Given the dissociation of methane to graphite (C) and hydrogen gas. For the methane at 298K,Given the following data:kJ= -74.85-mol= -80.67mol · KA,GE.graphite= A,Gån= 0%3DSolve the following:a. Calculate the equilibrium constant (K) of the dissociation of methane at 298K with theappropriate units.b. Assuming that enthalpy is independent of temperature, Calculate the equilibrium constant (K) ofmethane dissociation at 1000 K.C.Calculate the ratio between the amounts of methane and hydrogen gas at 298 K and 0.2 bar.

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Answered: Given the dissociation of methane to…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 108CP

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One of the reactions that destroys ozone in the upper atmosphere is NO(g)+O3(g)NO2(g)+O2(g) Using data from Appendix 4, calculate G and K (at 298 K) for this reaction.
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.
The Ostwald process for the commercial production of nitric acid involves three steps: 4NH3(g)+5O2(g)825CPt4NO(g)+6H2O(g)2NO(g)+O2(g)2NO2(g)3NO2(g)+H2O(l)2HNO3(l)+NO(g) a. Calculate H, S,G and K (at 298 K) for each of the three steps in the Ostwald process (see Appendix 4). b. Calculate the equilibrium constant for the first step at 825C, assuming H and S do not depend on temperature. c. Is there a thermodynamic reason for the high temperature in the first step, assuming standard conditions?
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?
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.
Given the following data for sodium Na(s): S =51.2 J/mol K Na(g): S =153.6 J/mol K H f =108.7 kJ/mol K estimate the temperature at which sodium sublimes at 1 atm. Na(s)Na(g)
Hydrogen sulfide can be removed from natural gas by the reaction 2H2S(g)+SO2(g)3S(s)+2H2O(g) Calculate G and K (at 298 K) for this reaction. Would this reaction be favored at a high or low temperature?
An important source of copper is from the copper ore, chalcocite, a form of copper(I) sulfide. When heated, the Cu2S decomposes to form copper and sulfur described by the following equation: Cu2S(s)Cu(s)+S(s) (a) Determine G298 for the decomposition of Cu2S(s). (b) The reaction of sulfur with oxygen yields sulfur dioxide as the only product. Write an equation that describes this reaction, and determine G298 for the process. (c) The production of copper from chalcocite is performed by roasting the Cu2S in air to produce the Cu. By combining the equations from Parts (a) and (b), write the equation that describes the roasting of the chalcocite, and explain why coupling these reactions together makes for a more efficient process for the production of the copper.
Thermite reactions have been used for welding metal parts such as railway rails and in metal refining. One such thermite reaction is Fe2O3(s)+2Al(s)Al2O3(s)+2Fe(s). Is the reaction spontaneous at room temperature under standard conditions? During the reaction, the surroundings absorb 851.8 kJ/mol of heat.
Table 16-1 shows the possible arrangements of four molecules in a two-bulbed flask. What are the possible arrangements if there is one molecule in this two-bulbed flask or two molecules or three molecules? For each, what arrangement is most likely?

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