MISSED THIS? Read Sections 19.8 (Page),19.10 (Page); Watch IWE 19.11.Estimate the value of the equilibrium constant at690 K for each of the following reactions usingthermodynamic data from the appendix.#Part A2NO2 (g) = N₂O4(g)AH for N₂O4 (g) is 9.16 kJ/mol.Express your answer using three significant figures.► View Available Hint(s)VE ΑΣΦΑ »K = 3.09SubmitPart BPrevious Answers Request AnswerX Incorrect; Try Again; 2 attempts remainingBr2 (g) + Cl₂ (g) = 2BrCl(g)AH for BrCl(g) is 14.6 kJ/mol. AS for BrCl(g) is 240.0 J/mol.Express your answer using three significant figures.► View Available Hint(s)Submit[ΫΠ| ΑΣΦK = 4.83S?CPrevious Answers Request Answer?

Answered: Image /qna-images/answer/29969312-669a-4708-8301-6163008ff4e0.jpg

MISSED THIS? Read Sections 19.8 (Page), 19.10 (Page); Watch [WE 19.11. Estimate the value of the equilibrium constant at 690 K for each of the following reactions using thermodynamic data from the appendix. ▼ 2NO2(g) = N2O4 (g) AH; for N₂O4 (g) is 9.16 kJ/mol. Express your answer using three significant figures. ▸ View Available Hint(s) K= 3.09 Submit [5] ΑΣΦ Part B Previous Answers Request Answer X Incorrect; Try Again; 2 attempts remaining Br2 (g) + Cl₂ (g) = 2BrCl(g) AH for BrCl(g) is 14.6 kJ/mol. AS for BrCl(g) is 240.0 J/mol. Express your answer using three significant figures. View Available Hint(s) [5] ΑΣΦ K = 4.83 Submit ? Previous Answers Request Answer ?

MISSED THIS? Read Sections 19.8 (Page), 19.10 (Page); Watch [WE 19.11. Estimate the value of the equilibrium constant at 690 K for each of the following reactions using thermodynamic data from the appendix. ▼ 2NO2(g) = N2O4 (g) AH; for N₂O4 (g) is 9.16 kJ/mol. Express your answer using three significant figures. ▸ View Available Hint(s) K= 3.09 Submit [5] ΑΣΦ Part B Previous Answers Request Answer X Incorrect; Try Again; 2 attempts remaining Br2 (g) + Cl₂ (g) = 2BrCl(g) AH for BrCl(g) is 14.6 kJ/mol. AS for BrCl(g) is 240.0 J/mol. Express your answer using three significant figures. View Available Hint(s) [5] ΑΣΦ K = 4.83 Submit ? Previous Answers Request Answer ?

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy

Section: Chapter Questions

Problem 102SCQ

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The equilibrium constant for a certain reaction increases by a factor of 6.67 when the temperature is increased from 300.0 K to 350.0 K. Calculate the standard change in enthalpy (H) for this reaction (assuming H is temperature-independent).
Using values of fH and S, calculate rG for each of the following reactions at 25 C. (a) 2 Na(s) + 2 H2O() 2 NaOH(aq) + H2(g) (b) 6 C(graphite) + 3 H2(g) C6H6() Which of these reactions is (are) predicted to be product-favored at equilibrium? Are the reactions enthalpy- or entropy-driven?
The value of G for the reaction 2C4H10(g)+13O2(g)8CO2(g)+10H2O(l) is 5490. kJ. Use this value and data from Appendix 4 to calculate the standard free energy of formation for C4H 10(g).
Consider the Haber process: N2(g)+3H2(g)2NH3(g);H=91.8kJ The density of ammonia at 25C and 1.00 atm is 0.696 g/L. The density of nitrogen, N2, is 1.145 g/L, and the molar heat capacity is 29.12 J/(mol C). (a) How much heat is evolved in the production of 1.00 L of ammonia at 25C and 1.00 atm? (b) What percentage of this heat is required to heat the nitrogen required for this reaction (0.500 L) from 25C to 400C, the temperature at which the Haber process is run?
When 7.11 g NH4NO3 is added to 100 mL water, the temperature of the calorimeter contents decreases from 22.1 C to 17.1 C. Assuming that the mixture has the same specific heat as water and a mass of 107 g, calculate the heat q. Is the dissolution of ammonium nitrate exothermic or endothermic?
Use the values of Hf in Appendix 4 to calculate H for the following reactions. (See Exercise 77 .) a. b. SiCl4(l)+2H2O(l)SiO2(s)+4HCl(aq) c. MgO(s)+H2O(l)Mg(OH)2(s)
Using data from Appendix 4, calculate G for the reaction NO(g)+O3(g)NO2(g)+O2(g) for these conditions: T=298KPNO=1.00106atm,PO3=2.00106atmPNO2=1.00107atm,PO2=1.00103atm
The combustion of methane can be represented as follows: a. Use the information given above to determine the value of H for the combustion of methane to form CO2(g) and 2H2O(l). b. What is Hf for an element in its standard state? Why is this? Use the figure above to support your answer. c. How does H for the reaction CO2(g) + 2H2O (1) CH4(g) + O2(g) compare to that of the combustion of methane? Why is this?
For the reaction TiCl2(s) + Cl2(g) TiCl4(), rG = 272.8 kj/mol-txn. Using this value and other data available in Appendix L, calculate the value of fG for TiCl2(s).
Using data from Appendix 4, calculate G for the reaction 2H2S(g)+SO2(g)3Srhombic(s)+2H2O(g) for the following conditions at 25C: PH2S=1.0104atmPSO2=1.0102atmPH2O=3.0102atm
Use the data in Appendix G to calculate the standard entropy change for H2(g) + CuO(s) H2O() + Cu(s)
Coal is used as a fuel in some electric-generating plants. Coal is a complex material, but for simplicity we may consider it to be a form of carbon. The energy that can be derived from a fuel is sometimes compared with the enthalpy of the combustion reaction: C(s)+O2(g)CO2(g) Calculate the standard enthalpy change for this reaction at 25C. Actually, only a fraction of the heat from this reaction is available to produce electric energy. In electric generating plants, this reaction is used to generate heat for a steam engine, which turns the generator. Basically the steam engine is a type of heat engine in which steam enters the engine at high temperature (Th), work is done, and the steam then exits at a lower temperature (Tl). The maximum fraction, f, of heat available to produce useful energy depends on the difference between these temperatures (expressed in kelvins), f = (Th Tl)/Th. What is the maximum heat energy available for useful work from the combustion of 1.00 mol of C(s) to CO2(g)? (Assume the value of H calculated at 25C for the heat obtained in the generator.) It is possible to consider more efficient ways to obtain useful energy from a fuel. For example, methane can be burned in a fuel cell to generate electricity directly. The maximum useful energy obtained in these cases is the maximum work, which equals the free-energy change. Calculate the standard free-energy change for the combustion of 1.00 mol of C(s) to CO2(g). Compare this value with the maximum obtained with the heat engine described here.