A student determines the value of the equilibrium constant to be 1.08×10° for the following reaction.3Fe2O3(s) + H2(g)2Fe;O4(s) + H,0(g)Based on this value of KeqiAG° for this reaction is expected to be (greater, less)than zero.Calculate the free energy change for the reaction of 1.50 moles of Fe,O3(s) at standard conditions at 298K.AG°,rxnkJ

Equilibrium Constant, Keq = 1.08 × 106 Temperature, T = 298 K Gas constant, R = 8.314 J K-1 mol-1…

A student determines the value of the equilibrium constant to be 1.08×106 for the following reaction. 3Fe,O3(s) + H2(g)- →2F¢;O4(s) + H2O(g) Based on this value of Keqi than zero. AG° for this reaction is expected to be (greater, less) Calculate the free energy change for the reaction of 1.50 moles of Fe,03(s) at standard conditions at 298K. AG° rxn kJ

A student determines the value of the equilibrium constant to be 1.08×106 for the following reaction. 3Fe,O3(s) + H2(g)- →2F¢;O4(s) + H2O(g) Based on this value of Keqi than zero. AG° for this reaction is expected to be (greater, less) Calculate the free energy change for the reaction of 1.50 moles of Fe,03(s) at standard conditions at 298K. AG° rxn kJ

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...

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A student determines the value of the equilibrium constant to be 5.14×1091 for the following reaction.H2CO(g) + O2(g)CO2(g) + H2O(l)Based on this value of Keq:G° for this reaction is expected to be (greater, less) fill in the blank 1 than zero.Calculate the free energy change for the reaction of 2.29 moles of H2CO(g) at standard conditions at 298K. G°rxn = ____________ kJ
A student determines the value of the equilibrium constant to be 8.14x10-37 for the following reaction. H,S(g) + 2H,0(1)–→3H,(g) + SO>(g) Based on this value of Keg AG° for this reaction is expected to be (greater, less) than zero. Calculate the free energy change for the reaction of 2.03 moles of H,S(g) at standard conditions at 298K. AG°rxn kJ Ixn
The neutralization of a strong acid and strong base has an enthalpy change, ∆H°, = -55.9 kJ/mol. The net ionic equation for this reaction is H⁺(aq) + OH⁻(aq) ⇌ H₂O(l) which is the reverse of the autoionization of water, and therefore its equilibrium constant, K = 1.0 × 10¹⁴ at 25°C. You can determine ∆S° from this data. Use the ∆H° and ∆S° values to calculate ∆G° at 50°C. Assume ∆H° and ∆S° are temperature independent.
[2] In the figure below, the standard free energy change is plotted in function of the temperature for the reactions: 20(s) +0,(g) → 20o(g) en C(s) +0,(g) → CO,(g) AG (kJ) -380 -400 -420 -440 800 900 1000 1100 T(K) How is it possible, starting from this drawing, to calculate the standard free energy change for the reaction below at a certain temperature?: CO2(9) + C(s) > 2CO(g)
A student determines the value of the equilibrium constant to be 6.29×104 for the following reaction.S(s,rhombic) + 2CO(g)SO2(g) + 2C(s,graphite)Based on this value of Keq:G° for this reaction is expected to be (greater, less) fill in the blank than zero.Calculate the free energy change for the reaction of 1.85 moles of S(s,rhombic) at standard conditions at 298K. G°rxn = _____ kJ
A student determines the value of the equilibrium constant to be 2.30 x 10¹6 for the following reaction. Ca(OH)2 (aq) + 2HCl(aq) → CaCl₂ (s) + 2H₂O(1) Based on this value of Keq AGO for this reaction is expected to be than zero. Calculate the free energy change for the reaction of 1.57 moles of Ca(OH)2 (aq) at standard conditions at 298 K. AGO rxn kJ
A student determines the value of the equilibrium constant to be 3.80×1013 for the following reaction.4HCl(g) + O2(g)2H2O(g) + 2Cl2(g)Based on this value of Keq:G° for this reaction is expected to be (greater, less) _____ than zero.Calculate the free energy change for the reaction of 2.00 moles of HCl(g) at standard conditions at 298K. G°rxn = ____ kJ
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A student determines the value of the equilibrium constant to be 2.33×1016 for the following reaction.Ca(OH)2(aq) + 2HCl(aq) ----> CaCl2(s) + 2H2O(l)Based on this value of Keq:ΔG° for this reaction is expected to be (greater, less) ____ than zero.Calculate the free energy change for the reaction of 2.34 moles of Ca(OH)2(aq) at standard conditions at 298K.ΔG°rxn = _______ kJ
A student determines the value of the equilibrium constant to be 2.69×10-10 for the following reaction.Fe2O3(s) + 3H2(g)2Fe(s) + 3H2O(g)Based on this value of Keq:G° for this reaction is expected to be (greater, less) fill in the blank than zero.Calculate the free energy change for the reaction of 2.05 moles of Fe2O3(s) at standard conditions at 298K. G°rxn = ____kJ
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What must the reaction quotient Q be, if the free energy is -961.941 kJ at 25.0°C? 5C2H2(g) + 5 H2(g) → C10H20(g) AGO = -925. 150 kJ.