a. The apparatus below was used to plate a strip of metal with copper. One electrode was made of copper and the other was the metal strip to be plated.
i . Which electrode, X or Y, is the metal strip?
ii . Is the metal strip an anode or a cathode?
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Reaction of zinc metal in copper sulfate solution.
The process that occurs in this redox reaction is shown below as two separate half-reactions, which can then be combined into the full redox reaction.
& text{Oxidation}: quad quad text{Zn}(s) rightarrow text{Zn}^{2+} (aq) + 2e^- \& underline{text{Reduction}: quad quad text{Cu}^{2+}(aq) + 2e^- rightarrow text{Cu}(s) qquad qquad qquad }\&text{Full Reaction}: quad text{Zn}(s) + text{Cu}^{2+}(aq) rightarrow text{Zn}^{2+}(aq) + text{Cu}(s)
Why does this reaction occur spontaneously? The activity series is a listing of elements in descending order of reactivity. An element that is higher in the activity series is capable of displacing an element that is lower on the series in a single-replacement reaction. This series also lists elements in order of ease of oxidation. The elements at the top are the easiest to oxidize, while those at the bottom are the most difficult to oxidize. The Table below shows the activity series together with each element’s oxidation half-reaction .
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