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In lecture today, Professor Lavelle said that you reverse the half-reaction that, after you reverse, will cause you to get a positive value of voltage. So, does this mean the voltage always has to end up as a positive value?
I think that statement mainly applies to the redox reactions having to do with batteries, since batteries never have a negative voltage. However, in the example on page 52 in the course reader, the is -0.54 V, showing that negative cell potentials are possible in certain cases.
Of course a negative net voltage is possible for a galvanic cell, it simply means so many volts of electricity need to be put into the system in order to have the reaction proceed in the set direction.
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