Final answer:
A spontaneous reaction with favored products has a negative Delta G, a K value greater than 1, and a positive E cell potential.
Step-by-step explanation:
When a reaction is spontaneous and products are favored, certain thermodynamic and electrochemical properties are related to the reactants and products. The Gibbs free energy (ΔG) is negative, indicating that the process is favorable and will occur without the addition of external energy. The equilibrium constant (K) is greater than 1, meaning the concentration of products is greater than the concentration of reactants at equilibrium, illustrating that products are favored. In terms of electrochemistry, the cell potential (E⁰₃₃₂₉) is positive, which shows that the electrochemical cell can perform work spontaneously when connecting the electrodes.
If ΔG is exactly zero, E⁰₃₃₂₉ is zero, and K is equal to 1, then the system is at equilibrium and neither reactants nor products are favored. Therefore, for a spontaneous reaction under standard conditions, the values of K and E⁰₃₃₂₉ are expected to be greater than 1 and greater than 0, respectively.