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- Demonstrate IN DETAIL, and justify the Maxwell relations used, in the proof of the following statement:i) State the third law of thermodynamics. How is it interpreted in a microscopic thermodynamic ense? (b) Briefly outline the reversible Carnot cycle and give all the necessary thermodynamic quantitiesGiven these relation, prove this without usin Maxwell relatios or thermodynamic squares as - (7), aP/T =
- 7) Use the Maxwell relations to show that the entropy of a perfect gas depends on the volume as Soc R Inv.(2) The Gibbs function G is (GF) ₁ P == ound ·S (06), = relationship (25) a = -(=++) ₂ thu modynamic property. If =V, prove the following3) Derive tue Joule -Tuom son coe- sefficiant for Vivial eguation of state in terms of volume expausion .
- Which one of the following is NOT a Maxwell thermodynamic relation? as (0) = (от), (0) = ( ), (1), = (P) aV ат as P ат a-), - All 'Bout Chemistry = as aV 49. (a) (b) (c)Which of the following functions are exact differentials? a dF=1xdx+1ydy b dF=1ydx+1xdy c dF=2x2y2dx+3x3y3dy d dF=2x2y3dx+2x3y2dy e dF=xndx+yndy,n= any integer f dF=(x3cosy)dx+(x3siny)dyIn Chapters 17 and 18 we have derived expressions for the absolute amounts of the energies H and G. However, in tables of thermodynamic data, we always tabulate H and G that is, changes in enthalpy and Gibbs energy. How do you explain this apparent discrepancy?
- Thermodynamic properties can also be determined for ions. Determine H,S,andG for the following two reactions, which are simply reactions of dissolution: NaHCO3(s)Na+(aq)+HCO3(aq)Na2CO3(s)2Na+(aq)+CO32(aq) Assume standard conditions standard concentration is 1M for ions in aqueous solution, and consult the table of thermodynamic properties in Appendix 2. What similarities and differences are there?Give the difference betweenConsider a gas of N fermions. (i) At T = 0, what does the Fermi momentum represent? (ii) Consider the occupation number for state i, (n;). In the limit of T → 0, what are the possible values (n;) can take? Explain your answer in terms of the relative values of the energy of the state and the chemical potential.