19. Chemical Thermodynamics

What is the equilibrium constant (K) at 305 K when the standard Gibbs free energy change (ΔG°) is -4.75 kJ/mol?

What is ΔG° (in kJ/mol) for a redox reaction where two electrons are transferred with E°cell = -0.206 V?

What is ΔG (in kJ) for the formation of solid UF6 from uranium and fluorine at 25 °C when the partial pressure of F2 is 0.045 atm, given that the standard free energy of formation of UF6(s) is -2068 kJ/mol? Is the reaction spontaneous in the forward or the reverse direction?

Calculate and report ΔrG°T for the dissolution of Ca(OH)2(s) in water at 25°C, given that ΔH° = -985.2 kJ/mol and ΔS° = -0.353 kJ/mol·K.

Using the given reactions, calculate the standard free energy of formation, ΔG°f, for phosphoric acid (H3PO4). Given: 1. P4 (s) + 5 O2(g) → P4O10(s) ΔG° = -2697.0 kJ/mol 2. 2 H2(g) + O2(g) → 2 H2O(g) ΔG° = -457.18 kJ/mol 3. 6 H2O(g) + P4O10(s) → 4 H3PO4(l) ΔG° = ?

What is the entropy change (ΔS) of a reaction that has an enthalpy change (ΔH) of -70 kJ and a Gibbs free energy change (ΔG) of 18 kJ at a constant temperature of 76 degrees Celsius?