RecitationSheet_Chp18

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CHEM 1040 Chapter 18 Recitation Sheet Name:_____________________________ What is entropy? Draw a particle view of a process demonstrating an increase in entropy. Before After à What is the sign of ΔS if there is an increase in entropy? Decrease in entropy? What are some things to look for in changes in entropy? Predict the sign of ΔS sys for the following processes (+,-,?): Process ΔS sys H 2 O (g) à H 2 O (l) Solid carbon dioxide sublimes 2 N 2 O (g) à 2 N 2 (g) + O 2 (g) Boiling of water I 2 (g) à I 2 (s) CaCO 3 (g) à CaO (s) + O 2 (g) What is the definition of a spontaneous process? Label the following processes as spontaneous, non- spontaneous, or not enough information. The combustion of natural gas The extraction of iron metal from iron ore A hot drink cooling to room temperature A bike going uphill A meteor falling to earth Obtaining hydrogen gas from liquid water A ball rolling down hill Metal rusting 2 N 2 O (g) à 2 N 2 (g) + O 2 (g) Entropy is typically reported with what units? What is the formula for calculating ΔS ° of a system? Using the Appendix, calculate the following ΔS ° sys CH 3 CH 2 OH (l) + 3 O 2 (g) à 2 CO 2 (g) + 3 H 2 O (g) Before calculating, what should the sign of ΔS ° sys be? Calculate ΔS ° sys (in J/mol·k)
ΔH° (kJ/mol) S° (J/mol·K) ΔG° (kJ/mol) CH 4 (g) -74.85 186.2 -50.8 O 2 (g) 205.0 CO 2 (g) -393.5 213.6 -394.4 H 2 O (l) -285.8 69.9 -237.2 The missing values are a definition. What is the equation for calculating Δ of anything? What is the ΔH° rxn for CH 4 (g) + 2 O 2 (g) à CO 2 (g) + 2 H 2 O (l) What is the ΔS° rxn ? What is the formula to calculate ΔG° from ΔH° and ΔS°? Calculate ΔG rxn of the previous reaction with CH 4 using your calculated ΔH° and ΔS° values. Using ΔG° values from the table, what is ΔG° rxn ? Should the numbers be about the same? Fill in the blanks ΔH ΔS ΔG Spontaneous? - + + - + + - -
Mark if the reaction is spontaneous, non-spontaneous, or not enough information a) A solid decomposes into a solid and a gas and is exothermic ⃝ Spontaneous ⃝ Non-spontaneous ⃝ Not enough info b) Two liquids react to form a gas and is endothermic ⃝ Spontaneous ⃝ Non-spontaneous ⃝ Not enough info c) Boiling water at 0 ° C ⃝ Spontaneous ⃝ Non-spontaneous ⃝ Not enough info d) A (g) + B (g) à C(g); ΔH rxn = -33.25 kJ ⃝ Spontaneous ⃝ Non-spontaneous ⃝ Not enough info A reaction has a ΔH rxn = +23.25 kJ and ΔS was +161.26 J/mol·K. At what temperatures is this reaction spontaneous? Using the reaction d, ΔS ° was -150.66 J/mol·K Without calculating, when is this reaction spontaneous? What is the boundary line between negative and positive? At what temperature is that boundary line? At what temperatures is this reaction spontaneous? How are Δ G and Δ G o different? What equation represents their relationship? Δ G o of H 2 (g) + I 2 (s) ⇌ 2 HI (g) is +2.60 kJ/mol at 25 o C Is this reaction spontaneous under those conditions? ⃝ Yes ⃝ No If the starting concentrations are P H2 = 5.35 atm and P HI = 1.75 atm, what is Q (note phases)? What is the value of Δ G for those conditions? Is this reaction spontaneous under these conditions? ⃝ Yes ⃝ No What is the value of K (hint: what is Δ G at equilibrium)?
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Using the thermodynamic chart provided, what is the K value for the following reaction at 25 °C? ࠵?࠵? ! (࠵?) + ࠵? " ࠵?(࠵?) ⇌ 3H " (࠵?) + ࠵?࠵?(࠵?) Δ G o (kJ/mol) CH 4 (g) -50.8 H 2 O (g) -228.6 CO (g) -137.2 CO 2 (g) -394.4 How do you calculate Δ G o rxn ? What is the relationship between K and Δ G o rxn ? What is K for this reaction? Using the thermodynamic chart provided above, what is the K value for the following reaction at 25 o C? ࠵?࠵? ! (࠵?) + 2 ࠵? " (࠵?) ⇌ 2 H " ࠵?(࠵?) + ࠵?࠵? " (࠵?)

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