Given your results in Part A and B, it is possible to construct an activity seri

Question

Given your results in Part A and B, it is possible to construct an activity series for the four metals. An activity series sorts metals by the strength they display as reducing agents, with the strongest reducing agent( whose ion is the weakest oxidizing agent) at the top of the series. To help place the metals in the right order, consider the following. Which metal is always the anode? That is the strongest reducing agent. Which is never the anode? That is the weakest reducing agent. Sort the other two metals into your activity series, and list all four metals in order. Now find the standard reduction potential for each metal’s reaction. Remember that iron (III) is given above. How do the standard reduction potentials relate to your activity series?

Here is my answer, is this right? Cell potentials are

Zn>Fe>Cu>Ag

-.76, -.036, .34, .80

Explanation / Answer

Zn is always anode. Zn is strongest reducing agent.

Ag+ acts as always cathode. but not as anode. SO, Ag is weakest reducing agent.

SO, the correct order of reducing ability of the given four elements is,

Zn > Fe > Cu > Ag

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