5 Ammonia is converted into nitrogen() oxide in industry by the Ostwald process: 4NH:(9) + 50:(9) = 4NO(g) + 6H;O(g) AH = -905.2 kJ mol The reaction is normally carried out at a pressure of around 500 kPa. a Use ideas about equilibrium to explain why pressures above 500 kPa are not used in industry for the Ostwald process. - -- b 200 moles of ammonia and 600 moles of oxygen are placed ina reactor at 600 K and a pressure of 500 kPa. At equilibrium, 100 moles of nitrogen(11) oxide have formed. Calculate a value for the equilibrium constant, K, including units, for this equilibrium. Give your answer to an appropriate number of significant figures.

5 Ammonia is converted into nitrogen() oxide in industry by the Ostwald process: 4NH:(9) + 50:(9) = 4NO(g) + 6H;O(g) AH = -905.2 kJ mol The reaction is normally carried out at a pressure of around 500 kPa. a Use ideas about equilibrium to explain why pressures above 500 kPa are not used in industry for the Ostwald process. - -- b 200 moles of ammonia and 600 moles of oxygen are placed ina reactor at 600 K and a pressure of 500 kPa. At equilibrium, 100 moles of nitrogen(11) oxide have formed. Calculate a value for the equilibrium constant, K, including units, for this equilibrium. Give your answer to an appropriate number of significant figures.

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

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 118CP: Consider the reaction H2(g)+Br2(g)2HBr(g) where H = 103.8 kJ/mol. In a particular experiment, equal...

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Consider the reaction 2SO2(g)+O2(g)2SO3(g) (a) Calculate G at 25C. (b) If the partial pressures of SO2 and SO3 are kept at 0.400 atm, what partial pressure should O2 have so that the reaction just becomes nonspontaneous (i.e., G=+1.0 k J)?
If wet silver carbonate is dried in a stream of hot air. the air must have a certain concentration level of carbon dioxide to prevent silver carbonate from decomposing by the reaction Ag2CO3(s)Ag2O(s)+CO2(g) H for this reaction is 79.14 kJ/mol in the temperature range of 25 to 125C. Given that the partial pressure of carbon dioxide in equilibrium with pure solid silver carbonate is 6.23 103 torr at 25C, calculate the partial pressure of CO2 necessary to prevent decomposition ofAg2CO3 at 110C. (Hint: Manipulate the equation in Exercise 79.)
Monochloroethane (C2H5Cl) can be produced by the direct reaction of ethane gas (C2H6) with chlorine gas or by the reaction of ethylene gas (C2H4) with hydrogen chloride gas. The second reaction gives almost a 100% yield of pure C2H5Cl at a rapid rate without catalysis. The first method requires light as an energy source or the reaction would not occur. Yet G for the first reaction is considerably more negative than G for the second reaction. Explain how this can be so.
Consider the reaction H2(g)+Br2(g)2HBr(g) where H = 103.8 kJ/mol. In a particular experiment, equal moles of H2(g) at 1.00 atm and Br2(g) at 1.00 atm were mixed in a 1.00-L flask at 25C and allowed to reach equilibrium. Then the molecules of H2 at equilibrium were counted using a very sensitive technique, and 1.10 1013 molecules were found. For this reaction, calculate the values of K, G, and S.
Silver carbonate, Ag2CO3, is a light yellow compound that decomposes when heated to give silver oxide and carbon dioxide: Ag2CO3(s)Ag2O(s)+CO2(g) A researcher measured the partial pressure of carbon dioxide over a sample of silver carbonate at 220C and found that it was 1.37 atm. Calculate the partial pressure of carbon dioxide at 25C. The standard enthalpies of formation of silver carbonate and silver oxide at 25C are 505.9 kJ/mol and 31.05 kJ/mol, respectively. Make any reasonable assumptions in your calculations. State the assumptions that you make, and note why you think they are reasonable.
Adenosine triphosphate, ATP, is used as a free-energy source by biological cells. (See the essay on page 624.) ATP hydrolyzes in the presence of enzymes to give ADP: ATP(aq)+H2O(l)ADP(aq)+H2PO4(aq);G=30.5kJ/molat25C Consider a hypothetical biochemical reaction of molecule A to give molecule B: A(aq)B(aq);G=+15.0kJ/molat25C Calculate the ratio [B]/[A] at 25C at equilibrium. Now consider this reaction coupled to the reaction for the hydrolysis of ATP: A(aq)+ATP(aq)+H2O(l)B(aq)+ADP(aq)+H2PO4(aq) If a cell maintains a high ratio of ATP to ADP and H2PO4 by continuously making ATP, the conversion of A to B can be made highly spontaneous. A characteristic value of this ratio is [ATP][ADP][H2PO4]=500 Calculate the ratio [B][A] in this case and compare it with the uncoupled reaction. Compared with the uncoupled reaction, how much larger is this ratio when coupled to the hydrolysis of ATP?
Natural gas, which is mostly methane, CH4, is a resource that the United States has in abundance. In principle, ethane can be obtained from methane by the reaction 2CH4(g)C2H6(g)+H2(g) (a) Calculate G° at 25°C for the reaction. Comment on the feasibility of this reaction at 25°C. (b) Couple the reaction above with the formation of steam from the elements: H2(g)+12O2(g)H2O(g)G=228.6kJ What is the equation for the overall reaction? Comment on the feasibility of the overall reaction.
A process that is reactant-favored at equilibrium can never be spontaneous. This statement is (a) true (b) false
Use data given in Tables 6.2 and 18.1 to obtain the value of Kp at 1000C for the reaction C(graphite)+CO2(g)2CO(g) Carbon monoxide is known to form during combustion of carbon at high temperatures. Do the data agree with this? Explain.
Benzene can be prepared from acetylene. 3C2H2(g)C6H6(g). Determine the equilibrium constant at 25 C and at 850 C. Is the reaction spontaneous at either of these temperatures? Why is all acetylene not found as benzene?
What types of experiments can be carried out to determine whether a reaction is spontaneous? Does spontaneity have any relationship to the final equilibrium position of a reaction? Explain.
A friend tells you, Free energy G and pressure P are related by the equation G = G + RT ln(P). Also, G is related to the equilibrium constant K in that when Gproducts = Greactantsthe system is at equilibrium. Therefore, it must be true that a system is at equilibrium when all the pressures are equal. Do you agree with this friend? Explain.

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