What is the equilibrium constant (K) at 305 K when the standard Gibbs free energy change (ΔG°) is +4.87 kJ/mol?

Calculate the value of ΔG° at 241.0°C for the formation of calcium chloride from its constituent elements: Ca(s) + Cl2(g) → CaCl2(s). Given that at 25.0°C, ΔH° is -795.8 kJ/mol, ΔG° is -748.1 kJ/mol, and ΔS° is -159.8 J/K.

Given the reaction IF7(g) + I2(g) → IF5(g) + 2 IF(g) with ΔH°rxn = -89 kJ, ΔH°f for IF7(g) = -941 kJ/mol, and ΔH°f for IF5(g) = -840 kJ/mol, calculate the standard enthalpy of formation (ΔH°f) for IF(g).

What is the change in Gibbs free energy, ΔG, at 25°C for the reaction N₂(g) + 3 H₂(g) → 2 NH₃(g) given ΔH = -92.22 kJ and ΔS = -198.75 J/K?

What is the equilibrium constant (K) at 305 K when the standard Gibbs free energy change (ΔG°) is +1.61 kJ/mol?

What is the equilibrium constant (K) at 305 K when the standard Gibbs free energy change (ΔG°) is -3.23 kJ/mol?

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?