A certain voltaic cell uses the half-reactions shown below:

Anode: Zr(s) + 2 H₂O(l) → ZrO₂(s) + 4 H⁺(aq) + 4 e^–
Cathode: Mn²⁺(aq) + 2 e^– → Mn(s)

Using the thermodynamic values below at 25.0°C, calculate the cell potential (E°) and the equilibrium constant K for the overall cell reaction.

For the reaction 2 I^–(aq) + Hg²⁺(aq) → I₂(s) + Hg(l) at 298 K, calculate Eº_cell, K, ΔGº_rxn, and fill the table below.

What are the balanced equation, standard emf, ΔG°, and K value at 298 K for the oxidation of aqueous chloride ion by Hg₂²⁺(aq) to produce Cl₂(g)?

Draw a cell setup for the electrolysis of molten ZnCl₂ and indicate the direction of the flow of electrons.

In an experiment, Hg₂Cl₂(s) is converted into Hg(l) and Cl₂(g). Is the overall reaction a galvanic or electrolytic cell?

Small-scale production of strontium metal can be performed using SrCl₂ placed in an electrochemical cell with molten KCl as the electrolyte. Upon reduction of SrCl₂, Cl^– ions are subsequently oxidized to Cl₂ gas. A set-up is pictured below.

Identify the reactions at the cathode and anode.

Provide the balanced equation and calculate the value of E° for the formation of O₂ and H₂O from H₂O₂ given the following half-reactions and corresponding E° values:

H₂O₂(aq) + 2 H⁺(aq) + 2e⁻ → 2 H₂O(l)                E°_H2O2→H2O = 1.78 V

O₂(g) + 2 H⁺(aq) + 2e⁻ → H₂O₂(aq)                     E°_O2→H2O2 = 0.70 V

Determine if the reaction is spontaneous under standard-state conditions.

Among the following spontaneous cell reactions,

Y⁺ + W → Y + W⁺

W⁺ + Z → W + Z⁺

Y⁺ + Z → Y + Z⁺

X⁺ + Z → X + Z⁺

Y⁺ + X → Y + X⁺

Identify the reaction that produces the highest voltage.

Everyday household items such as flashlights and radios use alkaline batteries. The overall reaction in the battery is as follows: Zn(s) + 2 MnO₂(s) ⇌ ZnO(s) + Mn₂O₃(s). Using a reliable source, give the two half-reactions that occur in the battery and calculate the standard emf generated by the voltaic cell. 

Determine what happens to the cell voltage when each of the following changes is made to the Daniell cell originally in standard conditions. Show the balanced equation for each reaction. 

a) 2.25 M Zn(NO₃)₂ is added to the anode compartment

b) 2.25 M CuSO₄ is added to the cathode compartment

c) 1.00 M Cu(NO₃)₂ is added to the cathode compartment

d) 2.25 M H₂SO₄ is added to the cathode compartment

At 25°C, the voltage of a Co/Co²⁺ concentration cell is 0.12 V. One of the half cells has a concentration of 1.2x10^-3 M. Determine the concentration of Co²⁺ in the other half-cell assuming that it has a smaller concentration