Thermodynamics Temperature Vs Heat Temperature Heat K C

Thermodynamics

Temperature Vs. Heat Temperature Heat K, °C k. J, kcal (Cal) Measure of average KE of motion of particles 1 kcal=4. 184 k. J Measure of total energy transferred from an object of high E to low E Note: A change in T is accompanied by a transfer of energy

Specific Heat c or cp specific for each substance = amount of energy required to raise the temperature of 1 g of a substance by 1°C

Thinking about specific heat List the following substances in terms of specific heat, from lowest to highest: water, gold, ethanol, granite

Thinking about specific heat List the following substances in terms of specific heat, from lowest to highest: Answer: gold, granite, ethanol, water 0. 129 0. 803 2. 44 4. 184 J/g·o. C

Relationship among temperature, heat and mass Change in heat = specific heat x mass x change in T q = cp x m x Units: heat absorbed or released, J cp in J/g·°C m in g ΔT in °C or K Δt

Example Problems 1. How much heat energy is released to your body when a cup of hot tea containing 200. g of water is cooled from 65. 0 o. C to body temperature, 37. 0 o. C? (cp. H 2 O = 4. 18 J/g·o. C) A: 23. 4 k. J

Example Problems 2. A 4. 50 -g nugget of pure gold absorbed 276 J of heat. What was the final temperature of the gold if the initial temperature was 25. 0 o. C? (cp of gold = 0. 129 J/g·o. C) Hint: begin by solving for DT A: 500. o. C

Example Problems 3. A 155 g sample of an unknown substance was heated from 25. 0 o. C to 40. 0 o. C. In the process, the substance absorbed 5696 J of energy. What is the specific heat of the substance? A: 2. 45 J/g·o. C

Using a Calorimeter (WS) 1. Put dried food sample in “bomb” 2. Burn it 3. Use ∆T of water to calculate ∆Hcomb of the food. 4. The amount of energy in food is measured in Cal, rather than k. J. 5. 1 Calorie = 1 kcal = 4. 184 k. J

Calorimetry Step 1 Calculate q from calorimeter data. q. H 2 O = cp. H 2 O x m. H 2 O x Dt. H 2 O Step 2 Relate q to the quantity of substance in the calorimeter.

Calorimetry Problem What is the heat of combustion, DHc , of sucrose, C 12 H 22 O 11, if 1. 500 g of sugar raises the temperature of water (3. 00 kg) in a bomb calorimeter from 18. 00 o. C to 19. 97 o. C? (cp. H 2 O = 4. 18 J/g·o. C) A: 16. 5 k. J/g sucrose, 5650 k. J/mol sucrose

Calorimetry Practice Problem You burned 1. 30 g of peanuts below an aluminum can which contained 200. 0 m. L of ice water (DH 2 O = 1. 00 g/m. L). The temperature of the water increased from 6. 7 o. C to 28. 5 o. C. Assume all of the heat energy produced by the peanuts went into the water in the can. (cp. H 2 O = 4. 18 J/go. C) What was the energy content of peanuts, in k. J/g (i. e. DHcomb of peanuts? A: 14. 0 k. J/g

Calorimetry Problem, p. 881, #6 (Honors) A 75. 0 g sample of a metal is placed in boiling water until its temperature is 100. 0 o. C. A calorimeter contains 100. 0 g of water at a temperature of 24. 4 o. C. The metal sample is removed from the boiling water and immediately placed in water in the calorimeter. The final temperature of the metal and water in the calorimeter is 34. 9 o. C. Assuming that the calorimeter provides perfect insulation, what is the specific heat of the metal? A: 0. 900 J/g·o. C

Enthalpy enthalpien= to warm (Greek) Enthalpy (H) = total E of a substance Enthalpy change (ΔH) = comparison between H of products and H of reactants in a reaction (ΔH=Hproducts Hreactants)

Heats of … ΔH = change in enthalpy (i. e. change in the amount of heat) The heat change which occurs during processes can be described as ΔHx, x=process name ΔHcomb= … combustion ΔHfus= … fusion ΔHvap= … vaporization ΔHrxn= … reaction ΔHf°= … formation ΔHsol= … solution Units: All in k. J/mol except heats of reaction and solution, which are just in k. J

Thermodynamics Word Problems Using DHx Data e. g. Calculate the heat required to melt 25. 7 g of solid methanol at its melting point. DHfus of methanol = 3. 22 k. J/mol (from Table 16 -6 on p. 502) 1. Convert mass of methanol to moles. 2. Multiply moles of methanol by DHfus. A: 2. 58 k. J

Thermodynamics Word Problems Using DHx Data How much heat is needed to vaporize 343 g of acetic acid (CH 3 COOH)? DHvap = 38. 6 k. J/mol (A = 220. k. J)

Temperature Changes of Water (WS)

Using Heat of Fusion Use Table 16 -6 on p. 502 for DHvapo and DHfuso for different substances. Calculate the energy required to melt 8. 5 g of ice at 0 o. C. The molar heat of fusion for ice is 6. 02 k. J/mol. A: 2. 8 k. J

Using Heat of Vaporization Calculate the total energy change (in k. J) required to a) heat 25 g of liquid water from 25 o. C to 100. o. C, then b) change it to steam at 100. o. C. cpliquid water = 4. 18 J/go. C, DHvap. H 2 O = 40. 6 k. J/mol. A: a) 7. 8 k. J b) 56 k. J Total = 64 k. J

Thermochemical Stoichiometry The amount of energy (in k. J) can be incorporated into mole ratios. C 6 H 12 O 6(aq) + 6 O 2(g) 6 CO 2(g) + 6 H 2 O(l) + 2870 k. J ΔH = -2870 k. J/mol glucose Mole Ratios Examples 1 mol C 6 H 12 O 6 6 mol O 2 2870 k. J 6 mol 1 mol 6 mol CO 2 C 6 H 12 O 6 H 2 O 2870 k. J

Thermochemical Stoichiometry Problems C 6 H 12 O 6(aq) + 6 O 2(g) 6 CO 2(g) + 6 H 2 O(l) + 2870 k. J 1. How much energy (in k. J) will be released when 675 g of glucose is burned? A: 10, 800 k. J

Thermochemical Stoichiometry Problems C 6 H 12 O 6(aq) + 6 O 2(g) 6 CO 2(g) + 6 H 2 O(l) + 2870 k. J 2. If 398 k. J is released when a certain amount of glucose is burned, how many grams of oxygen are consumed? A: 26. 6 g

Thermochemical Stoichiometry Problems C 6 H 12 O 6(aq) + 6 O 2(g) 6 CO 2(g) + 6 H 2 O(l) + 2870 k. J 3. If 5782 k. J is released when a certain amount of glucose is burned, how many liters of carbon dioxide are released, assuming the reaction takes place at STP? A: 271 L

Enthalpy ΔHrxn is + if endothermic (energy of products > energy of reactants) ΔHrxn is - if exothermic (energy of reactants > energy of products) 2 H 2 + O 2 2 H 2 O + 483. 6 k. J DH = - 483. 6 k. J

Hess’s Law The total enthalpy change for a chemical or physical change is the same whether it takes place in one or several steps.

Hess’s Law Version 1: Add equations together Version 2: Use heats of formation (DHfo) of products and reactants

Hess’s Law Version 1 Example: What is the change in enthalpy for converting graphite to diamond? Given: C(graphite) + O 2(g) CO 2(g) DH = -393. 5 k. J/mol C C(diamond) + O 2(g) CO 2(g) Step 1: Write rxn: DH = -395. 4 k. J/mol C C(graphite) C(diamond) Step 2: Add up rxns to get total rxn, canceling similar terms. C(graphite) + O 2(g) CO 2(g) DH = -393. 5 k. J/mol C C(diamond) + O 2(g) DH = +395. 4 k. J/mol C CO 2(g) _______________________ C(graphite) Note: C(diamond) DH = +1. 9 k. J/mol C Focus is on the DH. Adding equations is the way you get there.

Hess’s Law Version 1 Practice Calculate the heat of formation of pentane (C 5 H 12). Given: C(s) + O 2(g) CO 2(g) DH = -393. 51 k. J/mol H 2(g) + ½ O 2(g) H 2 O(l) DH = -285. 83 k. J/mol C 5 H 12(l) + 8 O 2(g) 5 CO 2(g) + 6 H 2 O(l) DH = -3536. 1 k. J/mol Final equation: 5 C(s) + 6 H 2(g) C 5 H 12(l) (A: -146. 4 k. J) DHfo = ?

Hess’s Law (Version 2) The enthalpy change of a rxn is equal to the heats of formation of the products minus the heats of formation of the reactants (and taking stoichiometric relationships into account). DH = SDHfo (products) – SDHfo (reactants)

Hess’s Law (Version 2) Example: Calculate ΔH for this reaction CH 4(g) + 2 O 2 g) CO 2(g) + 2 H 2 O(l) Given: DHfo CO 2(g)= -393. 5 k. J/mol DHfo H 2 O(l) = -285. 8 k. J/mol DHfo CH 4(g) = -74. 86 k. J/mol DHfo O 2(g) = 0 (Note: DHfo of free elements = 0)

Hess’s Law (Version 2) Step 1: Calculate the total DHfo for the products and the reactants. DHproducts = (-393. 5 k. J)(1 mol CO 2) + (-285. 8 k. J)(2 mol H 2 O) 1 mol = -965. 1 k. J DHreactants = (-74. 86 k. J)(1 mol CH 4) 1 mol = -74. 86 k. J

Hess’s Law (Version 2) Step 2: Plug these values into the following equation. DHrxn = DHproducts – DHreactants = -965. 1 k. J – (-74. 86 k. J) = -890. 2 k. J

Hess’s Law (Version 2) Practice Use standard enthalpies of formation from Appendix C, Table C-13 on p. 921 to calculate DHorxn for the following reaction: 4 NH 3(g) + 7 O 2(g) 4 NO 2(g) + 6 H 2 O(l) A: -1397. 9 k. J

Hess’s Law (Version 2) Practice Use standard enthalpies of formation from Appendix C, Table C-13 to calculate DHorxn for thermite reaction: 2 Al(s) + Fe 2 O 3(s) 2 Fe(s) + Al 2 O 3(s) A: - 851. 5 k. J

Reaction Pathways Why don’t exothermic reactions occur spontaneously (e. g. with no spark)? Energy is needed to overcome the mutual repelling of the atoms involved in the reaction.

Reaction Pathways Activation energy (Ea) = initial input of energy Note: Different reactions have different activation energies.

Reaction Profiles (WS) Exothermic Reaction Endothermic Reaction (a) Activation energy (b) Energy released by activated complex (c) ∆Hrxn = Hproducts – Hreactants

Effect of Adding a Catalyst on Reaction Rates

Entropy: S en- (Greek, = in) trope (Greek, = a turning) Entropy: degree of disorder or chaos In nature, things tend toward disorder It is usually much easier to go from low S to high S All chemical/physical changes involve changes in entropy. This natural tendency to disorder can be overcome by enthalpy.

Change in Entropy: ∆S Entropy change (∆S) = comparison in entropy of the products and reactants in a chemical equation ∆S = Sproducts – Sreactants +∆S increased entropy: S products > S reactants -∆S decreased entropy: S products < S reactants Units of S = J/mol • K Always use K in S calculations

Factors that Increase Entropy state change from solid to liquid to gas increased temperature (more collisions, more disorder) more particles of product than reactant (decomposition, dissolving)

Calculating ∆S from So ΔS = S°Products - S°Reactants Use the information in the table below to calculate ∆S for the following reaction: 2 SO 2(g) + O 2(g) 2 SO 3(g) ∆Hfo (k. J/mol) So (J/K. mol) SO 2(g) -297 248 SO 3(g) -396 257 O 0 [2 mol SO 3(257 J/mol K)] – 514 J/K – 701 J/K = -187 J/K Would this be favored? 2(g) [2 mol SO 2 (248 J/mol K) + 1 mol O 2(205 J/mol K)] = 205

Spontaneity Spontaneous = happens Spontaneity depends on: ∆S and ∆H of reaction Example: Combustion of octane is spontaneous 2 C 8 H 18(l) + 25 O 2(g) 16 CO 2(g) + 18 H 2 O(g) + k. J Exothermic Reaction (-∆H) Entropy increased (+∆S) due to More particle energy (l) (g) More product particles

Spontaneous Reactions Spontaneity depends on 1. Change in entropy of reaction (DS) 2. Change in enthalpy of reaction (DH) 3. Temperature (T in K) Gibbs Free Energy calculation

Gibbs Free Energy ΔG = ΔH - (TΔS) ΔG = - k. J; yes! spontaneous ΔG = + k. J; no! nonspontaneous

Gibbs Free Energy: ∆G = ∆H - T∆S Reaction is spontaneous if the sign of ∆G is negative. Is this reaction spontaneous @ 25 o. C? 2 SO 2(g) + O 2(g) 2 SO 3(g) T 298 K Favored? ∆H - 198 k. J Y ∆S -187 J/K N To take both the change in enthalpy AND entropy into account, calculate ∆G: ∆G = ∆H - T∆S = -198 k. J – 298 K (-0. 187 k. J/K) watch the units… = -198 k. J – (-55. 7 k. J) = -142 k. J So, is this reaction spontaneous at 298 K? YES.

Gibbs Free Energy: ∆G = ∆H - T∆S Is this reaction spontaneous @ 2000. K? 2 SO 2(g) + O 2(g) 2 SO 3(g) T 2000 K Favored? ∆H - 198. 2 k. J Y ∆S -187 J/K N ∆G = ∆H - T∆S = -198. 2 k. J – 2000. K (-0. 187 k. J/K) = -198. 2 k. J – (-374 k. J) = 176 k. J So, is this reaction spontaneous at 2000. K? NO. The reaction is spontaneous at low temps (enthalpy wins) but not spontaneous at very high temps (entropy wins) (decomposition occurs…. )

Gibbs Free Energy Will thermite reaction occur spontaneously at room temperature (298 K)? 2 Al(s) + Fe 2 O 3(s) 2 Fe(s) + Al 2 O 3(s) DH = -851. 5 k. J DS = -0. 038 k. J/K DG = ?

Gibbs Free Energy: ∆G = ∆H - T∆S Will thermite reaction occur spontaneously at room temp (298 K)? 2 Al(s) + Fe 2 O 3(s) ➝ 2 Fe(s) + Al 2 O 3(s) ∆H = -851. 5 k. J ∆S = -0. 038 k. J/K ∆G = ? -851. 5 k. J – [298 K (-0. 038 k. J/K)] = - 840 k. J Yes, ∆G is negative

Free Energy Practice Problems (extra) 1. For the reaction NH 4 Cl(s) NH 3(g) + HCl at 25 o. C, DH = 176 k. J/mol, DS = 0. 285 k. J/mol. K Calculate DG and decide if the reaction will be spontaneous in the forward direction at 25 o. C.

Free Energy Practice Problems extra 2. When graphite (C) reacts with hydrogen at 27 o. C, DH = -74. 8 k. J/mol and DS = -0. 0809 k. J/mol. K. Will this reaction occur spontaneously?

Free Energy Practice Problems extra 3. Calculate the standard entropy change, DS, that occurs when 1 mol H 2 O(g) is condensed to 1 mol H 2 O(l) at 25 o. C. So H 2 O(g) = 188. 7 J/mol. K So H 2 O(l) = 69. 94 J/mol. K

Free Energy Practice Problems extra 4. For the reaction H 2 O(g) + C(s) CO(g) + H 2 O(g), DH = 131. 3 k. J/mol, DS = 0. 134 k. J/mol. K a) Is the reaction spontaneous at 1350 K? b) At what temperature is the reaction spontaneous?

Relating Entropy and Enthalpy to Spontaneity: DG = DH – (TDS) DH DS Spontaneity Example (Is DG negative? ) (-) (+) exothermic disorder (-) value (-) exothermic order (+) value (+) endothermic disorder (+) value endothermic (-) order yes 2 K(s) + 2 H 2 O(l) 2 KOH(aq) + H 2(g) Yes at low T H 2 O(g) H 2 O(l) Yes at high T (NH 4)2 CO 3(s) 2 NH 3(g) + CO 2(g) + H 2 O(g) no 16 CO 2(g) + 18 H 2 O(l) 2 C 8 H 18(l)+25 O 2(g)