Assignment:
Survey of physical chemistry
State all of the assumptions (e.g. ideal gas etc).
(previous reaction is 2H2(g) + O2(g) ----> 2H2O(g))
Given the reaction in the previous question at 298 Kelvin where H2 has a partial pressure of 0.10 bar, O2 is at 0.20 bar, and H2o is at 1.5 bar:
(a) Determine the direction and quantify the change in free energy the reaction must undergo to reach equilibrium.
(b) Calculate the equilibrium constant.
(c) Illustrate the reaction on a plot of Free Energy versus % Reactants/Products (show ?GO, the approximate position of Q for the given partial pressures, and the position of Q at equilibrium).
Provide complete and step by step solution for the question and show calculations and use formulas.