EXPERIMENT 8 Oxidation-Reduction Reactions Part I-A Qualitative Redox Table for

Question

EXPERIMENT 8 Oxidation-Reduction Reactions Part I-A Qualitative Redox Table for Copper, Zinc, Iron, and Their lons 1. Write net ionic equations for any reactions taking place between the metals and metal ions listed below. If there is no visible evidence of reaction, write NR for "no reaction." Copper and zinc ion: Zinc and copper(II) ion: Iron and copper(II) ion: Iron and zinc ion: Copper and iron(II) ion: Zinc and iron(II) ion: 2. Which metal is the stronger reducing agent: Copper or zinc? a. b. Iron or copper? c. Iron or zinc? In the box at the right, construct a redox couple table for iron, copper, zinc, and their ions. Arrange the three metals in a column at the right-hand side, with the 3. · strongest reducing agent at the bottom and the weakest at the top. To the left of each metal symbol, make a slash; to the left of the slash, write the symbol for the oxidized form of the metal, for example, Cu2"/Cu. You now have a brief redox couple table. 105

Explanation / Answer

Ans 1 :

As a general rule the ions that have more negative standard electrode potentials than the other ions , can replace (reduce) them from their solutions , as they tend to be more stable in their oxidised form.

So here :

copper and zinc (II) ion : NR

zinc and copper (II) ion : Zn + Cu2+ = Zn2+ + Cu

Iron and copper (II) ion : Fe + Cu2+ = Fe2+ + Cu

Iron and zinc ion : NR

Copper and Iron (II) ion : NR

Zinc and Iron (II) ion : Zn + Fe2+ = Zn2+ + Fe

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