New Observations on the Copper-to-Silver-to-Gold Demonstration

Dorin Bejan , Jeff Hastie and Nigel J. Bunce
Department of Chemistry, University of Guelph, Guelph, Ontario N1G 2W1, Canada
J. Chem. Educ., 2008, 85 (10), p 1381
DOI: 10.1021/ed085p1381.2
Publication Date (Web): October 1, 2008
History, Education, and Documentation

Abstract

The demonstration in which a copper penny is converted first to "silver" and then to "gold" involves, as the first step, the deposition of zinc onto copper in hot NaOH solution. The reaction involves an electrochemical cell, with the deposition of zinc in the form of a surface layer of the silver-colored alloy γ-brass, accompanied by evolution of hydrogen at the copper cathode. The cathode potential falls progressively for a series of cells having Zn anode and cathodes varying in composition from Cu to brasses with Cu content down to less than 55% Cu, but H2 production is an independent process which appears to be unaffected. The silvery deposit can also be obtained conveniently by electrolytic deposition from a cell comprising zinc anode, copper cathode, and an electrolyte containing millimolar concentrations of both zinc sulfate and sodium sulfate.

Keywords (Audience):

High School / Introductory Chemistry

Keywords (Domain):

Demonstrations

Keywords (Feature):

JCE DigiDemos: Extensions

Keywords (Pedagogy):

Inquiry-Based / Discovery Learning

Keywords (Subject):

Copper
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  • Received: August 03, 2009

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