Question

I'm not sure why, but I'm having trouble calculating the very basic Standard Cell Potential for a given cell, more information below.

Answer 1

@JFraser ,

The given overall equation is \[\rm 3Cu^{2+}(aq)+2Cr(s) \rightarrow 3Cu(s)+2Cr^{3+}(aq),\]
where the values I found in the table for the standard electric potential of the related half-reactions is: \[\rm Cu^{2+} \rightarrow Cu(s)=0.34 \ V,\]\[\rm Cr^{3+}(aq) + 3e^{-} \rightarrow Cr(s)= -0.74 \ V\]

Answer 2

What I'm doing is changing the sign on the second listed potential value because of the reaction being the other way around, and because the value then becomes 0.74 V, and since it is the larger value---it then becomes the Cathode, yes? The higher Reduction Potential value always is the Cathode, and the lowest value is the Anode.

Answer 3

Nevermind, figured it out, it's 1.08 V, just an algebra error.

Answer 4

good! you're right