Use the standard free energy data below to determine the free energy change for the following reaction, run under standard conditions and at 298.15 KN2F4(g) + 6HF(g)2NH3(g) +5F2(g)NH3(9) F2(g) N2F4(g) HF(g)Substance:AG (kJ/mol): -16.4 0 79.9-275.4Oa.-211.9 kJ/molO b. 179.1 kJ/molOc.-179.1 kJ/molOd. 1539.7 kJ/molOe.-1539.7 kJ/mol

The balanced reaction: 2NH3(g) + 5 F2(g) → N2F4(g) + 6HF(g) ∆H˚rxn = Σnp∆H˚f(products) -…

Answered: Use the standard free energy data below…

Chemistry

10th Edition

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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4HCl(g) + O2(g)2H2O(g) + 2Cl2(g)Using the standard thermodynamic data in the tables linked above, calculate G for this reaction at 298.15K if the pressure of each gas is 11.80 mm Hg.
For the reaction Fe,O3(s) + 3H2(g)–2Fe(s) + 3H,O(g) AH° = 98.8 kJ and AS° = 142.5 J/K %3D The equilibrium constant for this reaction at 345.0 K is Assume that AH° and AS° are independent of temperature.
Use the standard molar entropies in the hint to calculate the AS value for the following reaction. 2H₂S(g) +30₂(g) → 2H₂O(g) +2SO₂(g) J/K
Consider the reaction: 2H₂(g) + O₂(g) → 2H₂O(g) Using standard thermodynamic data at 298 K, calculate the free energy change when 2.08 moles of H₂ (g) react at standard conditions. Substance AG (kJ/mol) H₂O(g) -228.6 H₂(g) 0.0 O₂(g) 0.0 AGO =-475.488 rxn kJ
11) Why can endothermic reactions be spontaneous?
Given the values of AH, ASn, and T, determine ASuniy and predict whether or not each reaction is spontaneous. (Assume that all reactants and products are in their standard states.) a. AH = -95 kJ; AS;n = -157 J/K; T = 298 K b. AH = -95 kJ; AS"n = -157 J/K; T = 855 K Calculate the Gibbs free energy for the above sets (a) and (b)
Consider the reaction: 2BrF3(g) → Br2(g) + 3F2 (g) Using standard thermodynamic data at 298 K, calculate the free energy change when 2.40 moles of BrF3 (g) react at standard conditions. Substance AG (kJ/mol) BrF3 (9) Br₂ (9) F₂ (g) AGTER Submit Answer kj -229.4 3.1 0.0 Retry Entire Group 9 more group attempts remaining
Please provide full
Use the data to calculate the standard entropy change for the following reaction: 5. S°[Mt(s)] 43.2 J/K mol Mt(s) + ½ O2(g) → MtO(s) S°[O2(g)] = 305.1 J/K-mol S°[MtO(s)] 62.6 J/K mol a) -133.2 J/K b) -285.7 J/K c) 285.7 J/K d) 133.2 J/K
Use the standard free energy data to determine the free energy change for the following reactions, which is run under standard state conditions and 25 °C. Identify it as spontaneous or nonspontaneous at this condition. CASO2H;0(s) → CaSOds) + 2H¿O(g) AG (CaSO s)= -1322.0 kJ'mol 40 (HOg)--228.59 kl'mol AG(CasO-H;0,s) =.]797,45 kJ/mol 0 18.3kJ/mol, nonspontaneous 0-18.3kJ/mol, spontaneous 0 156kl/mol, nonspontaneous
The reaction of methane with water to form carbon dioxide and hydrogen is nonspontaneous at 298 K. At what temperature will this system make the transition from nonspontaneous to spontaneous? The following data are valid at 298 K: CH4(g) + 2H2O(g) CO2(g) + 4H2(g) Substance: CH4(g) H2O(g) •CO2(g) AH°; (kJ/mol): -74.87 -241.8 -393.5 AG°F (kJ/mol): -50.81 -228.6 -394.4. S°(J/K • mol): 186.1 188.8 213.7 130.7 O 1047 K O 658 K O 1229 K O 683 K O 955 K

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