Determine which of the following are oxidation-reduction...

Determine which of the following are oxidation-reduction reactions. For those that are, identify the oxidizing and reducing agents. (a) $\mathrm{HgCl}_{2}(\mathrm{aq})+2 \mathrm{KI}(\mathrm{aq}) \longrightarrow \mathrm{HgI}_{2}(\mathrm{~s})+2 \mathrm{KCl}(\mathrm{aq})$ (b) $4 \mathrm{NH}_{3}(\mathrm{~g})+3 \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{~N}_{2}(\mathrm{~g})+6 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})$ (c) $\mathrm{CaCO}_{3}(\mathrm{~s})+2 \mathrm{HNO}_{3}(\mathrm{aq}) \longrightarrow \mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})$ $+\mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\ell)$ (d) $\mathrm{PCl}_{3}(\ell)+3 \mathrm{H}_{2} \mathrm{O}(\ell) \longrightarrow 3 \mathrm{HCl}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{PO}_{3}(\mathrm{aq})$

Determine which of the following are oxidation-reduction reactions. For those that are, identify the oxidizing and reducing agents.
(a) $\mathrm{HgCl}_{2}(\mathrm{aq})+2 \mathrm{KI}(\mathrm{aq}) \longrightarrow \mathrm{HgI}_{2}(\mathrm{~s})+2 \mathrm{KCl}(\mathrm{aq})$
(b) $4 \mathrm{NH}_{3}(\mathrm{~g})+3 \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{~N}_{2}(\mathrm{~g})+6 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})$
(c) $\mathrm{CaCO}_{3}(\mathrm{~s})+2 \mathrm{HNO}_{3}(\mathrm{aq}) \longrightarrow \mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})$
$+\mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\ell)$
(d) $\mathrm{PCl}_{3}(\ell)+3 \mathrm{H}_{2} \mathrm{O}(\ell) \longrightarrow 3 \mathrm{HCl}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{PO}_{3}(\mathrm{aq})$

Key Concepts

Reducing Agent

A reducing agent is the substance that donates electrons in a redox reaction, undergoing oxidation in the process. It causes the reduction of another species by losing electrons.

Oxidizing Agent

An oxidizing agent is the substance that accepts electrons during a redox reaction, becoming reduced in the process. It drives the oxidation of another species by taking electrons from it.

Oxidation?Reduction Reaction

A redox reaction is a chemical reaction in which electrons are transferred between reactants, causing changes in their oxidation states. In these reactions, one species is oxidized (loses electrons) and another is reduced (gains electrons), making it possible to identify electron donors and acceptors.

Oxidation State

The oxidation state is an assigned value that reflects the degree of oxidation of an atom in a compound. By comparing the oxidation states of atoms before and after a reaction, one can determine if a redox process has occurred.

Transcript

00:01 Hi, in this problem, we are given some of the chemical reactions.

00:06 We have to identify the reactions which are oxidation reduction reactions.

00:11 And for those oxidation reduction reactions, we need to identify the oxidizing agent and the reducing agent.

00:17 So oxidation reaction is that reaction where there is an increase in oxidation number of the species, while the reduction reaction involves the decrease in the oxidation number of oxidation state of the species.

00:30 So we will be using the concept of oxidation states here to identify whether the reaction is oxidation reduction or not.

00:37 The first reaction is this.

00:40 In this reaction, first we will write the oxidation states of all the species involved.

00:46 Chlorine has minus 1, oxidation state, mercury has plus 2.

00:50 In this, minus 1 for iodine plus 1 for potassium.

00:55 Then here, minus 1 for iodine, mercury has plus 2 oxidation state.

00:59 And potassium has oxidation state of plus one, chlorine has oxidation state of minus one.

01:07 Now here we can very clearly see that none of the species has changed its oxidation state, that is oxidation states of all the species are same in the reactant as well as in the product.

01:20 So this reaction is not oxidation reduction reaction.

01:37 And so there will be no oxidizing as well as reducing agent in the reaction.

01:43 Then we have the second reaction where if we write the oxidation states plus one for hydrogen minus three for nitrogen here, zero for oxygen, zero for nitrogen, minus two for oxygen and plus one for hydrogen...

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