2) The equilibrium constant Keq for the reaction A B is 1 x 105 at room temperature (25°C). a) You make a solution containing compound A at a concentration of 1 M and compound B at a concentration of 1 mM of B, and let the reaction proceed to equilibrium. What are the equilibrium concentrations of A and B? b) Calculate the standard free-energy change (AG) for this reaction. c) What is the standard free-energy change (AG) for the inverse reaction (BA)? d) With the provided information, can you estimate how long will it take this reaction to reach equilibrium? e) In a reaction cell that has not reached equilibrium, we have the following instantaneous concentrations: [A] = 0.05 mM; [B] = 15 mM. Calculate the actual free-energy change (AG) for the system as it reaches equilibrium at 25°C.

Table 2 Isotopic masses Mass (amu) Table 1 Standard free energy of formation at 600 K Isotope Compound AG? (kJ/mol) 140 Eu 139.9281 -25.2 CH48) CO«) H2O(g) 141 Eu 140 Gd 141Gd 140.9249 -56.9 139.9337 -215.1 140.9321 142 Gd 140Sm 141Sm 141.9281 139.9190 140.9185 142Sm 141.9152 Identify the following reaction as acid-base, Lewis acid-base, redox or none of the above. CH4 + 2 O2 → CO2 + 2 H2O

4. Determine whether the hydrogenation of propene gas reaction at 298 is spontaneous or nonspontaneous by calculating AG C,H, (g) + H, (g) → CH, (1) Enthalpy of formation Entropy C,H, 267 J/mol*K 20.6kJ/mole. C,H, 270.2 J/mol*K-103.9 kJ/mol.

Please give a explanation and show work