Consider the reaction Al2O3(s) + 3C(graphite) + 3Cl2(g) → 2AICI3(s) + 3CO(g) Determine the following at...
Consider the reaction SnO2(s) + 2C(graphite) + 2Cl2(g) SnCl4(l) + 2CO(g) Determine the following at 298 K: Ho = -186.13 Correct: Your answer is correct. kJ/mol So = 144.75 Correct: Your answer is correct. J/mol-K Go = 229.04 Incorrect: Your answer is incorrect. kJ/mol What is log K at 298K (log K = ln K/2.3026)? log K = 40.15 Correct: Your answer is correct. (Hint log K = (ln K)/2.3026) Assume that Ho and So are temperature independent to determine...
3. Consider the following reaction and data: Al2O3 (1) + 3C (s) → 2A1 (1) + 3CO (g) AH° = 1340.0 kJ/mol AS9=586 J/K.mol a. Based on what we learned in the thermodynamics chapter, why is the entropy positive in this reaction? Hint: look at the chemical reaction. b. Calculate AG° at 1000.0 °C c. Is your answer to (b) spontaneous or nonspontaneous? d. What voltage (Eºcell) would be needed to produce ONE mole of aluminum?
4. Consider the reaction 3 C (graphite)2 H2O (g) CH4 (g) 2 CO (g) The following data are needed (all are at 298 K): S(J mol K) AH(kJ mol AAG(kJ mol) compound C, graphite 0 5.740 Н.О (g) - 241.82 188.83 - 228.57 CH4 (g) 186.26 -74.81 - 50.72 СО (g) 197.67 - 137.17 - 110.53 a) Determine A,G° and K for this reaction at 298 K and comment on the spontaneity of this process b) If you find that...
Using the following data determine the temperature (in K) at which the reaction H2O(g)+ C(s,graphite) ↔ H2(g) + CO(g) this becomes spontaneous. ΔfH° (H2O(g)) = -251.2 kJ mol-1 ΔfH° (C(s,graphite)) = 0.0 kJ mol-1 ΔfH° (H2(g)) = 0.0 kJ mol-1 ΔfH° (CO(g)) = -110.1 kJ mol-1 S° (H2O(g)) = 192.6 J K-1 mol-1 S° (C(s,graphite)) = 6.4 J K-1 mol-1 S° (H2(g)) = 136.9 J K-1 mol-1 S° (CO(g)) = 192.4 J K-1 mol-1
and
50. Given the following, determine AGof at 298 K for SnO. Sn(s)+SnO2(s) 2SnO(s); AG° = 12.0 kJ at 298K Substance AGOF(kJ/mol) at 298 K SnO(s) SnO2(s) ? -515.8 95. Consider the following reaction: 3C(s)+4H2(g) -C3H8(g); AH =-104.7 kJ; AS° = -287.4J/K at 298 K What is the equilibrium constant at 400.0 K for this reaction?
Calculate ΔSo in J/K for the following reaction: 2Fe2O3(s) + 3C(s) → 4Fe(s) + 3CO2(g) So(Fe2O3(s)) = 87.4 J/K/mol So(C(s)) = 5.7 J/K/mol So(Fe(s)) = 27.3 J/K/mol So(CO2(g)) = 213.7 J/K/mol
Consider the following reaction at 298 K. C(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/KC(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/K Calculate the following quantities. ΔSsys=ΔSsys J/K ΔSsurr= J/K ΔSuniv= J/K
1) Consider the following reaction: 3C(s) + 4H2(g) → C3H8(g); AH° = -104.7 kJ; AS = -287.4J/K at 298 K What is the equilibrium constant at 300.0 K for this reaction? AGº = -RT In K. AG° = AH° - TAS" (R=8.3145J/mol.K) (6 points)
Consider the reaction at 298 K. C(graphite)+2 H 2 (g)⟶ CH 4 (g)Δ?°=−74.6 kJ C(graphite)+2H2(g)⟶CH4(g)ΔH°=−74.6 kJ Calculate the quantities. Delta Ssys=_______ J/K Delata Ssurr =_______ J/K
macnillan learning Consider the following reaction at 298 K: 2C(graphite +01g) -> 2CO(g) F1° =-221.0 kJ / mol Calculate the following quantities. Find standard entropy values here. Number J/ (mol K sys Number J/(mol K surr Number Previous ⓧ Gve Up & View Solution > Check Answer Next Exit ..