In which direction does a reaction proceed if ln(Q/K) is positive?

When ln(Q/K) is positive, this indicates that the reaction quotient (Q) is less than the equilibrium constant (K). This situation suggests that the concentration of products compared to reactants is lower than it would be at equilibrium, which is why Q is not equal to K.

In this context, the system will shift to the right, towards the products, to reach the equilibrium state. The reaction will proceed in the forward direction until the concentrations of the reactants and products adjust such that Q equals K, indicating equilibrium has been established.

Therefore, a positive value of ln(Q/K) directly indicates that the reaction moves towards the formation of more products to balance the system and achieve equilibrium.