Enter your answer in the provided box. 0 Calculate AG for the following reaction at 25°C. You will have to look up the thermodynamic data. 2 C2H6g)+7 02(g)4 CO2(g)+6 H2O() kJ So (JIK mol) AG'f (kJ/mol) AHf (kJ/mol) Formula 229.5 -32.89 -84.7 C2H6 219.5 68.1 52.3 CНа CO(G) 197.9 -137.3 -110.5 CO2(9) 213.6 -394.4 -393.5 CO2(aq) 121.3 -386.2 -412.9 CO32- (aq) -53.1 -528.1 -676.3 HCO3 (aq) -587.1 94.98 -691.1 HаСОз(аg) 187.4 -699.7 -623.2 69.9 HаО() -285.8 -237.2 H2O(g) 188.7 -241.8 -228.6 197.9 COG) -137.3 -110.5 213.6 CO2(g) -394.4 -393.5 121.3 CO2(aq) O2(g) -386.2 -412.9 205.0 0 0 O3(aq) 16.3 -12.09 110.88 O3(g) 163.4 142.2 237.6 e ere to search F1 F2 F3 F4 F5 F6 F7 F8 F9 #

Enter your answer in the provided box. 0 Calculate AG for the following reaction at 25°C. You will have to look up the thermodynamic data. 2 C2H6g)+7 02(g)4 CO2(g)+6 H2O() kJ So (JIK mol) AG'f (kJ/mol) AHf (kJ/mol) Formula 229.5 -32.89 -84.7 C2H6 219.5 68.1 52.3 CНа CO(G) 197.9 -137.3 -110.5 CO2(9) 213.6 -394.4 -393.5 CO2(aq) 121.3 -386.2 -412.9 CO32- (aq) -53.1 -528.1 -676.3 HCO3 (aq) -587.1 94.98 -691.1 HаСОз(аg) 187.4 -699.7 -623.2 69.9 HаО() -285.8 -237.2 H2O(g) 188.7 -241.8 -228.6 197.9 COG) -137.3 -110.5 213.6 CO2(g) -394.4 -393.5 121.3 CO2(aq) O2(g) -386.2 -412.9 205.0 0 0 O3(aq) 16.3 -12.09 110.88 O3(g) 163.4 142.2 237.6 e ere to search F1 F2 F3 F4 F5 F6 F7 F8 F9 #

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 10.61PAE: Estimate the temperature range over which each of the following reactions is spontaneous. (a)...

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Similar questions

Estimate the temperature range over which each of the following reactions is spontaneous. (a) 2Al(s)+3Cl2(g)2AlCl3(s) (b) 2NOCl(g)2NO(g)+Cl2(g) (c) 4NO(g)+6H2O(g)4NH3(g)+5O2(g) (d) 2PH3(g)3H2(g)+2P(g)
When ammonium chloride is added to water and stirred, it dissolves spontaneously and the resulting solution feels cold. Without doing any calculations, deduce the signs of G, H, and S for this process, and justify your choices.
If you calculate a value for G for a reaction using the values of Gf in Appendix 4 and get a negative number, is it correct to say that the reaction is always spontaneous? Why or why not? Free energy changes also depend on concentration. For gases, how is G related to the pressure of the gas? What are standard pressures for gases and standard concentrations for solutes? How do you calculate G for a reaction at nonstandard conditions? The equation to determine G at nonstandard conditions has Q in it: What is Q? A reaction is spontaneous as long as G is negative; that is, reactions always proceed as long as the products have a lower free energy than the reactants. What is so special about equilibrium? Why dont reactions move away from equilibrium?
Liquid water at 25C is introduced into an evacuated, insulated vessel. Identify the signs of the following thermodynamic functions for the process that occurs: H, S, Twater, Ssurr,, Suniv.
Given the following information at 25C, calculate G at 25C for the reaction 2A(g)+B(g)3C(g) Substance Hf(kJ/mol) S(J/molK) A(g) 191 244 B(g) 70.8 300 C(g) 197 164 a 956 kJ b 956 kJ c 346 kJ d 346 kJ e 1.03 103 kJ
10.46 Discuss the effect of temperature change on the spontaneity of the following reactions at 1 atm. (a) Al2O3(s)+2Fe(s)2Al(s)+Fe2O3(s) H = 851.5kJ; S =38.5 J/K (b) N2H4(l)N2(g)+2H2(g) H =-50.6 kJ; S= 0.3315 kJ/K (c) SO3(g)SO2(g)+12O2(g) H = 98.9 kJ; S= 0.0939 kJ/K
Given that H f for HF(aq) is -320.1 kJ/mol and S for HF(aq) is 88.7 J/mol K, find Ka for HF at 25C.
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?
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
1. For the reaction 2 Hg(l) + O2(g) → 2 HgO(s), ∆rH° = 181.6 kJ/mol-rxn. What is the enthalpy change to decompose 1.00 mol of HgO(s) to O2(g) and Hg(l)? 3633 kJ −90.8 kJ 90.8 kJ 363.3 kJ
Using values of fH and S, calculate rG for each of the following reactions at 25 C. (a) 2 Na(s) + 2 H2O() 2 NaOH(aq) + H2(g) (b) 6 C(graphite) + 3 H2(g) C6H6() Which of these reactions is (are) predicted to be product-favored at equilibrium? Are the reactions enthalpy- or entropy-driven?
In a spontaneous process, S(universe) is (a) 0 (b) = 0 (c) 0

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