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Based on the following thermodynamic data, Species AfHº (kJ/mol) SO (/K.mol) M(s) 0.0 27.4 O2(g) 0.0...
6. Use the following thermodynamic data to calculate me following thermodynamic data to calculate AS for...
6. Use the following thermodynamic data to calculate me following thermodynamic data to calculate AS for the formation of Fe2O3 at 298.2 K Species Fe(s) O2(g) Fe2O3(s) AH (kJ/mol-rxn) S (J/Komol-rxn) AH producers - 0.0 27.8 0.0 Alveolu 205.1 -825.5 87.4 -825.5 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) a) -2202.7J/ KX b) -546.2 J/K AS-A Sproducts-AS rearsants c) +546.2 J/K d) +2202.7J/ KV (2 X 87,4)-((4X27.8)+(3x205.1)) e) +4984.9 J/K 1 = 174,8-(111.27615.3) Ssurr -4H = 174,8-726.5 Assus =-551.75l...
Thermodynamic Quantities for Selected Substances at 298.15 K (25 °C) Substance AHºf (kJ/mol) AG°f (kJ/mol) S (J/K-m...
Thermodynamic Quantities for Selected Substances at 298.15 K (25 °C) Substance AHºf (kJ/mol) AG°f (kJ/mol) S (J/K-mol) Oxygen O2 (g) H20 (1) 0 -285.83 205.0 69.91 -237.13 10 CHCOOH 0 Sulfur S (s, rhombie) 0 SO2(g) -269.9 SO3(g) -395.2 -300.4 31.88 248.5 256.2 OM-370.4 FASO for the decomposition of gaseous sulfur trioxide to solid elemental sulfur 3. The value of ASº for the d and gaseous oxygen, 2503 (g) → 28 (s, rhombie) + 302 (g) J/K. mol. (show your...
1. Thermodynamic data at 298 K. So (J/K) AHOf (kJ/mol) 205 0 O2 (g) 239 142.7...
1. Thermodynamic data at 298 K. So (J/K) AHOf (kJ/mol) 205 0 O2 (g) 239 142.7 O3 (g) a) Calculate the standard entropy change for the production of ozone from oxygen at 298 K. Is this an increase or decrease in randomness? Explain briefly. -> 203 (g) 302 (g) b) Calculate the standard free energy change for this reaction. Is this reaction spontaneous under standard conditions? c) Calculate the AG° of formation for ozone.
CO(g) + O2(g) -> CO2(g) (unbalanced) Using the equation and thermodynamic data: AH(rxn) --566.0 kJ (for the bal...
CO(g) + O2(g) -> CO2(g) (unbalanced) Using the equation and thermodynamic data: AH(rxn) --566.0 kJ (for the balanced equation) Substance sºu/mol*K) O2(g) 205.0 CO(g) 197.7 CO2(g) 213.8 NOTE: Write all answers to four significant figures. a. What is the Assys(J/mol*K) - b. What is the Assurr(J/mol*K) = c. What is the Asuniv(J/mol*K) - d. At what temperature(°C) will the reaction go from spontaneous to non-spontaneous?
15. Consider the following two reactions, with thermodynamic data at 298.15 K (1) Pb(s) + CO(g)...
15. Consider the following two reactions, with thermodynamic data at 298.15 K (1) Pb(s) + CO(g) → Pb0(s) + C(graphite) (2) 2 C(graphite) + O2(g) → 2 CO(g) Ar =-107 kl mori ΔG. =-51 kl mor Which of the following statements is(are) FALSE? (Assume AHt and AS" are independent of temperature.) G,-[PbO(s)) +188 kJ mol-1 Both reactions are spontaneous under standard conditions at room temperature. AS"for reaction 2 is-178 J K-1 mori at 298.15 K. Reaction 2 is spontaneous at...
Using the equation and thermodynamic data: CO(g) + O2(g) --> CO2(g) (unbalanced) AH(rxn) = -566.0 kJ...
Using the equation and thermodynamic data: CO(g) + O2(g) --> CO2(g) (unbalanced) AH(rxn) = -566.0 kJ ( for the balanced equation) Substance sºu/mol*K) O2(g) 205.0 CO(g) 197.7 CO2(g) 213.8 NOTE: Write all answers to four significant figures. a. What is the Assys(J/mol*K) = b. What is the Assurr(J/mol*K) = c. What is the Asuniv( J/mol*K) = d. At what temperature(°C) will the reaction go from spontaneous to non-spontaneous?
Calculate the equilibrium constant from the standard free energy change. Using standard thermodynamic data (linked), calculate...
Calculate the equilibrium constant from the standard free energy change. Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction 2502(g) + O2(0) 2503(9) AH°F (kJ/mol) AGⓇ, (kJ/mol sº (/mol K) 205.1 Oxygen 02(0) (9) O3(9) 249.2 231.7 161.1 142.7 163.2 238.9 AH°: (kJ/mol Agºr (kJ/mol) 5° (J/mol K) 31.8 0.3 0.3 278.8 3 3.0 167.8 33.0 - 15.0 Sulfur S(s, rhombic) S(s, monodinic) S(g) Sz"(aq) Sg(9) SzCl2(g) SF6(9) H2S(9) soz(9) SO3(0) 1 0....
Substance(kJ/mol) M304 M(s) 02(9) Consider the decomposition of a metal oxide to its elements, wh...
Substance(kJ/mol) M304 M(s) 02(9) Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. -11.00 0 0 M1,0),(s) 근 3MW-202(g) What is the standard change in Gibbs energy for the reaction, as written, in the forward direction? Number kJ/ mol What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K? Number K-0.44 What is the equilibrium pressure of O2(g) over M(s) at 298 K? Number Po,0.666 atm...
Use standard thermodynamic data (in the Chemistry References) to calculate AG at 298.15 K for the...
Use standard thermodynamic data (in the Chemistry References) to calculate AG at 298.15 K for the following reaction, assuming that all gases have a pressure of 10.88 mm Hg. 2NO(g) + O2(g)—>2NO2(g) AG= kJ/mol Nitrogen AHºf (kJ/mol) AG°f (kJ/mol) sº (J/mol K) N2(g) 191.6 N(9) 472.7 455.6 153.3 NH3(9) -46.1 -16.5 192.5 NH3(aq) -80.0 -27.0 111.0 NH4+ (aq) -132.0 -79.0 113.0 NO(9) 90.3 86.6 210.8 NOCI(g) 51.7 66.1 261.8 NO2(9) 33.2 240.1 51.3 104.2 N2O(9) 82.1 219.9 N204(9) 9.2 97.9...
Using the data: C2H4(g), = +51.9 kJ mol-1, S° = 219.8 J mol-1 K-1 CO2(g), = ‑394 kJ...
Using the data: C2H4(g), = +51.9 kJ mol-1, S° = 219.8 J mol-1 K-1 CO2(g), = ‑394 kJ mol-1, S° = 213.6 J mol-1 K-1 H2O(l), = ‑286.0 kJ mol-1, S° = 69.96 J mol-1 K-1 O2(g), = 0.00 kJ mol-1, S° = 205 J mol-1 K-1 calculate the maximum amount of work that can be obtained, at 25.0 °C, from the process: C2H4(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(l)
6. Use the following thermodynamic data to calculate me following thermodynamic data to calculate AS for the formation of Fe2O3 at 298.2 K Species Fe(s) O2(g) Fe2O3(s) AH (kJ/mol-rxn) S (J/Komol-rxn) AH producers - 0.0 27.8 0.0 Alveolu 205.1 -825.5 87.4 -825.5 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) a) -2202.7J/ KX b) -546.2 J/K AS-A Sproducts-AS rearsants c) +546.2 J/K d) +2202.7J/ KV (2 X 87,4)-((4X27.8)+(3x205.1)) e) +4984.9 J/K 1 = 174,8-(111.27615.3) Ssurr -4H = 174,8-726.5 Assus =-551.75l...
Thermodynamic Quantities for Selected Substances at 298.15 K (25 °C) Substance AHºf (kJ/mol) AG°f (kJ/mol) S (J/K-mol) Oxygen O2 (g) H20 (1) 0 -285.83 205.0 69.91 -237.13 10 CHCOOH 0 Sulfur S (s, rhombie) 0 SO2(g) -269.9 SO3(g) -395.2 -300.4 31.88 248.5 256.2 OM-370.4 FASO for the decomposition of gaseous sulfur trioxide to solid elemental sulfur 3. The value of ASº for the d and gaseous oxygen, 2503 (g) → 28 (s, rhombie) + 302 (g) J/K. mol. (show your...
1. Thermodynamic data at 298 K. So (J/K) AHOf (kJ/mol) 205 0 O2 (g) 239 142.7 O3 (g) a) Calculate the standard entropy change for the production of ozone from oxygen at 298 K. Is this an increase or decrease in randomness? Explain briefly. -> 203 (g) 302 (g) b) Calculate the standard free energy change for this reaction. Is this reaction spontaneous under standard conditions? c) Calculate the AG° of formation for ozone.
CO(g) + O2(g) -> CO2(g) (unbalanced) Using the equation and thermodynamic data: AH(rxn) --566.0 kJ (for the balanced equation) Substance sºu/mol*K) O2(g) 205.0 CO(g) 197.7 CO2(g) 213.8 NOTE: Write all answers to four significant figures. a. What is the Assys(J/mol*K) - b. What is the Assurr(J/mol*K) = c. What is the Asuniv(J/mol*K) - d. At what temperature(°C) will the reaction go from spontaneous to non-spontaneous?
15. Consider the following two reactions, with thermodynamic data at 298.15 K (1) Pb(s) + CO(g) → Pb0(s) + C(graphite) (2) 2 C(graphite) + O2(g) → 2 CO(g) Ar =-107 kl mori ΔG. =-51 kl mor Which of the following statements is(are) FALSE? (Assume AHt and AS" are independent of temperature.) G,-[PbO(s)) +188 kJ mol-1 Both reactions are spontaneous under standard conditions at room temperature. AS"for reaction 2 is-178 J K-1 mori at 298.15 K. Reaction 2 is spontaneous at...
Using the equation and thermodynamic data: CO(g) + O2(g) --> CO2(g) (unbalanced) AH(rxn) = -566.0 kJ ( for the balanced equation) Substance sºu/mol*K) O2(g) 205.0 CO(g) 197.7 CO2(g) 213.8 NOTE: Write all answers to four significant figures. a. What is the Assys(J/mol*K) = b. What is the Assurr(J/mol*K) = c. What is the Asuniv( J/mol*K) = d. At what temperature(°C) will the reaction go from spontaneous to non-spontaneous?
Calculate the equilibrium constant from the standard free energy change. Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction 2502(g) + O2(0) 2503(9) AH°F (kJ/mol) AGⓇ, (kJ/mol sº (/mol K) 205.1 Oxygen 02(0) (9) O3(9) 249.2 231.7 161.1 142.7 163.2 238.9 AH°: (kJ/mol Agºr (kJ/mol) 5° (J/mol K) 31.8 0.3 0.3 278.8 3 3.0 167.8 33.0 - 15.0 Sulfur S(s, rhombic) S(s, monodinic) S(g) Sz"(aq) Sg(9) SzCl2(g) SF6(9) H2S(9) soz(9) SO3(0) 1 0....
Substance(kJ/mol) M304 M(s) 02(9) Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. -11.00 0 0 M1,0),(s) 근 3MW-202(g) What is the standard change in Gibbs energy for the reaction, as written, in the forward direction? Number kJ/ mol What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K? Number K-0.44 What is the equilibrium pressure of O2(g) over M(s) at 298 K? Number Po,0.666 atm...
Use standard thermodynamic data (in the Chemistry References) to calculate AG at 298.15 K for the following reaction, assuming that all gases have a pressure of 10.88 mm Hg. 2NO(g) + O2(g)—>2NO2(g) AG= kJ/mol Nitrogen AHºf (kJ/mol) AG°f (kJ/mol) sº (J/mol K) N2(g) 191.6 N(9) 472.7 455.6 153.3 NH3(9) -46.1 -16.5 192.5 NH3(aq) -80.0 -27.0 111.0 NH4+ (aq) -132.0 -79.0 113.0 NO(9) 90.3 86.6 210.8 NOCI(g) 51.7 66.1 261.8 NO2(9) 33.2 240.1 51.3 104.2 N2O(9) 82.1 219.9 N204(9) 9.2 97.9...
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