Final answer:
In chemistry, ∆G < 0, Ecell > 0, and K > 1 indicate a forward spontaneous reaction favoring products, while ∆G > 0, Ecell < 0, and K < 1 denote a reverse spontaneous reaction favoring reactants. At ∆G = 0, Ecell = 0, and K = 1, the system is at equilibrium with no net change.
Step-by-step explanation:
When analyzing chemical reactions, certain parameters can be utilized to predict the direction of the reaction under standard conditions. ∆G (Gibbs free energy change), K (equilibrium constant), and Ecell (cell potential) are these parameters, providing insight into the reaction's spontaneity and equilibrium position.
If ∆G is less than zero (∆G < 0), it indicates that the reaction will proceed spontaneously in the forward direction, favoring the formation of products. Conversely, if ∆G is greater than zero (∆G > 0), the reaction is non-spontaneous in the forward direction and spontaneous in the reverse direction, favoring reactants. At ∆G equal to zero (∆G = 0), the system has reached equilibrium and there is no net change in reactants or products.
Similarly, an Ecell greater than zero (Ecell > 0) indicates a positive voltage and a spontaneous reaction as written, while a negative Ecell implies a spontaneous reaction in the opposite direction. For the equilibrium constant K, a value greater than 1 (K > 1) signifies that, at equilibrium, the concentration of products is greater than that of reactants, indicating product-favored conditions. If K is exactly 1 (K = 1), it denotes an exact balance between reactants and products, characterizing equilibrium.