is in the atmosphere of the sun, a reservoir with a temperature of 5800Kand an electron concentration of about 2×1019per cubic meter. Calculate Φfor both the occupied and unoccupied states, to determine which is more stable under these conditions. To compute the chemical potential of the electrons, treat them as an ideal gas. At about what temperature would the occupied and unoccupied states be equally stable, for this value of the electron concentration? (As in Problem 5.20, the prediction for such a small system is only a probabilistic one.)

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