CH301 Worksheet 11 1. What is the second law of thermodynamics? How does this apply to someone exploding ahydrogen balloon? 2 H2(g) + O2(g) → 2 H20(g)2. Let's talk about signs. What does a positive or negative value mean for change inenthalpy (ΔH), work (w), and change in Gibb's free energy (ΔG)? Remember, be thesystem! And try to do this one from memory. Don't just copy it directly from the notes.3. A bomb calorimeter is filled with 2 L of water. After a reaction, the temperature of thewater raises from 25.0 °C to 28.3 °C. The density and heat capacity of water are 1 g/mLand 4.184 J/(g∙K), respectively. The heat capacity of the calorimeter is 85 J per K.Determine ΔH of the reaction.4. The same bomb calorimeter is filled with 2 L of a liquid that has a density of 1.7 gramsper mL. A reaction releases 250 kJ of heat, and the temperature of the liquid increases from25 °C to 27 °C. What is the heat capacity of the liquid?5. The liquid is allowed to cool down to 25 °C. The calorimeter is equipped with anotherreaction that releases 400 kJ of heat. What is the final temperature of the liquid after thereaction is complete?6. Balance the following reaction of hydrazine with methanol. Calculate the work done.N2H2(l) + CH3OH(l) → CH2O(g) + N2(g) + H2(g)7. If the work done on a system is 5.7 kJ, and the external pressure is equal to 3.5 atm. Isthe volume of the system increasing or decreasing?8. In your own words, what is Hess's Law?9. Use the following data to calculate the change in enthalpy.Overall reaction: H2S (g) + 2 O2(g) → S03(g) + H2O(l)1. H2SO4(l) → H2S(g) + 2 O2(g) ΔH = 78.5 kJ2. H2SO4(l) → SO3(g) + H2O(g) ΔH = 20.5 kJ3. H2O(g) → H2O(l) ΔH = -11 kJ10. Use the following data to calculate the change in enthalpy.Overall reaction: N2H4(l) + H2(g) → 2NH3(g)1. N2H4(l) + CH4O(l) → CH2O(g) + N2(g) + 3H2(g) ΔH=-185KJ2. N2(g) + 3H2(g) → 2NH3(g) ΔH=-230KJ3. CH4O(l) → CH2O(g) + H2(g) ΔH=-325KJ11. Determine the ΔHrxnfor the reaction using the provided bond energies:CH4(g) + I2(g) → CH3I(g) + HI (g)Bond energies:C-H : 416 kJ/mol H-I: 299 kJ/molI-I: 151 kJ/mol C-I: 213 kJ/molIs the reaction endothermic or exothermic?12. Determine the boiling point for iron. ΔHvap= 349.6 kJ/mol and ΔSvap= 111.55J/(mol∙K)13. Calculate the amount of heat given off when 11 grams of manganese (Mn) is oxidized toMn2O3(s) at standard state conditions. ΔHf,Mn2O3(s) = -962.3 kJ/mol14. Calculate the work done on the systems with only one mole of reactant:a. 2NO2 (g) → N2O4 (g) at 30 °Cb. 2NO (g) → N2 (g) + O2 (g) at 300 °C15. Calculate ΔSuniverseafter the completion of the following reaction:2NiS(s) + 3O2(g) → 2SO2(g) + 2NiO(s) at 25 °C ΔH = -890 kJSubstance S(J/Kmole)SO2248NiO 38O2205NiS 5316. Determine the ΔG when:ΔSuniverse= 1303 J/KΔSsurr= 1.300 kJ/KT = 25 °C17. Balance the following combustion reaction and determine the ΔHrxn.C7H16 + O2 → CO2 + H20Bond EnergiesC-C: 346 kJ/mol O=O: 498 kJ/molC-H: 413 kJ/mol C=O: 799 kJ/molH-O: 463 kJ/mol C-O: 358 kJ/molO-O: 146 kJ/molIf the reaction is carried out at 25 °C what is the ΔSsurr?18. Determine the minimum temperature for a reaction with ΔH = 271 kJ and ΔS = 195 J/Kto be spontaneous.19. Consider the reaction: CO(g) + Cl2(g) → COCl2(g)Calculate ΔGrxnat 25 °CSubstance ΔHf (kJ/mol) S (J/ mol K)CO -110.5 197.6Cl2 0.0 223.0COCl2 -223.0 289.220. Determine ΔGffor SO2(g). Assume 25 °C for all reactions.ΔHf,SO2(g) = -297 kJ/molSm,SO2(g) = 248 J/(K mol)Then determine ΔGrxn of the following reaction:ΔGf Cu2S (s) = -86.2 kJ/molCu2S(s) + O2(g) → SO2(g) +
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