ch19_chemical_thermodynamics

ch19_chemical_thermodynamics - ∆ S value for a...

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Chapter 19: Chemical Thermodynamics 1. What is the 1 st law of thermodynamics? 2. If a process is nonspontaneous, can it occur? Explain. 3. What is the 2 nd law of thermodynamics? 4. During a reversible process, the surroundings undergo an entropy change, ΔSsurr = -78 J/K. What is the entropy change of the system for this process? 5. What is the 3 rd law of thermodynamics? 6. Define three different types of motion that molecules can undergo. 7. Label each process as exhibiting an increase or decrease in entropy of the system. a. CaCO 3 (s) CaO(s) + CO 2 (g) b. H 2 O(l) H 2 O(s) c. N 2 (g) + 3H 2 (g) 2NH 3 (g) d. H 2 O(s) H 2 O(g) 8. Given that the process of dissolving NaCl in water absorbs 3.9 kJ/mol of heat, what is the sign for ΔH of this reaction? Is this reaction endothermic or exothermic? NaCl(s) Na + (aq) + Cl - (aq) 9. If the H value for a spontaneous process is greater than zero, what is the sign of S?
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Unformatted text preview: ∆ S value for a spontaneous process is less than zero, what is the sign of ∆ H? 11. What is the sign of ∆ S when solid copper is cooled from 100 ° C to 25 ° C? Why? 12. Given the following reaction: 2A(g) → 3B(g) a. If ΔG ° for A is –370.4 kJ/mol and B is –300.4 kJ/mol at 25 ° C, what is ΔG ° ? b. Is the reaction spontaneous? c. Calculate ΔG r when the partial pressure of A is 2atm and B is 3atm. 13. The partial pressures of NO 2 and N 2 O 4 in a reaction flask at 298K are 0.30atm and 0.15atm, respectively. What is the value of ΔG r under conditions for 2NO 2 (g) → N 2 O 4 (g) if K = 8.8? 13. Predict the sign of ∆ G ° for reactions with each of the following equilibrium constants: a. K << 1 b. K = 1 c. K >>1 14. If K < Q, is a reaction spontaneous as written? 15. If ΔG r ° = -15.94kJ/mol, what is the value of K?...
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ch19_chemical_thermodynamics - ∆ S value for a...

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