Kk.351 Use the data given here to calculate the values of AG at 25 °C for thereaction described by the equationA+B=CAG=677.1The spontaneous reaction isentropy-driven to the left.enthalpy-driven to the right.enthalpy-driven to the left.CompoundABсIf A His and ASin are both positive values, what drives the spontaneous reaction and in what direction at standard conditions?Question Source: McQuarneAG (kJ/mol)+387.7-621.3+402.0And Gallogtyde-GeneralkJ

The given reaction is : A + B ⇌ C In this question, it has been found to calculate the ∆G°f at…

Use the data given here to calculate the values of AG at 25 °C for the reaction described by the equation A+B=C AGE= 677.1 The spontaneous reaction is entropy-driven to the left. enthalpy-driven to the right. enthalpy-driven to the left. Compound A B C If A His and ASin are both positive values, what drives the spontaneous reaction and in what direction at standard conditions? Question Source McQuarne AG (kJ/mol) +387.7 -621.3 +402.0 And Gallogy 4e-Gener kJ

Use the data given here to calculate the values of AG at 25 °C for the reaction described by the equation A+B=C AGE= 677.1 The spontaneous reaction is entropy-driven to the left. enthalpy-driven to the right. enthalpy-driven to the left. Compound A B C If A His and ASin are both positive values, what drives the spontaneous reaction and in what direction at standard conditions? Question Source McQuarne AG (kJ/mol) +387.7 -621.3 +402.0 And Gallogy 4e-Gener kJ

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

Chapter20: The Representative Elements

Section: Chapter Questions

Problem 12Q: The major industrial use of hydrogen is in the production of ammonia by the Haber process:...

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Consider the reaction below at 25°C: 2MnO4(aq)+16H+(aq)+10Br(aq)2Mn2+(aq)+5Br2(l)+8H2O Use Table 17.1 to answer the following questions. Support your answers with calculations. (a) Is the reaction spontaneous at standard conditions? (b) Is the reaction spontaneous at a pH of 2.00 with all other ionic species at 0.100 M? (c) Is the reaction spontaneous at a pH of 5.00 with all other ionic species at 0.100 M? (d) At what pH is the reaction at equilibrium with all other ionic species at 0.100 M?
Determine the standard free energy change, Gf, for the formation of S2-(aq) given that the Gf for. Ag*(aq) and Ag2S(s) are 77.1 kJ/mole and 395 kJ/mole respectively, and the solubility product for Ag2S(s) is 81051.
Hydrogen has been suggested as the fuel of the future. One way to store it is to convert it to a compound that can be heated to release the hydrogen. One such compound is calcium hydride, Cal-12. This compound has a heat of formation of -186.2 kJ/mol and a standard entropy of 42.0 J/mol K. What is the minimum temperature to which calcium hydride would have to be heated to produce hydrogen at one atmosphere pressure?
The major industrial use of hydrogen is in the production of ammonia by the Haber process: 3H2(g)+N2(g)2NH3(g) a. Using data from Appendix 4, calculate H, S, and G for the Haber process reaction. b. Is the reaction spontaneous at standard conditions? c. At what temperatures is the reaction spontaneous at standard conditions? Assume H and S do not depend on temperature.
Given: P4(s)+5O2(g)P4O10(s)G298=2697.0kJ/mol 2H2(g)+O2(g)2H2O(g)G298=457.18kJ/mol 6H2O(g)+P4O10(s)4H3PO4(l)G298=428.66kJ/mol (a) Determine the standard free energy of formation, Gf, for phosphoric acid. (b) How does your calculated result compare to the value in Appendix G? Explain.
The free energy change for a reaction, G, is an extensive property. What is an extensive property? Surprisingly, one can calculate G from the cell potential. , for the reaction. This is surprising because : is an intensive property. How can the extensive property G be calculated from the intensive property ?
For the following reactions at constant pressure, predict if HE,HE,orH=E a. 2HF(g)H2(g)+F2(g) b. N2(g)+3H2(g)2NH3(g) c. 4NH3(g)+5O2(g)4NO(g)+6H2O(g)
Given the following standard free energies at 25°C for the following reactions: N2O5(g)2NO(g)+32O2(g)G=59.2kJNO(g)+12O2(g)NO2(g)G=35.6kJ Calculate G° at 25°C for the following reaction: 2NO2(g)+12O2(g)N2O5(g)
When magnesium metal is added to a beaker of HCl(aq), a gas is produced. Knowing that magnesium is oxidized and that hydrogen is reduced, write the balanced equation for the reaction. How many electrons are transferred in the balanced equation? What quantity of useful work can be obtained when Mg is added directly to the beaker of HCl? How can you harness this reaction to do useful work?
Using data from Appendix 4, calculate H, G, and K (at 298 K) for the production of ozone from oxygen: 3O2(g)2O3(g) At 30 km above the surface of the earth, the temperature is about 230. K and the partial pressure of oxygen is about 1.0 103 atm. Estimate the partial pressure of ozone in equilibrium with oxygen at 30 km above the earth's surface. Is it reasonable to assume that the equilibrium between oxygen and ozone is maintained under these conditions? Explain.
Calculate E°, G°, and K at 25°C for the reaction 3Mn2+(aq)+2MnO4(aq)+2H2O5MnO2(s)+4H+(aq)
Calculate E°, G°, and K at 25°C for the reaction 3MnO4(aq)+4H+(aq)+Cl2(g)2Mn2+(aq)+2ClO3(aq)+2H2O