(a) Define oxidation in terms of electron transfer. (b) Consider the following: Cu\(_{(s)}\) + 2Ag\(^{+}_{(Ag)}\)...
CHEMISTRY
WAEC 1994
(a) Define oxidation in terms of electron transfer.
(b) Consider the following: Cu\(_{(s)}\) + 2Ag\(^{+}_{(Ag)}\) \(\to\) Cu\(^{2+}_{(aq)}\) + 2Ag\(_{(s)}\)
(i) State the species that is reduced
(ii) Write half-cell equation for each of the species.
Explanation
(a) Oxidation is defined as the loss or removal of electron.
(b)(i) The species that is reduced is Ag\(^+\)
(ii) Cu \(\rightleftharpoons\) Cu\(^{2+}\) + 2e\(^-\)
2Ag\(^+\) + 2e\(^-\) \(\rightleftharpoons\) 2Ag
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