Nitrate (NO3 and Nitrite (NO2) look a lot alike, and so do Sufate (S042 and Sulf

Question

Nitrate (NO3 and Nitrite (NO2) look a lot alike, and so do Sufate (S042 and Sulfite (s032). Some redox potentials in the tower are pH specific, for example Iron (Fe) depends on pH Make sure you pick the one the question is asking you about. Use the equation E cell Ereduction + E0oxidation and the redox tower on page 82 of the textbook to solve for E0cell. What is the redox potential ( E) for the oxidation of glucose paired with the reduction of Fe3+ at physiological pH (pH-7)? . Enter your answer rounded to two decimal places Do these half reactions form a spontaneous reaction? A) Yes B) No Enter A for yes or B for no.

Explanation / Answer

For the nitrate and the sulphate cell we will first determine what reaction to choose for oxidation and what to choose for reduction half reactions .

As we can see , sulphate has a negative reduction EMF ( -0.52)

The nitrates have reduction emf of (+0.42) . Positive value means the reaction is feasible . This means in a cell with sulphate and nitrate , nitrate will be reduced and sulphate will be oxidised .

Now for the Ecell , we need to find Eox and Ered for the cell.

As we know ,sulphate will be oxidised , but on the tower we have reduction EMF . So we just inverse the negative sign to positive and we have the Eox .

Therefore ,

Ecell = Eox + Ered =( +0.52) + (+0.43) = +0.95 V .

2) redox potential is calculated by adding up the emf of the oxidation and reduction half reactions .

Oxidation emf of glucose = +0.43

Reduction emf of iron = +0.2

There fore redox potential = (+0.43) + (+0.2) = +0.63V .

3) yes because the Ecell will be positive

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