The reduction of iron and the oxidation of zinc creates a theoretical battery. Calculate the initial voltage of the battery if there are 1.3 M of Zn²⁺ and 2.8 M of Fe²⁺ in a 1.0-liter half-cells initially.

Predict the sign of E° when K > 1 and determine the value of K if E° = 0 V.

At 298 K, the standard cell potential of a cell is +0.124 V. If there are 4 electrons transferred in the reaction, what is the equilibrium constant value for the reaction?

Consider the reaction of Cu²⁺(aq) and Ni(s) at 25 °C. Calculate the equilibrium constant for this reaction using reduction potentials.  

At 298 K, the standard cell potential of a cell is +0.124 V. If there are 4 electrons transferred in the reaction, what is the equilibrium constant value for the reaction?

A cell produces 1.10 V at 298 K. Determine the equilibrium constant for the reaction happening inside the cell if n = 1.

At 25°C, what are the K_eq and ∆G°_rxn for the disproportionation reaction of liquid hydrogen peroxide to liquid water and oxygen gas?

An electrochemical is depicted with the cell notation Cu | Cu²⁺ || Mn³⁺ | Mn²⁺ | Pt. Draw the cell and show the flow of electrons and ions.