REPORT SHEET EXPERIMENT 22 Date Lab Section Name A. Reactions of copper, iron, z
ID: 481012 • Letter: R
Question
REPORT SHEET EXPERIMENT 22 Date Lab Section Name A. Reactions of copper, iron, zinc, and silver color change or ppt? cell A-1. copper(ID ion zinc metal net ionic reaction color change or ppt cell A-2. copper(ID ion silver metal net ionic reaction color change or ppt? Cell A-3. copper(ID ion iron metal net ionic reaction color change or ppt? Cell B-1. iron (III ion copper metal net ionic reaction color change or ppt? Cell B-2. iron(IID ion zinc metal net ionic reaction color change or ppt? Cell B-3, iron ion silver metal net ionic reaction color change or ppt? Cell C-1. zinc (ID ion copper metal net ionic reaction Cell C-2. zinc(ID ion iron metal color change or ppt? net ionic reaction Cell C-3, zinc (ID ion silver metal color change or ppt? net ionic reaction Cell D-1. silver(I) ion zinc metal color change or ppt? net ionic reaction Cell D-2. silver(Dion copper metal color change or ppt? net ionic reaction Cell D 3. silver(I) ion iron metal color change or ppt? net ionic reaction page 1Explanation / Answer
Every metal is associated with some reduction potential values which signifies how easily they can accept electron and reduce. If a metal ion reduces very easily, it will act as an oxiding agent for any metal with a lower value of reduction potential. In short , between metal A and B if A has a higher value of reduction potential than B, then A will oxidise B and will itself get reduced.
The reduction potential values of four metal Zn, Fe, Cu and Ag is as follows:
Zn ==> -0.76 V
Fe ==> -0.44 V
Cu ==> +0.34 V
Ag ==> +0.80V
Cell A1 ==> brown ppt Cu^2+ + Zn ---> Cu + Zn ^2+
Cell A2 ==> brown ppt Cu^2+ + Fe ---> Cu + Fe ^2+
Cell A3 ==> no reaction
Cell B1 ==> blue solution Cu + 2Fe^3+ --> 2Fe^2+ + Cu^2+
Cell B2 ==> yellow solution Zn + 2Fe^3+ ----> 2Fe^2+ + Zn ^2+
Cell B3 ==> No reaction
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