(a) What is the standard Gibbs free energy of the reaction CO(g) + H₂O(g) → CO₂(g) + H₂(g) when K = 1.00? 

(b) From data available in Appendix 2A, estimate the temperature at which K = 1.00. 

(c) At this temperature, a cylinder is filled with CO(g) at 10.00 bar, H₂O(g) at 10.00 bar, H₂(g) at 5.00 bar, and CO₂(g) at 5.00 bar. What will be the partial pressure of each of these gases when the system reaches equilibrium? 

(d) If the cylinder were filled instead with CO(g) at 6.00 bar, H₂O(g) at 4.00 bar, H₂(g) at 5.00 bar, and CO₂(g) at 10.00 bar, what would the partial pressures be at equilibrium?

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2A THERMODYNAMIC DATA AT 25 °C Inorganic Substances Substance Aluminum Al(s) Al³+ (aq) AI(OH)3(s) Al₂O3(s) AlCl3(s) AlBr,(s) Antimony Sb(s) SbH3(g) SbCl3(g) SbCls (g) Arsenic As(s), gray AsO³(aq) A$2S3(S) Barium Ba(s) Ba²+ (aq) BaO(s) BaCO3(s) BaCO3(aq) Molar mass, M/(g.mol-¹) 26.98 26.98 78.00 101.96 133.33 266.68 121.76 124.78 228.11 299.01 74.92 138.92 246.05 137.33 137.33 153.33 197.34 197.34 Enthalpy of formation, AH/(kJ-mol-¹) 0 -524.7 -1276 -1675.7 -704.2 -527.2 0 +145.11 -313.8 -394.34 0 -888.14 - 169.0 0 -537.64 -553.5 -1216.3 -1214.78 Gibbs free energy of formation, AG/(kJ.mol-¹) 0 -481.2 -1582.35 -628.8 0 +147.75 -301.2 -334.29 0 -648.41 -168.6 0 -560.77 -525.1 -1137.6 -1088.59 Molar heat capacity, Cr.m/(J.K-¹-mol¹) 24.35 79.04 91.84 100.6 25.23 41.05 76.69 121.13 24.64 116.3 28.07 47.78 85.35 Molar entropy, Sm/(J.K¹-mol-¹) 28.33 -321.7 50.92 110.67 180.2 45.69 232.78 337.80 401.94 35.1 -162.8 163.6 62.8 +9.6 70.42 112.1 -47.3