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Thermodynamics Part I: Spontaneity of Rxns

Thermodynamics Part I: Spontaneity of Rxns. Jespersen Chap. 19 Sec 1 thru 6. Dr. C. Yau Fall 2014. 1. First Law of Thermodynamics. The first law of thermodynamics states that internal energy (E) may be transferred as heat (q) or work (w) but it cannot be created or destroyed.

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Thermodynamics Part I: Spontaneity of Rxns

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  1. ThermodynamicsPart I: Spontaneity of Rxns Jespersen Chap. 19 Sec 1 thru 6 Dr. C. Yau Fall 2014 1

  2. First Law of Thermodynamics The first law of thermodynamics states that internal energy (E) may be transferred as heat (q) or work (w) but it cannot be created or destroyed. ΔE = q + w Whatever is not part of the system (sys) is part of the surroundings (surr), and together they constitute the universe (univ): Euniv = Esys + Esurr Since E cannot be created nor destroyed, ΔEuniv = 0 = ΔEsys + ΔEsurr Rearrangement gives… ΔEsys = –ΔEsurr 2

  3. First Law of Thermodynamics • E = internal energy of a system (the sum of the kinetic and potential energy of all its particles) • ΔE = change in the internal energy of system = Eproducts – Ereactants • ΔE = q + w heat work • w = - PΔV where P is atmospheric pressure and ΔV is change in volume • w is called "PV work." 3

  4. First Law of Thermodynamics • w = – PΔV In an exothermic rxn, part of the heat released is used in heating the surrounding gas, which expands and pushes back the atmosphere. Expansion means Vfinal > Vinitialand ΔV = Vfinal – Vinitial , and so ΔV is positive. and w = – PΔV is negative. (P andΔV are both positive.) • Negative w means work is done BY the system, on the surrounding. Internal E of the system is decreased (consistent with the sign.) Volume is increasing, getting larger. 4

  5. Work (w) = – Patm·ΔV In reactions, work is most often due to the expansion or contraction of a system caused by a change in the moles of gases. The deployment of an airbag is one example of this process 1 C3H8(g) + 5 O2(g) →3 CO2(g) + 4 H2O(g) 6 moles of gas→ 7 moles of gas Since PV=nRT, PΔV= ΔnRT. Thus, we can predict the work: w= - PΔV = - ΔnRT (where Δn = 1 for example above)

  6. Some airbags contain sodium azide: NaN3. Did you know it is incorrect to hold wheel at 10-2?

  7. First Law of Thermodynamics What the + and – signs mean.... ΔE = q + w q is + heat is absorbed by the system q is – heat is released by the system w is + work is done on the system w is – work is done by the system ΔE is + internal energy is increased ΔE is – internal energy is decreased 7

  8. q versus ΔH qP is transfer of heat when at constant pressure(when rxn is in an open vessel) qV is transfer of heat when at constant volume(when rxn is in a steel container and so V cannot change) For constant P, H (enthalpy) is defined as H = E + PV and ΔH = ΔE + PΔV rearrangement gives ΔE = ΔH – PΔV but we also know that ΔE = q + w = q + (-PΔV) ΔH – PΔV = q + (-PΔV) simplifies to ΔH = qP 8

  9. q versus ΔH When V is constant, ΔV = 0 and so PΔV = 0 ΔE = q + w ΔE = q –PΔV becomes ΔE = qv Summary: At constant P, qP =ΔH At constant V, qv =ΔE 9

  10. H H products reactants reactants products ΔH = enthalpy change = Hfinal – Hinitial ΔH + endothermic, heat is absorbed ΔH – exothermic, heat is released It would seemexothermic rxns are spontaneous and endothermic rxns are non-spontaneous.

  11. SpontaneousChanges A spontaneous change = change that occurs by itself without an ongoing input of energy from outside the system The burning of a match is spontaneous. Once it is lit, it will burn without further intervention. An ice cube melting at room temp is spontaneous…. BUT it is endothermic! Heat has to be ADDED. Why is it spontaneous??

  12. Entropy (S) Entropy (S) is the degree of disorder. ΔS = change in entropy = Sfinal – Sinitial When a system becomes more disorderly... orderdisorder, chaos smaller S larger S ΔS = Sfinal – Sinitial > 0 (positive) ΔS is + for a process that ends up more disordered.

  13. Entropy (S) • Entropy is a measure of randomness • The more possible arrangement of particles, the higher the entropy • Processes favor high probability (p) Less ways to distribute E Spontaneous process More ways to distribute E Spontaneous processes tend to disperse energy.

  14. Entropy (S) • The greater the number of energetically equivalent versions there are of a system… • the larger is the statistical probability… • therefore the larger the value of the entropy (more randomness) Paper currency: 2 ways to count out $2.00. Coins: 5 ways to count out $2.00 using 50¢ and 25 ¢. Counting with coins has higher entropy than counting with paper money. Fig. 19.7 p.877

  15. Which of the following has the most entropy in standard conditions? • H2O(l) • NaCl(aq) • AlCl3(s) • Can’t tell from the information Which system has more disorder?

  16. Entropy Change with + Sign REMEMBER: ΔS is positive if we end up with more disorder What kind of changes lead to positive ΔS? Energy of motion becomes more dispersed (spread out more). • Volume (of gas) increases • Phase changes (solid to liquid to gas) • Dissolving a salt (solid to solvated ions) • Chem rxns where solid changes to gas; gas to more molecules of gas. • Increase in number of particles • Increase in number of bonds

  17. Factors Affecting Entropy (ΔS) • Mixing • Volume change of gas • Change in physical state

  18. In general, increase in temperature leads to larger disorder (larger entropy). At 0 Kelvin (absolute zero), particles are essentially motionless (S = 0). As T increases, motion increases and S increases.

  19. Fig. 19.11: Entropy is affected by number of particles. Rxn that produces more particles will have a positive S (more spontaneous).

  20. Predict The Sign Of Δ S In The Following: • Dry ice →carbon dioxide gas • Moisture condenses on a cool window • AB →A + B • A drop of food coloring added to a glass of water disperses • 2Al(s) + 3Br2(l) →2AlBr3(s) + - + + -

  21. Example 19.2 p. 880 Predict the algebraic sign of ΔS for the rxns: a) 2 NO2(g) N2O4(g) b) C3H8 (g) + 5O2(g) 3CO2(g) + 4H2O (g) negative # molecules of gas increased ΔS is positive. Do Pract Exer 5, 6, 7 p. 880

  22. Second Law of Thermodynamics Second Law of Thermodynamics states that all real processes occur spontaneously in the direction that increases the entropy of the universe (system plus surroundings). Whenever a spontaneous event takes place in our universe, the total entropy of the universe increases. ΔStotal > 0 (positive) The entropy of the universe is constantly rising. 22

  23. Third Law of Thermodynamics The Third Law of Thermodynamics states that a perfect crystal has zero entropy at absolute zero. Ssys = 0 at 0 K Unlike enthalpy H which cannot be measured (only ΔH can be measured), entropy S can be determined. So = entropy at standard state (what are the conditions of standard state?) 1 atm; at specified temp, usually 25oC; if aqueous, at 1 M concentration. REMEMBER!

  24. Calculating S from S Similar to calculating H from Hf we can calculate S from S of the reactants and products: S =  nS(products) -  nS(reactants) Where n =coefficient in balanced eqn, taking into account # moles of each product/reactant. n has units of moles S usually has units of J/(mol.K) (not kJ/(mol.K)) Thus, nS has units of ....?

  25. Hess’ Law Quick review on Hess’ Law and enthalpy change from Gen Chem I: H° = (sum of nHf° products  sum of nHf° reactants) where n = # moles = coefficient in balanced eqn. What exactly is Hf°? IMPORTANT TO KNOW! It is the enthalpy change for the formation of one mole of substance from its elements at standard states: 25oC, 1 atm, 1M if aqueous soln. Write the corresponding chem eqn for Hf° of… a) Ca3(PO4)2 (s) b) SO2 (g) c) Br2 (l)

  26. Example 19.3 p. 885 Urea ( a cmpd found in urine) is manufactured commercially from CO2 and NH3. One of its uses is as a fertilizer where it reacts slowly with water in the soil to produce ammonia and carbon dioxide. the ammonia provides a source of nitrogen for growing plants. CO(NH2)2(aq) + H2O (l) CO2(g) + 2NH3(g) What is the standard entropy change when one mole of urea reacts with water? p. 885 -Table 19.1 gives standard S values, but Appendix C (p.A-40) gives a very extensive table of thermodynamic values (including ΔHfo and ΔGo values). See next slide.

  27. CO(NH2)2(aq) + H2O (l) CO2(g) + 2NH3(g) Substance So (J/mol K) CO(NH2)2 (aq)173.8 H2O (l) 69.96 CO2 (g)213.6 NH3(g) 192.5 Pay attention to the physical states! H2O (g) 188.7 and O2(g) 205.0 NOT ZERO! Ans. 354.8 J/K Do Pract Exer 9 & 10 p. 887

  28. Putting it all together… Gibbs free energy(G) = H – TΔS At constant T and P, Gibbs free energy change ΔG = ΔH - T ΔS Learn this!! ΔG = Gfinal - Ginitial ΔG, ΔH, ΔS are all state functions. (They are dependent only on their initial and final states and not the pathway of getting there.) A reaction is spontaneous if ΔG is negative. (Gfinal is less than Ginitial)

  29. Prediction of Spontaneity Negative G = process is spontaneous Negative H (exothermic) promotes spontaneity. Positive S (towards more disorder) promotes spontaneity. So, an exothermic reaction that leads to more disorder would be a spontaneous rxn. ΔG = ΔH - T ΔS LEARN THIS NOW! T always positive....WHY? Negative Positive

  30. Gibbs Free Energy & Spontaneity ΔG = ΔH - T ΔS Note the role of temperature (T). It determines how important the S term is to be. At high T, the entropy factor plays an important role. IfS is + (promoting spontaneity), at high T, the rxn is said to be “entropy driven.” IfS is - & H is - (H, not S, is promoting spontaneity), at low T, the rxn is said to be “enthalpy driven.” Before we do the calculations, let's examine the conditions when ΔG is negative. What is the significance of it being neg.?

  31. G° = H°  T S° Remember rxn is spontaneous when G° = - • H° = - and S°= + G°= - at all temp exothermicto more disorder • H° = - and S°= -G°= - at low temp exothermic to less disorder (at low T, rxn is “enthalpy driven”.) • H° = + and S°= -G°= + at all temp endothermic to less disorder • H° = + and S°= + G°= - at high temp endothermic to more disorder (at hi T, rxn is “entropy driven”.) When H° and S° have the same sign, spontaneity is determined by the temperature.

  32. Fig. 19.13 p. 884 When H° and S° have the same sign, spontaneity is determined by the temperature.

  33. Gibbs Free Energy & Spontaneity You did this type of calculation in Paper HW#5 already. You can calculate ΔG by 2 methods: (depending on which information is available) 1) G° = (of nGf° of products)  ( of nGf° of reactants) where n = # moles = coefficient in balanced eqn. 2) G° = H°  T S° where H° = ( of nHf° products  of nHf° reactants) S° = ( of nS° products nS° reactants)

  34. Calculate ΔG0 for the following using both approaches at 298K: CaCO3(s)→CO2(g) + CaO(s) Which approach is needed if you want ΔG0at 500K? (Which approach has a T term in it?)

  35. Example 19.4 p. 887 Calculate ΔGo from values of ΔHo and ΔSo for CO(NH2)2(aq) + H2O (l) CO2(g) + 2NH3(g) Table 7.2 p. 285 gives you ΔHfo values and Table 19.1 p. 885 gives you So values. Alternatively, you can go to Appendix C and get them all there. ΔSo we already calculated in Example 18.3 (354.8 J/K) ΔHo comes out to be 191.2 kJ. What is ΔGo? Ans. + 13.4 KJ

  36. Effect of T on ΔG Example 19.9 p. 899 N2O4(g) 2NO2(g) at 25oC the value of ΔGo for the reaction is +5.40 kJ. What is the approximate value of ΔGo for the reaction at 100oC? Which method are you going to use to calculate ΔG? Why can’t we calc with G° = G(products) -  G(reactants) for 100oC? Ans. ΔGo at 100oC is – 8.1 kJ ΔGo at 25oC is +5.40 kJ Nonspontaneous rxn became spontaneous at 100oC. How?? This means G° = H°  T S° H° is positive and S° is positive. (does not promote spont.)(promotes spontaneity) At high temperature, the rxn is "entropy driven". Do Pract Exer 21, 22 p. 900

  37. G° = H°  T S° When is the reaction “enthalpy-driven”? What does that mean?.... …spontaneity is governed by the enthalpy alone, not by entropy. (G neg; S neg) …enthalpy-driven at low T, but what other factor that would make  T S° negligible? What condition would cause S° to be near zero? Compare: a) CaO(s) + SO2(g) CaSO3(s) b) 3CaO(s) + 2Fe(s) 3Ca(s) + Fe2O3(s)

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