Ch 10 (II)Supplemental InstructionIowa State UniversityLeader: LaurenCourse: Chem 167Instructor: HolmeDate: 11/01/091. Using values from Appendix E, calculate the standard enthalpy change for each of the following reactions: a) 2 SO2(g) + O2(g) 2 SO3(g) b) Mg(OH)2(s) MgO(s) + H2O(l) c) CH4(g) + 4 Cl2(g) CCl4(l) + 4 HCl(g) d) SiCl4(l) + 2 H2O(l) SiO2(s) + 4 HCl(g)2. Complete combustion of 1 mol of acetone (C3H6O) gives of 1790 kJ of heat: C3H6O(l) + 4 O2(g) 3 CO2(g) + 3 H2O(l) ∆H = -1790 kJ Using this information together with data from Appendix E, calculate the enthalpy of formation of acetone.3. What is the third law of thermodynamics?4. Use Appendix E to compare the standard entropies at 25⁰C for the following pairs of substances, and explain the difference in entropy values: a) Sc(s) and Sc(g) b) NH3(g) and NH3(aq) c) 1 mol P4(g) and 2 mol P2(g) d) C(graphite) and C(diamond)Supplemental Instruction1060 Hixson-Lied Student Success Center v 294-6624 v www.si.iastate.edu5. Using S⁰ values from Appendix E, calculate ∆S⁰ values for the following reactions. In each case account for the sign of ∆S⁰. a) C2H4(g) + H2(g) C2H6(g) b) Be(OH)2(s) BeO(s) + H2O(g)6. Spontaneous processes that occur with a decrease in the system’s entropy are exothermic. There are also spontaneous processes that occur with an increase in the system’s entropy, and those tend to be endothermic. So, the spontaneity of a reaction seems to involve two thermodynamic concepts: enthalpy and entropy, which are used in a new state function, __________________________. (∆G = ∆H - T∆S)7. If the reaction is exothermic, then the spontaneous reaction is ______________ driven. If the system increases in randomness, than the spontaneous reaction is _______________ driven.8. a) If ∆G is _____ (-,+,0), the reaction is spontaneous in the forward direction. b) If ∆G is _____ (-,+,0), the reaction is at equilibrium. c) If ∆G is _____ (-,+,0), the reaction in the forward direction is nonspontaneous. 9. For a certain chemical reaction, ∆H⁰ = -35.4 kJ and ∆S⁰ = -85.5 J/K. a) Is the reaction exothermic or endothermic? b) Does the reaction lead to an increase or decrease in the disorder of the system? c) Calculate ∆G⁰ for the reaction at 298 K. d) Is the reaction spontaneous at 298 K under standard conditions? If it is, is it entropy or enthalpy