At 1500 degree C the equilibrium constant for the reaction CO(g) + 2H_2(g) CH_3OH(g) has the value K_p = 1.4 times 10^-7, Calculate Delta G degree for this reaction at 1500 degree C. a) 105 kJ/mol b) 1.07 kJ/mol c) -233 kJ/mol d) -105 kJ/mol e) 233 kJ/mol Calculate Delta S degree for the reaction 4Cr(s) + 3O_2(g) rightarrow 2Cr_2 O_3(s). Substance: Cr(s) O_2(g) Cr_2O_3(s) S degree (J/K middot mol): 23.77 205.138 81.2 a) -548.1 J/K b) -147.7 J/K c) 147.7 J/K d) 310.1 J/K e) 548.1 J/K Consider saturated solutions of the following compounds. Which solution has the highest concentration of F^- ion? a) BaF_2 Ksp = 1.3 times 10^-6 b) CaF_2 Ksp = 3.9 times 10^-11 c) MgF_2 Ksp = 3.7 times 10^-8 d) PbF_2 Ksp = 3.6 times 10^-8 e) SrF_2 Ksp = 7.9 times 10^-10 Entropy is a measure of a) free energy. b) the heat of a reaction. c) molecular randomness. d) the rate of a reaction. For iron(III) hydroxide, Fe(OH)_3, the relationship between K_sp and s, the molar solubility, is K_sp = s^2 K_sp = 3s^4 K_sp = 4s^3 K_sp = 27s^4 K_sp = 3s^2