A(g) + B(g) -----> C(g)  ΔH = -25kJ/mole Is the reaction above spontaneous at all temps, no temp, low temp, or high temps?

Calculate ΔG for the reaction below, where the T = 298K, ΔH = 28.05 kJ, and the ΔS = 109 J/K. NH4NO3(s)  + H2O(l)     NH4+ (aq) + NO3- (aq)

What is the free energy change at 25oC for the reaction below, if the standard entropies of reactants and products are So (C(gr)) = 5.74 J/mol*K, So(H2(g)) = 130.68 J/mol*K, and So (C4H10(g)) = 310.1000 J/mol*K and the heat of formation of C4H10(g) is -126.1400 kJ/mol.4C(gr) + 5H2(g) ↔ C4H10(g)   ΔGo = -16.995 kJ   ΔGo = 16.995 kJ   ΔGo = 235.285 kJ   ΔGo = -235.285 kJ

Determine whether the following reactions are spontaneous or non-spontaneous. a) N2 (g) + 3 H2 (g) ⟶ 2 NH3 (g), ΔG = -32,960 J b) 2 NH3 (g) ⟶ N2 (g) + 3 H2 (g), ΔG = 32,960 J HINT: The change in free energy (ΔG) for reaction is equal to the difference in free energy between the products (Gproducts) and the reactants (Greactants): ΔG = (Gproducts) - (Greactants) In spontaneous reactions, the free energy of the products (Gproducts) of a reaction is less than the free energy of the reactants (Greactants). When this is the case, will the change in free energy (ΔG) will have a negative value or a positive value?