A solution containing 0.15 M Pb2+ , 1.5×10−6 M Pb4+ , 1.5×10−6 M Mn2+ , 0.15 M MnO−4 , and 0.94 M HNO3 was prepared. For this solution, the balanced reduction half‑reactions and overall net reaction shown can occur. 5[Pb4++2e−↽−−⇀Pb2+] ?∘+=1.690 V 2[MnO−4+8H++5e−↽−−⇀Mn2++4H2O] ?∘−=1.507 V 5Pb4++2Mn2++8H2O↽−−⇀5Pb2++2MnO−4+16H+ A. Determine ?∘cell , Δ?∘ , and ? for this reaction. Calculate the value for the cell potential, ?cell , and the free energy, Δ? , for the given conditions. Calculate the value of ?cell for this system at equilibrium. ?cell= V D. Determine the pH at which the given concentrations of Pb2+ , Pb4+ , Mn2+ , and MnO−4 would be at equilibrium. pH=
A solution containing 0.15 M Pb2+ , 1.5×10−6 M Pb4+ , 1.5×10−6 M Mn2+ , 0.15 M MnO−4 , and 0.94 M HNO3 was prepared. For this solution, the balanced reduction half‑reactions and overall net reaction shown can occur. 5[Pb4++2e−↽−−⇀Pb2+] ?∘+=1.690 V 2[MnO−4+8H++5e−↽−−⇀Mn2++4H2O] ?∘−=1.507 V 5Pb4++2Mn2++8H2O↽−−⇀5Pb2++2MnO−4+16H+ A.
Determine ?∘cell , Δ?∘ , and ? for this reaction.
Calculate the value for the cell potential, ?cell , and the free energy, Δ? , for the given conditions.
Calculate the value of ?cell for this system at equilibrium. ?cell= V D.
Determine the pH at which the given concentrations of Pb2+ , Pb4+ , Mn2+ , and MnO−4 would be at equilibrium. pH=
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