The reaction8 CO2(g) + 10 H20(g)2 C4H10(g) + 13 O2(3)has AG° = -5407 kJ. Determine the value of AG°¢ for C4H10(g).Standard Free Energies of Formation of Typical Substancesat 298.15 KTABLE 18.2SubstanceAG(kJ mol-1)SubstanceAG?(kJ mol-1)SubstanceAG?(kJ mol-)CaO(s)-604.2K,SO,6)-1316.4Ag()AgCI()-109.7Ca(OH),()-896.76N(g)-16.7NH3(g)NH.CI()Al()0.00CaSO(6)-1320.3-1435.2- 203.9CaSO H,O()CaSO,2H,0()Al,O,6)-1576.4-1795.7NO(g)+ 86.69C() (graphite)CO()NO,(g)+51.84-137.3-394.4Fe(s)N,0(g)+103.6-50.79Fe,O,(6)-741.0+98.28-58.6H,(g)Na(s)CH,C(CH,OH(/)CO(NH)2()CO(NH),(aq)-166.2H,O(g)-228.6Na,CO,()-1048-197.2H,O()-237.2NaHCO,()-851.9NaCl(s)-384.0HCI(gHNO,(/)-203.8-95.27CH(-79.91NaOH(s)-382+209CH.(+68.12H,SO,(1)-689.9Na,SO()-1266.8-32.9HC,H,0,()-392.5CH,OH()-174.8Hg(/)PbO()-189.3+17.3Hg(g)+31.8S()SO,(g)So,()Ca(s)K()-300.4C2CO,()KCI()-408.3-370.4-1128.8CaCh6)-750.2kJeTextbook and Media

Answered: Image /qna-images/answer/44c88612-a6cc-4975-abff-02766970f081.jpg

The reaction 8 CO2(g) + 10 H20(g) 2 C4H10(g) + 13 O2(3) has AG° = -5407 kJ. Determine the value of AG°f for C4H10(g). Standard Free Energies of Formation of Typical Substances at 298.15 K TABLE 18.2 Substance AG (kJ mol-1) Substance AG? (kJ mol-1) Substance AG? (kJ mol-1) Ag() CaO(s) -604.2 K,SO,6) -13164 -109.7 Ca(OH),() -896.76 N(g) -16.7 NH,(g) NH.CI() Al() 0.00 CaSO,6) -1320.3 -1435.2 - 203.9 CaSO H,O() CaSO,2H,0() Al,O,6) -1576.4 + 86.69 NO(g) NO,() N,0(g) C) (graphite) -1795.7 +51.84 CO() -137.3 -394.4 Fe(s) +103.6 CH(g -50.79 Fe,O,(6) -741.0 +98.28 Na(s) H(g) H,0(g) -58.6 CH,C( CH,OH(/) CO(NH)2() CO(NH),(aq) -166.2 -228.6 Na,CO,() -1048 -197.2 H,O() -237.2 NaHCO,() -851.9 NaCl(s) -384.0 HCI(g HNO,() -203.8 -95.27 CH( -79.91 NaOH() -382 +209 +68.12 H,SO,() -689.9 Na,SO,() -1266.8 -32.9 HC,H,0,(1) -392.5 CH,OH(/) Hg(/) PbO() -189.3 -174.8 +17.3 Hg(g) +31.8 Ca(s) K() SO,(g) -300.4 C2CO,() KCI() -408.3 SO,() -370.4 -1128.8 CaC6) -750.2 kJ eTextbook and Media

The reaction 8 CO2(g) + 10 H20(g) 2 C4H10(g) + 13 O2(3) has AG° = -5407 kJ. Determine the value of AG°f for C4H10(g). Standard Free Energies of Formation of Typical Substances at 298.15 K TABLE 18.2 Substance AG (kJ mol-1) Substance AG? (kJ mol-1) Substance AG? (kJ mol-1) Ag() CaO(s) -604.2 K,SO,6) -13164 -109.7 Ca(OH),() -896.76 N(g) -16.7 NH,(g) NH.CI() Al() 0.00 CaSO,6) -1320.3 -1435.2 - 203.9 CaSO H,O() CaSO,2H,0() Al,O,6) -1576.4 + 86.69 NO(g) NO,() N,0(g) C) (graphite) -1795.7 +51.84 CO() -137.3 -394.4 Fe(s) +103.6 CH(g -50.79 Fe,O,(6) -741.0 +98.28 Na(s) H(g) H,0(g) -58.6 CH,C( CH,OH(/) CO(NH)2() CO(NH),(aq) -166.2 -228.6 Na,CO,() -1048 -197.2 H,O() -237.2 NaHCO,() -851.9 NaCl(s) -384.0 HCI(g HNO,() -203.8 -95.27 CH( -79.91 NaOH() -382 +209 +68.12 H,SO,() -689.9 Na,SO,() -1266.8 -32.9 HC,H,0,(1) -392.5 CH,OH(/) Hg(/) PbO() -189.3 -174.8 +17.3 Hg(g) +31.8 Ca(s) K() SO,(g) -300.4 C2CO,() KCI() -408.3 SO,() -370.4 -1128.8 CaC6) -750.2 kJ eTextbook and Media

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

For the reaction 4HCI(g) + O2(g)- →2H2O(g) + 2C1½(g) AH° = -114.4 kJ and AS° = -128.9 J/K The standard free energy change for the reaction of 1.62 moles of HCl(g) at 332 K, 1 atm would be kJ. This reaction is (reactant, product) favored under standard conditions at 332 K. Assume that AH° and AS° are independent of temperature.
a) b)
Consider the reaction 2 SO2 (g) + O2 (g) <-> 2 SO3 (g) at 298 K. What is Go for this reaction? What is G when the partial pressures are P of SO2 = 1.0 x 10^-4 atm, P of O2 = 0.20 atm, and P of SO3 = 0.10 atm? Is the reaction spontaneous under the conditions in (b)? Why or why not?
12) Calculate AG°pm for the following reaction at 25.0 °C. Is the reaction spontaneous? 3 H2 (g) + N2 (g) 2 NH3 (g) Substance AH°t (kJ/mol) AG°r (kJ/mol) S (J/mol K) H2 (g) 130.7 N2 (g) 0. 191.6 NH3 (g) -45.9 -16.4 192.8
Consider the reaction - 4NO28) + 02(g) 2N205(g) at 25°C for which the following data are relevant: AHf S° N205 13.30 kJ/mol 355.7 J/K.mol NO2 33.15 kJ/mol 239.9 J/K.mol 02 O k/mol 204.8 J/K-mol Calculate AG° for the reaction at 25°C. 1.35 x 105 k 94.7 k 29.0 kj 135 k
2H2O(g) ----> 2H2(g) + O2(g) The reaction above is only spontaneous at temperatures above 2000K. Is the reaction endothermic (+ΔH) or exothermic (-ΔH)?
In a biochemical reaction, A + B ® C with DG= 30 kJ/mol. Which of the following reactions, if any, might be effectively coupled to this reaction so that it becomes more spontaneous? I. C + D -> B + E Delta G = –40 kJ/mol II. C + D -> B + E Delta G = +40 kJ/mol
The free energy change is related to the enthalpy change and the entropy change: ΔG = ΔH – T ΔS. What is ΔS for reaction 3? Question 8 options: –200 J mol–1 K–1 400 J mol–1 K–1 200 J mol–1 K–1
For each equation answer the following questions: i) What does each variable stand for? ii) What are the units of each variable? iii) Each is a way to calculate a change in entropy, but for what type of situation is each equation used? a) ΔS = qrev/T b) ΔS = nR ln(V2/V1) c) ΔS = C ln (T2/T1) d) S = k ln W e) ΔS = ΔHvap/Tb f) ΔS = ΔHfus/Tf
Table 2. Gibbs Free Energies of formation (kJ), ∆G°f, for Ions in 1M Solution and Ionic Solids Cations Cl--131.228 I--51.57 NO3--108.74 SO4-2-744.53 Ag+77.107 AgCl -109.789 -66.19 -33.41 -618.41 Calculated values of ∆G°rxn and the ∆Grxn of each box, Predicted results (ppt or no ppt).Observations (Rxn or No Rxn). S or support and R for Refute Cations Cl- I- NO3- SO4-2 Ag+ Ba+2
Determine whether the following reactions are spontaneous or non-spontaneous. a) N2 (g) + 3 H2 (g) ⟶ 2 NH3 (g), ΔG = -32,960 J b) 2 NH3 (g) ⟶ N2 (g) + 3 H2 (g), ΔG = 32,960 J HINT: The change in free energy (ΔG) for reaction is equal to the difference in free energy between the products (Gproducts) and the reactants (Greactants): ΔG = (Gproducts) - (Greactants) In spontaneous reactions, the free energy of the products (Gproducts) of a reaction is less than the free energy of the reactants (Greactants). When this is the case, will the change in free energy (ΔG) will have a negative value or a positive value?
A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 63.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.