Consider the following reaction: Zn (s) + Cu 2+ (aq) ? Zn 2+ (aq) + Cu (s) Which Statement is true? Zn is the reducing agent Zn is reduced Cu2+ is oxidized Cu2+ is the reducing agent Cu is oxidized
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This means zinc is losing electrons and is acting as the reducing agent. ** Show more…
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Transcript
Hello, so let's answer now the question. So we have here a redox equation. So we have here a zinc in solid form, plus we have a copper ion, okay, a copper in equious solution, and the reaction will yield zinc in aqueous solution plus copper in solid form. Now, which of the following here is true? Take note that when we speak of oxidation number decreased, if the oxidation number decreased, then that is reduction. If the oxidation number increased, then that is oxidation. And take note that the reducing agent is oxidized during the reaction by losing electron. And on the other hand, the oxidizing agent becomes reduced or becomes reduced by accepting electron. So here in the reaction, zinc is oxidized. So zinc is oxidized. It is oxidized because it loses electron. The oxidation number of zinc in solid form is zero. Then it becomes positive 2. Therefore, it loses two electrons. And the copper, ions here in aqueous solution is reduced since the number of the oxidation is positive 2 it gains electron or it gains 2 electron that's why here the oxidation number becomes 0 so from positive 2 to 0 so the copper ions gain…
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