I have a question on redox reactions. When given certain metals for a redox reaction, how...

I have a question on redox reactions. When given certain metals for a redox reaction, how do I decide which element is reduced and which is oxidized? For example, one question I was given was: Write the balanced redox equation for the reaction between copper sulfate and zinc sulfate. How would I decide which is the oxidized metal and which is the reduced metal in this type of problem? I can identify the metals oxidized and reduced in a given equation, but have trouble producing the equation if given only the metals.

Expert Solution

Oxidation-reduction

When in a given equation, the metal which gets oxidized would have standard reduction potential value lower than the metal which gets reduced. This is according to the arrangement of metals in an electrochemical series. Higher the standard reduction potential value of the metal is, stronger it is as an oxidizing agent, that is it acts as oxidizing agent while itself getting reduced in the process. Similarly, Lower the standard reduction potential value of the metal is, stronger it is as an reducing agent, that is it acts as reducing agent while itself getting oxidized in the process. So by looking at the electrochemical series one can easily identify which metal gets oxidizied and which gets reduced easily.

queen_honey_blossom answered 2 years ago

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