Help Solving a Puzzling Galvanic Cell Experiment!

AI Thread Summary
The experiment involved a galvanic cell with zinc and iron half-cells, measuring a potential of 0.287V, which is significantly lower than the expected 1.53V based on standard electrode potentials. The standard potential for the reduction of Fe+3 to Fe+2 is 0.77V, while zinc's reduction potential is -0.76V. The discrepancy arises from the actual concentrations and activities of the ions in the solutions, which can affect the measured cell potential. Additionally, the Nernst equation may need to be applied to account for the non-standard conditions. Understanding these factors is crucial for interpreting the experimental results accurately.
supercali
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iwe had an expirament that goes like this
we made a galvanic cell with half cell zinc and its solution (Zn(NO3)2) and the other half cell was with iron and its solution (Fe(NO3)3) (the Fe solution with ions Fe+3) (both same concentration!) the potential i measured was 0.287V
now i just don't understand how can this be
because the standard potential of Fe+3 + e -> Fe+2 is 0.77V and for Zink it is -0.76V thus we should get in the experiment that the measured potential is 1.53V i just can't understand my result
help please
 
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You won't get different answer here than the one I have posted on chemical forums.
 
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