Questions: Identify the reactant that is oxidized in the following reaction: Cu(s) + 2 Ag^+(aq) -> Cu^2+(aq) + 2 Ag(s) View Available Hint(s) Ag(s) Ag^+(aq) Cu(s) Cu^2+(aq)

Transcript text: Identify the reactant that is oxidized in the following reaction: \[ \mathrm{Cu}(s)+2 \mathrm{Ag}^{+}(a q) \rightarrow \mathrm{Cu}^{2+}(a q)+2 \mathrm{Ag}(s) \] View Available Hint(s) $\mathrm{Ag}(s)$ $\mathrm{Ag}^{+}(a q)$ $\mathrm{Cu}(\mathrm{s})$ $\mathrm{Cu}^{2+}(a q)$

Solution

Solution Steps

Step 1: Identify the Oxidation States of Reactants and Products

First, we need to determine the oxidation states of the elements in the reactants and products.

For $\mathrm{Cu}(s)$, the oxidation state is 0.
For $\mathrm{Ag}^{+}(aq)$, the oxidation state is +1.
For $\mathrm{Cu}^{2+}(aq)$, the oxidation state is +2.
For $\mathrm{Ag}(s)$, the oxidation state is 0.

Step 2: Determine the Changes in Oxidation States

Next, we compare the oxidation states of each element before and after the reaction to see which element is oxidized (loses electrons) and which is reduced (gains electrons).

$\mathrm{Cu}(s)$ changes from 0 to +2, indicating it loses 2 electrons.
$\mathrm{Ag}^{+}(aq)$ changes from +1 to 0, indicating it gains 1 electron.

Step 3: Identify the Oxidized Reactant

Oxidation involves the loss of electrons. Since $\mathrm{Cu}(s)$ loses electrons (its oxidation state increases from 0 to +2), it is the reactant that is oxidized.

Final Answer

$\boxed{\mathrm{Cu}(s)}$

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