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?

Given the following E°_red

Cl₂(g) + 2 e⁻ → 2 Cl⁻ (aq)                                                  E°_red = 1.36 V

MnO₄⁻(aq) + 8 H⁺(aq) + 5 e⁻ → Mn²⁺(aq) + 4 H₂O(l)       E°_red = 1.51 V

What is the value of the equilibrium constant for the reaction at 298 K? 

10 Cl⁻ (aq) + 2 MnO₄⁻(aq) + 16 H⁺(aq) → 2 Mn²⁺(aq) + 8 H₂O(l) + 5 Cl₂(g)

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

For each of the Q/K ratios, identify whether E_cell and ΔG are negative, positive, or zero. 

Q/K ratios: <1, =1, >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.

A galvanic cell is made up of a Zn/Zn²⁺ anode and Pb/Pb²⁺ cathode connected together by a wire. A salt bridge also connects the two cells. Write a cell notation for this galvanic cell.