Thermodynamics and equilibrium are concepts that overlap. Given the following information, estimate the magnitude (is it large, small or close to 1) of K for each reaction listed and explain based on thermodynamic values of delta H and delta S for the reactions A, B, and C. You may calculate delta H and delta S values using constants from the thermodynamics table on the content page or you can qualitatively interpret the entropy change of a reaction (delta S) using these factors below: i) If there are more particles (# of moles) in the products compared to the reactants, delta S is positive. ii) If there are less particles (# of moles) in the products compared to the reactants, delta S is negative. iii) If there are more gas particles (# of moles) in the products compared to the reactants, delta S is positive. iv) If there are less gas particles (# of moles) in the products compared to the reactants, delta S is negative. A) Fe₃O₄ (s) + 4H₂ (g) --> 3Fe(s) + 4 H₂ O(g) B) 4NH₃ (g) + 5O₂ (g) --> 4NO(g) + 6H₂ O(l) C) BaCO₃ (s) + C(s, graphite) --> BaO(s) + 2CO(g)