A reaction has AH° = +193 kļ/mol and AS° = +112 J/mol-K. At what temperature is the value of AG° equal to zero? A 1.72 K B) 298 K C) 580 K (D 1720 K E) None of these

For a given reaction, ΔH = +31.15 kJ/mol and ΔS = +126.83 J/K · mol. Above what temperature is the reaction is spontaneous?

For a particular chemical reaction, ΔH = 4.3 kJ and ΔS = –19 J/K. Under what temperature condition is the reaction spontaneous?

Calculate the equilibrium constant at 10.7 °C for each of the following reactions from the value of ΔG° = 56.1 kJ.I2(s)+Cl2(g)⟶2ICl(g)

The standard enthalpy of a reaction (ΔH°) is -80.9 kJ/mol and the standard entropy of the reaction (ΔS°) is 52.1 (J/mol*K). What is the ΔG° of this reaction at 300 K in kJ?

Calculate ΔGrxn at 375 K for the reaction below when PCO = 2.20 atm and PCO2 = 5.10 atm.  Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)        ΔG°rxn = –28.0 kJ

The pressure dependence of G is quite different for gases and condensed phases. Calculate ΔGm for the process (C,solid,graphite,1bar,298.15K)→(C,solid,graphite,300.bar,298.15K) The density for graphite is 2250 kg⋅m−3 Calculate ΔGm for the process (He,g,1bar,298.15K)→(He,g,300.bar,298.15K)

Calculate ΔG°rxn, ΔH°rxn, and ΔS°rxn of the following reaction: 2O3(g) -> 3O2(g)

Estimate ΔG°rxn for the following reaction at 307 K.CH4(g) + 2 O2(g) → CO2 (g) + H2O (l) ΔH°= -890.4 kJ; ΔS°= -242.2 J/K +816.0 kJ +66.3 kJ -66.3 kJ -816.0 kJ -250 kJ

A reaction has AH°= 100 kJ/mol and AS°= 250 J/mol.K. Is the reaction spontaneous at room temperature? If not, under what temperature conditions will it become spontaneous?