Question

1. A voltaic cell is constructed that is based on the following reaction:
Sn2+(aq)+Pb(s)→Sn(s)+Pb2+(aq).

A. If the concentration of Sn2+ in the cathode compartment is 1.30 M and the cell generates an emf of 0.25 V , what is the concentration of Pb2+ in the anode compartment?

B. If the anode compartment contains [SO2−4]= 1.30 M in equilibrium with PbSO4(s), what is the Ksp of PbSO4?

2. A voltaic cell utilizes the following reaction:
2Fe3+(aq)+H2(g)→2Fe2+(aq)+2H+(aq).

A. What is the emf for this cell when [Fe3+]= 3.60 M , PH2= 0.98 atm , [Fe2+]= 8.0×10⁻⁴ M , and the pH in both compartments is 3.85?

3.

The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard-state conditions, the equation is

E=E∘−2.303RTnFlog10Q

where E is the potential in volts, E∘ is the standard potential in volts, R is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred, F is the Faraday constant, and Q is the reaction quotient. At standard temperature, 25 ∘C or 298 K, the equation has the form

E=E∘−(0.0592n)logQ

The reaction quotient has the usual form

Q=[products]x[reactants]y

A table of standard reduction potentials gives the voltage at standard conditions, 1.00 M for all solutions and 1.00 atm for all gases. The Nernst equation allows for the calculation of the cell potential E at other conditions of concentration and pressure.

A. For the reaction

2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g).  E∘=0.483 V

what is the cell potential at 25 ∘C if the concentrations are [Co3+]= 9.40×10⁻²M , [Co2+]= 0.641 M , and [Cl−]= 0.440 M and the pressure of Cl2 is PCl2= 8.60 atm ?

Answer 1

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