Please answer and show all work for parts A-C, thank you!! Thermodynamics table is shown below :) 10. For the reaction: CH4(g) + 2 O2(g)CO2(9) + 2 H20) AS = -154 J/Ka. At what temperature does this reaction begin to occur spontaneously?(Hint: use the Thermodynamic Tables)b. Is the reaction spontaneous at 50°C (show your work)?c. Calculate the Joules of work done on or by the system (state which) when1 mole of CH4 is combusted at 127°C (Hint: R = 8.31 J/mole K & look at theprevious reaction) THERMODYNAMIC TABLESAGfValuesΔΗValuesSubstancekJ/moleSubstancekJ/moleco (g)-137Co(g)-110Co2 (g)-395Co2 (g)-394Fe2 03 (s)-742CHa OH (1)-238H2 0 (1)-237CH4 (g)-75H2 0 (g)- 228C2 Ha (g)+52NH3 (g)-17Fe2 03 (s)-824NO (g)+87H2 0 (1)-286-242NO2 (g)+51H2 0 (g)Nac1(s)N2 04 (g)+98-413-470С2 Hs ОН (1)-390NAOH (aq)NH3 (g)HC2 H3 02 (1)-175-46NO (g)+90C2 Hs OH (1)- 485HC2 H3 02 (1)-278Atomization EnergiesBond EnergiesAtomkJ/mole atomBondkJ/mole bondC(g)715C-C(g)348c1(g)121c-c1(g)326H(g)218C=0 (g)724I(g)107C-0(g)1075Na(g)108C-H(g)4150(g)249H-H(g)436N(8)473H-C1(g)432I-I(g)150

Given reaction: Spontaneity of a reaction is determined by ∆G value. If the value is negative, the…

10. For the reaction: CH4(g) + 2 O2(g) C2(9) + 2 H20m AS = -154 J/K a. At what temperature does this reaction begin to occur spontaneously? (Hint: use the Thermodynamic Tables) b. Is the reaction spontaneous at 50°C (show your work)?

10. For the reaction: CH4(g) + 2 O2(g) C2(9) + 2 H20m AS = -154 J/K a. At what temperature does this reaction begin to occur spontaneously? (Hint: use the Thermodynamic Tables) b. Is the reaction spontaneous at 50°C (show your work)?

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 10.91PAE: The reaction shown below is involved in the refining of iron. (The table that follows provides all...

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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
The reaction shown below is involved in the refining of iron. (The table that follows provides all of the thermodynamic data you should need for this problem.) 2Fe2O3(s)+3C(s,graphite)4Fe(s)+3CO2(g) (a) Find H for the reaction. (b) S for the reaction above is 557.98 J/K. Find S° for Fe2O3(s). (c) Calculate G for the reaction at the standard temperature of 298 K. (There are two ways that you could do this.) (d) At what temperatures would this reaction be spontaneous? Compound Hf (kJ mol-1) S° (kJ mol-1) Gf (J mol-1 K-1) Fe2O3(s) -824.2 ? -742.2 C(s, graphite) 0 5.740 0 Fe(s) 0 27.3 0 CO2(g) -393.5 213.6 -394.4.83
Thermodynamics provides a way to interpret everyday occurrences. If you live in northern climates, one common experience is that during early winter, snow falls but then melts when it hits the ground. Both the formation and the melting happen spontaneously. How can thermodynamics explain both of these seemingly opposed events?
On the basis of your experience, predict which reactions are spontaneous: (a) PbO2(s)Pb(s)+O2(g)(b) N2(l)N2(g) at 25C (c) C6H12O6(s)C6H12O6(l) at 25C (d) Ca2+(aq)+CO32(aq)CaCO3(s)
Nickel metal reacts with carbon monoxide to form tetra-carbonyl nickel, Ni(CO)4: Ni(s)+4CO(g)Ni(CO)4(g) This reaction is exploited in the Mond process in order to separate pure nickel from other metals. The reaction above separates nickel from impurities by dissolving it into the gas phase. Conditions are then changed so that the reaction runs in the opposite direction to recover the purified metal. (a) Predict the sign of S for the reaction as written above. (b) Use tabulated thermodynamic data to calculate H, S , and G for the reaction. (c) Find the range of temperatures at which this reaction is spontaneous in the forward direction.
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.
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For the reaction C2H2(g)+4F2(g)2CF4(g)+H2(g) S is equal to 358 J/K. Use this value and data from Appendix 4 to calculate the value of S for CF4(g).
What happens to the entropy of the universe during a spontaneous process?
Define the standard enthalpy of formation. What are standard states for elements and for compounds? Using Hess's law, illustrate why the formula Hreaction=npHf(products)nfHf(reactants) works to calculate H for a reaction.
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Many biochemical reactions that occur in cells require relatively high concentrations of potassium ion (K+). The concentration of K + in muscle cells is about 0.l5 M. The concentration of K+ in blood plasma is about 0.0050 M. The high internal concentration in cells is maintained by pumping K+ from the plasma. How much work must be done to transport 1.0 mole of K+ from the blood to the inside of a muscle cell at 37C, normal body temperature? When 1.0 mole of K+ is transferred from blood to the cells, do any other ions have to be transported? Why or why not?