Environmental issues arising from arsenic toxicity are frequently associated with the oxidation of pyrite, which generates significant SO4^2- and acid. Write a balanced half-cell reaction for the oxidate of HS^- to SO4^2-. Assume aHS^-=aSO4^2- (a stands for activity) and plot a phase boundary between the two ions on an Eh-pH diagram. PLEASE HELP! I dont understand how to do this at all.
Thermodynamic data Delta Gf (KJ/mol)
Al^3+ -485.0
Ni^2+ -45.6
NH4^+ -79.31
NO3^- -108.74
SO4^2- -177.75
HS^- 2.93
H2O -237.129
You have the reaction:
Using the energies of formation you can calculate the energy of reaction
The energy for the electron is negligible and for the H+ is 0 thus, the energy for water is -237.129 kJ/mol, for SO4 -744.53 kJ/mol and for HS- 12.05kJ/mol, I am using from my own data because you are mixing some in kcal and other is kJ
Now you can calculate the potential:
Using the nernst equation:
n is the electrons transfered
<-----You can rearrange the [H+] concentration into pH, and assuming the [SO4]=[HS]
<-----using the logarithm rules, the 9 is the coefficient of the log and form the definition pH=-log[H+], yields:
<------This is the equation of the line that divides the two ions in a Eh-pH diagram
Environmental issues arising from arsenic toxicity are frequently associated with the oxidation of pyrite, which generates...