A certain half-reaction has a standard reduction potential . An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have

Check the explanation

Explanation:

The potential of a cell can be calculated as:

cell = E . cathode - E

So, incase we will be needing a potential of at least 1.10 V and there is a cathodic potential of 1.03 V, we will therefore be needing an anodic potential with a value of -0.07 V or lower (that is, more negative). So yes, there is a minimum and it should be - 0.07 V.

so far the cell has to be of AT LEAST 1.10 V and an upper limit is absent, then the reduction potential at the anode has no maximum value (again, we will have to take into account that it has to be more negative than -0.07 V).

A half-reaction that complies and corrolates with this condition is the following (written as an oxidation, which is how it actually happens at the anode):

Pb(s) --> Pb2+(aq) + 2 e-

pythagoras' theorem

square root (-5^2+9^2)

square root (25+81)

square root (106)

angle is tan^-1(9/5)

neg x, pos y