Calculate the cell potential of the following:
Pb(s) + 2SO4^2-(aq) + 4H^+ = H2SO3(aq) + PbSO4(s) + H2O(l)
To calculate the cell potential, we need to use the Nernst equation, which is given by:
E = E° - (RT / nF) ln(Q)
First, let's determine the half-reactions for the anode and cathode:
Anode (oxidation half-reaction):
Pb(s) -> PbSO4(s) + 2e-
Cathode (reduction half-reaction):
2H+(aq) + 2e- -> H2(g)
Now, let's find the standard cell potential by using standard reduction potentials:
E°cell = E°cathode - E°anode
The standard reduction potential for the reduction of 2H+(aq) to H2(g) is 0.00 V, and the standard reduction potential for the reduction of PbSO4(s) to Pb(s) is -0.36 V.
E°cell = 0.00 V - (-0.36 V)
E°cell = 0.36 V
Next, let's calculate the reaction quotient, Q:
Q = [H2SO3] / ([PbSO4] * [H+]^4)
Finally, let's substitute the values into the Nernst equation:
E = 0.36 V - ( (8.314 J/mol*K) * T) / (2 * (96485 C/mol) ) ln(Q)
Where T is the temperature in Kelvin.
Please provide the concentration values for [H2SO3], [PbSO4], and [H+], as well as the temperature at which you would like to calculate the cell potential.