Final answer:
For an electrochemical cell with k=0.05 and Q=0.10, we can conclude that Q > k, indicating the reaction will proceed in reverse to reach equilibrium, and Ecell is less than E°cell, indicating a non-spontaneous reaction under standard conditions.
Step-by-step explanation:
In an electrochemical cell, the relationship between Q (the reaction quotient), k (the equilibrium constant), and the cell potentials Ecell and E°cell can be understood through the Nernst equation.
Given that k is 0.05, and Q is 0.10, we can say that Q is greater than k. This implies that the reaction is not at equilibrium and will proceed in the reverse direction to reach equilibrium. Since Q > k, the cell potential Ecell must be less than E°cell, as the reaction is moving toward equilibrium where Q will equal k, and Ecell will reach 0 V. This status signifies a non-spontaneous reaction under standard conditions.
Additionally, according to the Nernst equation, for every tenfold change in Q, the cell potential changes by 0.0591/n V (where n is the number of moles of electrons transferred in the reaction).
Therefore, Ecell will continue to decrease until Q equals k, or when the concentrations of the reactants and products have reached equilibrium positions.