Ch 10 Supplemental InstructionIowa State UniversityLeader: LaurenCourse: Chem 167Instructor: HolmeDate: 10/29/091. Decide whether the following are true or false. If it is false, revise the unbolded part of the sentence to make it true. a) Plastics will decrease in quality when recycled because nature tends to move T F towards disorder. b) A spontaneous process is one that will stop without intervention. T F c) The formation of CH4 and O2 molecules from CO2 and H2O at room temp T F and 1 atm of pressure is a spontaneous process. d) w and q are not state functions, but entropy is. T F e) Most spontaneous processes are exothermic. Explain. T F f) Nature tends to move towards more order. T F2. Consider the vaporization of liquid water to steam at a pressure of 1 atm. a) Is this process endothermic or exothermic? b) In what temperature range is it a spontaneous process? c) In what temperature range is it a nonspontaneous process? d) At what temperature are the two phases in equilibrium?3. What is entropy?Supplemental Instruction1060 Hixson-Lied Student Success Center v 294-6624 v www.si.iastate.edu4. There are many different ways with which energy can be distributed among particles. Therefore, there are many _______________, or manners in which a collection of particles attain a particular energy.5. The higher the entropy, the __________ the number of microstates.6. The normal boiling point of methanol (CH3OH) is 64.7⁰C, and its molar enthalpy of vaporization is ∆Hvap = 71.8 kJ/mol. a) When CH3OH(l) boils at its normal boiling point, does its entropy increase or decrease? b) Calculate the value of ∆S (in J/K) when 1.00 mol of CH3OH(l) is vaporized at 64.7⁰C. 7. Would the following reaction represent a negative or positive change in entropy? Why? 2 SO2(g) + O2(g) 2SO3(g) 8. What is the 2nd law of thermodynamics?9. In a certain spontaneous process the system undergoes an entropy change, ∆S = 42 J/K. What can you conclude about ∆Ssurr?10. To create order in one place, a process must create _________ (more, less, no) disorder somewhere else.11. Hess’s Law: The heat evolved in a given process can be expressed as the sum of the heats of several processes that, when added, yield the process of interest. Based on this definition, complete the following problem (you may have to switch a process around to get the desired final equation. Calculate the enthalpy change for the reaction P4O6(s) + 2O2(g) P4O10 given the following enthalpies of reaction: P4(s) + 3O2(g) P4O6(s) ∆H = -1640.1 kJ P4(s) + 5O2(g) P4O10(s) ∆H = -2940.1