The Ksp for a very insoluble salt is 4.2 * 10-47 at 298 K. What is ∆G° for the dissolution of the salt in water?

COMPOUND ∆Hf (kJ/mole) S° (J/K mole) MgCO3 –1111 65.86 BaCO3 –1213 112.1 MgO –601.6 27.0 BaO –548 72.1 CO2 –393.5 213.8 Calculate ∆G° for the reaction of MCO3 ---> MO + CO2 at 25°C for the alkaline earth compounds Mg and Ba

Use the ∆G = ∆H – T∆S relationship to justify why the solubility of KOH(s) in water decreases as temperature is increased. Do not do any calculations. (HINT: the So value for KOH(s) is greater than that for KOH(aq).)

Determine K for a reaction at 200 K if ∆G° =24.4 kJ/mol. (R = 8.314 J/mol ･ K)

What is K for a reaction if ∆G° =-205.7 kJ/mol at 25°C? (R = 8.314 J/mol ･ K)

Determine the equilibrium constant for a reaction at 200.0 K if ∆G° =97.00 kJ/mol. (R = 8.314 J/mol ･ K)

Determine the equilibrium constant for a reaction at 200.0 K if ∆G° =-13.10 kJ/mol. (R = 8.314 J/mol ･ K)

Determine ∆G° for a reaction when ∆G = -117.2 kJ/mol and Q = 23 at 298 K. (R = 8.314 J/mol ･ K)

For the reaction delta H° = 98.8 kJ/mol and delta S° =141.5 J/(mol*K). 3H2 (g) +Fe2O2(s) →2Fe(s) +3H2O(g) (19) Over what temperature range (if any) is the reaction spontaneous?