Gg.73. Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy AH and reaction entropyAS.Note: if you have not been given enough information to decide a sign, select the "unknown" option.reactionMCobservationsThis reaction is spontaneous except below-48 °C but proceeds at a lower ratebelow 185. "CThis reaction is always spontaneous, butproceeds slower at temperatures abou-38. "CThis reaction in othermicAll is65 19conclusionsAN isAN ISA3 isXalkond E(picken)(pack one)[pick one) Bpik one) B5 ?

This problem is based on Thermodynamics. Here we have to use 2nd law of thermodynamics to find out…

Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy AH and reaction entropy AS. Note: if you have not been given enough information to decide a sign, select the "unknown" option. reaction M t observations This reaction is spontaneous except below -48 °C but proceeds at a lower rate below 185. "C This reaction is always spontaneous, but proceeds slower at temperatures abo -38. "C This reaction thermic conclusions All is AN is AN IS A3 is X kond) E (pick one) (pack one) [picke B pk one) B 5 ?

Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy AH and reaction entropy AS. Note: if you have not been given enough information to decide a sign, select the "unknown" option. reaction M t observations This reaction is spontaneous except below -48 °C but proceeds at a lower rate below 185. "C This reaction is always spontaneous, but proceeds slower at temperatures abo -38. "C This reaction thermic conclusions All is AN is AN IS A3 is X kond) E (pick one) (pack one) [picke B pk one) B 5 ?

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 10.51PAE: 10.51 The combustion of acetylene was used in welder's torches for many years because it produces a...

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What is the second law of thermodynamics? For any process, there are four possible sign combinations for Ssys and Ssurr. Which sign combination(s) always give a spontaneous process? Which sign combination(s) always give a non-spontaneous process? Which sign combination(s) may or may not give a spontaneous process?
Many plastic materials are organic polymers that contain carbon and hydrogen. The oxidation of these plastics in air to farm carbon dioxide and water is a spontaneous process; however, plastic materials tend to persist in the environment. Explain.
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.
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.
How does the second law of thermodynamics explain a spontaneous change in a system that becomes more ordered when that process is exothermic?
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).
Use data from Appendix D to calculate the standardentropy change at 25°C for the reaction CH3COOH(g)+NH3(g)CH3NH2(g)+CO2(g)+H2(g) Suppose that 1.00 mol each of solid acetamide, CH3CONH2(s), and water, H2O(l), react to give thesame products. Will the standard entropy change belarger or smaller than that calculated for the reactionin part (a)?
The enthalpy of vaporization of ethanol is 38.7 kJ/mol at its boiling point (78C). Determine Ssys, Ssurr, and Suniv when 1.00 mole of ethanol is vaporized at 78C and 1.00 atm.
Explain why absolute entropies can be measured.
The biological oxidation of ethanol, C2H5OH, is also a source of Gibbs free energy. (a) Does the oxidation of 1 g ethanol give more or lessenergy than the oxidation of 1 g glucose?(Hint:Writethe balanced equation for the production of carbondioxide and water from ethanol and oxygen, and useAppendix J.) (b) Comment on potential problems of replacing glucosewith ethanol in your diet.
In the thermodynamic definition of a spontaneous process, why is it important that the phrase “continuous intervention” be used rather than just “intervention?”
10.69 If a sample of air were separated into nitrogen and oxygen molecules (ignoring other gases present), what would be the sign of for this process? Explain your answer. The next four questions relate to the following paragraph [Frank L. Lambert, Journal of Chemical Education, 76(10), 1999, 1385]. "The movement of macro objects from one location to another by an external agent involves no change in the objects' physical (thermodynamic) entropy. The agent of movement undergoes a thermodynamic entropy increase in the process."