What is the balanced overall (net) cell reaction?

draw a diagram of the cell and calculate the standard cell potential

show a particle diagram of what the salt bridge looks like.

Calculate Eocell. Is this cell spontaneous?

Write equations for the reaction between iron and a solution of silver nitrate to produce Fe2+ ions and Ag(s):

a. write the balanced half-cell reactions

b. write the overall balanced equation for the reaction

c. Calculate Eocell. Is this cell spontaneous?

d. Calculate Ecell if the starting concentrations are [Fe2+] = 0.5M and [Ag+] = 2.5 M

Write equations for the reaction between manganese (IV) dioxide and the hypochlorite ion to produce the permanganate ion and the chloride ion in basic solution:

a. write the balanced half-cell reactions

b. write the overall balanced equation for the reaction

c. draw a diagram of the cell and calculate the standard cell potential

d. Calculate the standard free energy of this cell.

e. Calculate K of this reaction.

Given the following standard reduction potentials in acid solution:

O2 + 4H+ + 4e- ↔ 2H2O E° = +1.23V

Sn4+ + 2e- ↔ Sn2+ E° = +0.13V

Zn2+ + 2e- ↔ Zn(s) E° = -0.76V

Write the formula of the weakest reducing agent.

Write the formula of the strongest reducing agent.

Write the formula of the strongest oxidizing agent.

Write a balanced equation for a spontaneous reaction which involves the tin and zinc redox couples.

Permanganate ions oxidize iodide ions to iodine in acidic solution, and are reduced to manganese(II) ions. Write and balance the net ionic equation for the reaction by the ion-electron method.

Given the two half reactions and their potentials, which net reaction is spontaneous?

Ni2+(aq) + 2e- → Ni(s) E° = -0.25 V

Mg2+(aq) + 2e- → Mg(s) E° = -2.37 V

a) Ni(s) + Mg2+(aq) → Mg(s) + Ni2+(aq) b) Ni2+(aq) + Mg(s) → Mg2+(aq) + Ni(s)

c) Ni(s) + Mg(s) → Mg2+(aq) + Ni2+(aq) d) Mg2+(aq) + Ni2+(aq) → Mg(s) + Ni(s)

e) Mg2+(aq) + Mg(s) → Ni(s) + Ni2+(aq)

Consider the following pairs of half-reactions, decide which of the two half-reactions will occur at the anode and which will occur at the cathode, draw diagrams for the cells, and calculate the standard cell potentials:

a. Co2+ (aq) + 2e- → Co(s) Eo = -0.28V b. Ni2+ (aq) + 2e- → Ni(s)

Ag+ (aq) + e- → Ag(s) Cu2+ (aq) + 2e- → Cu(s)

An electrochemical cell of notation Pd | Pd2+ | | Cu2+ | Cu has an E° = -0.65 V. If we know that the standard reduction potential of Cu2+/Cu is E° = 0.34 V, what is the standard reduction potential for Pd2+/Pd?

Many different ways have been proposed to make batteries. One cell is set up with copper and lead electrodes in contact with CuSO4(aq) Pb(NO3)2(aq), respectively. If the Pb2+ and Cu2+ are each 1M, what is the cell potential? Pb2+ + 2e- ↔ Pb E° = -0.13V

Cu2+ + 2e- ↔ Cu E° = +0.34V

If sulfuric acid is added to the Pb(NO3)2 solution, forming a precipitate of PbSO4, what will happen to the cell potential?