Consider the cell Pt(s)|H 2 (g,1atm)|H + (aq, a = 1)|Fe 3+ (aq),Fe 2+ (aq)|Pt(s) given that
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Consider the cell Pt(s)|H2(g,1atm)|H+ (aq, a = 1)|Fe3+ (aq),Fe2+ (aq)|Pt(s) given that Fe3+(aq) + e– ⇋ Fe2+ (aq) and E° = 0.771V.
a. If the cell potential is 0.712V, what is the ratio of Fe2+ (aq) to Fe3+ (aq)?
b. What is the ratio of these concentrations if the cell potential is 0.830V?
c. Calculate the fraction of the total iron present as Fe3+ (aq) at cell potentials of 0.650, 0.700, 0.750, 0.771, 0.800, and 0.900V. Graph the result as a function of the cell potential.
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Overall reaction H 2 g 2Fe 3 aq 2Haq 2Fe 2 aq E ...View the full answer
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