3127. The NBS Tables of Chemical Thermodynamic Properties in the Journal of Physical &Chemical Reference Data, Vol. 11, 1982, p 252, report the following data:ESpΔΗAGkJ/molkJ/molJ/K-molKI2(aq)55.19-51.57111.3A12(aq)22.6 m 16.46137.2PI,(aq)51.5)-51.4239.3a. Using the data in the table, use Hess's law to calculate thetriiodide formation.12 (99) +1 (99) → 15 (ad)AH AH (13) AH (In)noAS 239. 33/4 mol. 3py and entropy for the= -9.21 kml-51.5 kJ)-(-55.19k) - (22.6k)) AH na ons-18.91mol-137-2-18.91AH°=AS°=-9.2kmHopefully close if not tub. Compare your results to the values calculated above and try to account for any "differences.c. Use the free energy data in the table above to calculate the free energy for the reactionand use this value to calculate an equilibrium constant for the reaction at 25°C.(AG-RTInKq)productof tqmom u alibas my enemastaya sbibdini shiboiAG₁ =Keq1. Compare your value of the equilibrium constant to value in the question above and tryto account for any differences.ome of the Learning Objectives of this experiment are listed on the first page of thisperiment. Did you achieve the Learning Objectives? Explain your answer.

Step 1:Given thermodynamical data:To find: the enthalpy change and the entropy change for the…

Answered: 312 7. The NBS Tables of Chemical…

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Calculate (a) the (molar) Gibbs energy of mixing, (b) the(molar) entropy of mixing when the two major componentsof air (nitrogen and oxygen) are mixed to form air at 298 K.The mole fractions of N2 and 0 2 are 0.78 and 0.22. respectively. (c) Is the mixing spontaneous?
Gibbs free energy (G) is a measure of the spontaneity of a chemical reaction. It is the chemical potential for a reaction, and is minimized at equilibrium. It is defined as G=H-TS where H is enthalpy, T is temperature, and S is entropy. The chemical reaction that causes iron to corrode in air is given by 4Fe+302-2Fe2O3 TXn in which at 298 K, AH ASixn - 543.7 J/K. H = - 1684 kJ and Part A What is the standard Gibbs free energy for this reaction? Assume the commonly used standard reference temperature of 298 K. Express your answer as an integer and include the appropriate units. ► View Available Hint(s) AGrxn Submit μÅ Value t Ć Units ?
The reduction of iron(III) oxide (Fe2O3) to pure iron during the first step of steelmaking, 2 Fe2O3(s) 4 Fe(s) + 302 (g) is driven by the high-temperature combustion of coke, a purified form of coal: C(s) + 0,(g) → CO₂ (g) Suppose at the temperature of a blast furnace the Gibbs free energies of formation AG, of CO2 and Fe2O3 are -412. kJ/mol and -836. kJ/mol, respectively. Calculate the minimum mass of coke needed to produce 470. t of pure iron. (One metric ton, symbol t, equals 1000-kg.) Round your answer to 2 significant digits. kg x10
Calculate (a) the (molar) Gibbs energy of mixing, (b) the (molar) entropy of mixing when the two major components of air (nitrogen and oxygen) are mixed to form air at 298 K. The mole fractions of N2 and O2 are 0.78 and 0.22, respectively. (c) Is the mixing spontaneous?
The reduction of iron(III) oxide (Fe2O3) to pure iron during the first step of steelmaking, 2 Fe2O3(s) 4Fe(s) + 302 (g) is driven by the high-temperature combustion of coke, a purified form of coal: C(s) + O2(g) - - CO2(g) Suppose at the temperature of a blast furnace the Gibbs free energies of formation AG of CO2 and Fe2O3 are -428. kJ/mol and -821. kJ/mol, respectively. Calculate the minimum mass of coke needed to produce 680. t of pure iron. (One metric ton, symbol t, equals 1000 kg.) Round your answer to 2 significant digits.
Calculate the standard Gibbs reaction energy for the reaction at 298 K, 2CH3CHO(g) + O2(g) - > 2CH3 COOH(I) Given the following data, Sm\deg (CH3CHO(g )) = 250.30 J K-1 mol-1 Sm\deg (O2(g)) = 205.10 JK -1 mol-1 Sm\deg (CH3COOH(l))=159.80~K-1~mol-1\backslash Delta fHm\deg (CH3CHO(g))=-166.20~kJ~mol-1\backslash Delta fHm\deg (O2(g)) = 0.00 kJ mol-1 \Delta fHm\ deg (CH3COOH(I)) = 484.50 kJ mol-1
The temperature dependence of the heat capacity of non-metallic solids is found to follow the Debye T3 -law at very low temperatures, with Cp,m = aT3. (a) Derive an expression for the change in molar entropy on heating for such a solid. (b) For solid nitrogen, a= 6.15 x 10-3 J K-4 mol-1. What is the molar entropy of solid nitrogen at 5 K?
Without carrying out an explicit calculation, explain there lative values of the standard molar entropies (at 298 K) of the following substances: (a) Ne(g) (146 J K-1 mol-1) compared with Xe(g) (170 J K-1 mol-1), (b) H2O(g) (189 J K-1 mol-1) compared with D2O(g) (198 J K-1 mol-1), (c) C(diamond) (2.4 J K-1 mol-1) compared with C(g raphite) (5.7 J K-1 mol-1).
Based on the following thermodynamic data, calculate the boiling point of ethanol in degrees Celsius. AH; (kJ mol-1) (J K-1 S° Substance mol-1) C2 H;OH(1) - 277.7 160.6 C2H;OH(9) – 235.1 282.6 Express the boiling point numerically in degrees Celsius using two significant figures.
(a) An ideal gas of mass 4.5 g and molar mass of 17 g.mole-1 occupies 12.7 L at 310 K. Answer the following questions based on the conditions presented. (i) Calculate the work done under a constant external pressure of 30 kPa until the volume of gas has increased by 3.3 L. (ii) Calculate the work done in an isothermal and reversible expansion process resulting in a final volume of 16L. (iii) If the gas has a molar heat capacity of 30.8 J.mol-1.K-1 and is subjected to a constant volume process until it reaches a temperature of 350K, calculate the heat transfer in kJ.mol-1 of the gas. (b) Calculate the standard enthalpy of formation of N2O5 (g) from N2 (g) and O2 (g), in kJ. mol-1, from the following data: 2NO(g) + O2(g) ® 2NO2(g) DH = -114.1 kJ 4NO2(g) + O2(g) ® 2N2O5(g) DH = -110.2 kJ N2(g) + O2(g) ® 2NO(g) DH = +180.5 kJ
Use the fundamental equation of therodynamics here tocalculate the change Gibbs energy when 3.1 mmol N_2(g) occupying 3.0L at 350 K expandsisothermally to 15 L.
Calculate (a) the standard reaction entropy and (b) the change in entropyof the surroundings (at 298 K) of the reaction N2(g) + 3 H2(g) → 2 NH3(g). (c) Hence calculate the standard Gibbs energy of the reaction.

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