Question

List three reasons why an experimentally measured reduction potential would not equal the theoretical reduction potential.

Answer 1

Solution :

There are many things which cause the cell REDUCTION potential to be less than theoretical REDUCTION potential:

Anything at all which causes any internal resistance in the cell or the circuit being used to measure it will reduce the measured potential.

As well, frequently, non standard conditions may be used in a lab.

The standard cells are for 1 M solutions. They are measured at 25 degrees Celsius. Differences in these conditions will cause changes. If a reactant or product is a gas, it needs to be bubbled over a platinum (inert) electrode with a pressure of 1 atm.

Other much more significant differences also impact. Unless the electrodes are super clean, with a fresh metal surface that has no oxide layer at all, then the oxide layer will interfere with the reaction and reduce the measure potential. The salt bridge can cause interference to the easy flow of ions, and so cause internal resistance and lower the measured potential. How much will depend on a lot of factors about how it is made etc.

If the connections within your circuit are not perfect, the measured potential will be less as well.

I am sure you are beginning to imagine now that there are many factors which are very difficult to get just right.

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