Consider the following reaction occurring at 25C Nitrogen monoxide gas reacts with hydrogen gas to form ammonia gas and water vapor (steam) Use Appendix 2 to obtain-the data required to find the following: (fill in the blanks with a numerical response only. Do not write the units in your answer.) 1. Enthalpy of reaction: AH kJ/mol %3D 2. Entropy of system: AS J/mol 3. Entropy of surroundings: AS J/mol %3D surr 4. Entropy of universe: AS univ J/mol

Consider the following reaction occurring at 25C Nitrogen monoxide gas reacts with hydrogen gas to form ammonia gas and water vapor (steam) Use Appendix 2 to obtain-the data required to find the following: (fill in the blanks with a numerical response only. Do not write the units in your answer.) 1. Enthalpy of reaction: AH kJ/mol %3D 2. Entropy of system: AS J/mol 3. Entropy of surroundings: AS J/mol %3D surr 4. Entropy of universe: AS univ J/mol

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter10: Entropy And The Second Law Of Thermodynamics

Section: Chapter Questions

Problem 10.88PAE: Nickel metal reacts with carbon monoxide to form tetra-carbonyl nickel, Ni(CO)4:...

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The reaction CO2(g)+H2(g)CO(g)+H2O(g) is not spontaneous at room temperature but becomes spontaneous at a much higher temperature. What can you conclude from this about the signs of H and S , assuming that the enthalpy and entropy changes are not greatly affected by the temperature change? Explain your reasoning.
10.51 The combustion of acetylene was used in welder's torches for many years because it produces a very hot flame: C2H2(g)+52O2(g)2CO2(g)+H2O(g) H= -1255.5 kJ (a) Use data in Appendix E to calculate S for this reaction, (b) Calculate G and show that the reaction is spontaneous at 25°C. (c) Ls there any temperature range in which this reaction is not spontaneous? (d) Do you think you could use Equation 10.4 to calculate such a temperature range reliably? Explain your answer.
Limestone is predominantly CaCO3, which can undergo the reaction CaCO3(s)CaO(s)+CO2(g). We know from experience that this reaction is not spontaneous, yet S for the reaction is positive. How can the second law of thermodynamics explain that this reaction is not spontaneous?
A 2.50-mol sample of gas is compressed isothermally from 20.0 L to 5.00 L under a constant external pressure of 10.0 atm. Calculate w, q, U, and H for the process.
Acetic acid in vinegar results from the bacterial oxidation of ethanol. C2H5OH(l)+O2(g)CH3COOH(l)+H2O(l) What is S for this reaction? Use standard entropy values. (See Appendix C for data.)
Methane can be produced from CO and H2.The process might be done in two steps, as shown below, with each step carried out in a separate reaction vessel within the production plant. Reaction 1 CO(g)+2H2(g)CH3OH(l) S = -532 J/K Reaction 2 CH3OH(l)CH4(g)+12O2(g) S= +162 J/K NOTE: You should be able to work this problem without using any additional tabulated data. (a) Calculate H for reaction 1. (b) Calculate Gf for CO(g). (c) Calculate S° for O2(g). (d) At what temperatures is reaction 1 spontaneous? (e) Suggest a reason why these two steps would need to be carried out separately. Substance Hf (kJ mol-1) Gf (kJ mol-1) S (J mol-1 K-1) CO(s) -110.5 197.674 CH3OH( l ) -238.7 -166.4 126.8 CH4(g) -74.8 186.2
Explain why the statement No process is 100 efficient is not the best statement of the second law of thermodynamics.
The standard molar entropy of iodine vapor, I2(g), is 260.7 J Kl mol-1 and the standard molar enthalpy of formation is 62.4 kJ/mol. a) Calculate the entropy change for vaporization of 1 mol of solid iodine (use data from Table 16.1 or Appendix J). b) Calculate the enthalpy change for sublimation of iodine. c) Assuming that rSdoes not change with temperature, estimate the temperature at which iodine would sublime (change directly from solid to gas).
Recall that incomplete combustion of fossil fuels occurs when too little oxygen is present and results in the production of carbon monoxide rather than carbon dioxide. Water is the other product in each case. (a) Write balanced chemical equations for the complete and incomplete combustion of propane. (b) Using these equations, predict which will have the larger change in entropy. (c) Use tabulated thermodynamic data to calculate G for each reaction. (d) Based on these results, predict the sign and value of G for the combustion of carbon monoxide to form carbon dioxide.
Explain why absolute entropies can be measured.
Using tabulated thermodynamic data, calculate G for these reactions. (a) Mg3N2(s)+6H2O(l)2NH3(g)+3Mg(OH)2(s) (b) 4CH3NH2(g)+9O2(g)4CO2(g)+10H2O(l)+2N2(g) (c) Fe3O(s)+4CO(g)3Fe(s)+4CO2(g) (d) P4O10(s)+6H2O(l)4H3PO4(aq)
For the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then use those values to answer the following questions. (a) Is this reaction spontaneous at 25°C? Explain your answer. (b) If the reaction is not spontaneous at 25°C, will it become spontaneous at higher temperatures or lower temperatures? (c) To show that your prediction is accurate, choose a temperature that corresponds to your prediction in part (b) and calculate G . (Assume that both enthalpy and entropy are independent of temperature.)