Chemistry, 05.07.2019 09:00 aj12381

Determine the oxidizing agent in the following reaction. ni(s) + 2 agclo4(aq) → ni(clo4)2(aq) + 2 ag(s)

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Answer from: hollandhogenson

The oxidizing agent in the reaction is silver perchlorate.

Given:

A chemical reaction between nickel and silver perchlorate:

$Ni(s) + 2 AgClO_4(aq) \rightarrow Ni(ClO_4)_2(aq) + 2 Ag(s)$

To find:

The oxidizing agent in the reaction.

Solution:

$Ni(s) + 2 AgClO_4(aq) \rightarrow Ni(ClO_4)_2(aq) + 2 Ag(s)$

The oxidation state of nickel in nickel metal = 0The oxidation state of nickel in nickel perchlorate = +2

The oxidation state of nickel changing from 0 to +2 which means that it had undergone an oxidation reaction.

The oxidation state of silver in silver perchlorate = +1The oxidation state of silver in silver metal = 0

The oxidation state of silver changing from +1 to 0 which means that it had undergone a reduction reaction.

The substance here undergoing reduction and oxidizing the other is a silver ion, hence, silver perchlorate is an oxidizing agent.The substance here undergoing oxidation and reducing the other is nickel, hence, nickel metal is a reducing agent.

The oxidizing agent in the reaction is silver perchlorate.

Learn more about an oxidizing agent and a reducing agent here:

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Answer from: dej33

Silver perchlorate $\text{AgClO}_4$ serves as the oxidizing agent in this reaction.

Explanation

Both silver perchlorate $\text{AgClO}_4$ in the reactants and nickel (II) perchlorate $\text{Ni}(\text{ClO}_4)_2$ in the products exists as ionic salt dissolved in an aqueous solution. Rewriting the chemical equation as an ionic one might help eliminate spectator ions and make changes in oxidation states more apparent.

Ionic equation:

$\text{Ni} \; (s) + 2 \; \text{Ag}^{+} \; (aq) + 2\; \text{ClO}_4 \; (aq) \to \text{Ni}^{2+} \; (aq) + 2\; \text{ClO}_4^{-} \; (aq) + 2 \; \text{Ag} \; (aq)$

Two perchlorate ions are present on both sides of the equation. These ions act as spectator ions that take no part in the overall reaction. Thus it is possible to determine the oxidizing and reducing agent without knowing the oxidation state of atoms in the perchlorate ion. Marking oxidation states on top of each element gives the following equation:

$\stackrel{0}{\text{Ni}} \; (s) + 2 \; \stackrel{+1}{\text{Ag}^{+}} \; (aq)\to \stackrel{+2}{\text{Ni}^{2+}} \; (aq) + 2 \; \stackrel{0}{\text{Ag}} \; (aq)$

There is a decrease in the oxidation state of silver, from +1 to 0. Silver atoms, therefore, gain electrons and are reduced. The reactant containing silver ions, silver perchlorate, thus acts as the oxidation agent of this reaction.

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Determine the oxidizing agent in the following reaction. ni(s) + 2 agclo4(aq) → ni(clo4)2(aq) + 2 ag...

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