The Ostwald process for the commercial production of nitric...

The Ostwald process for the commercial production of nitric acid involves the following three steps: $$4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)$$ $$2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)$$ $$3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{HNO}_{3}(a q)+\mathrm{NO}(g)$$ a. Which reactions in the Ostwald process are oxidation–reduction reactions? b. Identify each oxidizing agent and reducing agent.

The Ostwald process for the commercial production of nitric acid involves the following three steps:
$$4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)$$
$$2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)$$
$$3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{HNO}_{3}(a q)+\mathrm{NO}(g)$$
a. Which reactions in the Ostwald process are oxidation–reduction reactions?
b. Identify each oxidizing agent and reducing agent.

Key Concepts

Disproportionation Reaction

A disproportionation reaction is a special type of redox reaction in which a single substance undergoes both oxidation and reduction simultaneously. This concept is important when dealing with reactions where the same species is transformed into two different products with different oxidation states, illustrating the concurrent electron donation and acceptance within a single reaction.

Reducing Agent

A reducing agent is a substance that donates electrons, thereby causing another substance to be reduced as it itself becomes oxidized. Recognizing reducing agents is fundamental when analyzing redox reactions, as it clarifies which reactant is responsible for the electron donation, making it crucial for understanding reaction mechanisms.

Oxidation–Reduction (Redox) Reactions

Redox reactions are chemical processes in which electrons are transferred between species, causing changes in their oxidation states. A thorough understanding of these reactions involves tracking the flow of electrons and determining which species are oxidized (lose electrons) and which are reduced (gain electrons). These concepts are essential for analyzing and balancing reactions in both laboratory and industrial settings.

Oxidizing Agent

An oxidizing agent is a substance that facilitates oxidation by accepting electrons from another species, causing that species to be oxidized while the oxidizing agent itself is reduced. This concept is critical in redox chemistry because it helps determine the direction of electron transfer and the roles of various reactants in industrial processes.

Transcript

00:01 Ok, so we have three different reactions.

00:02 We're trying to figure out which ones are oxidation reductions, which means we're going to be required to label the oxidation numbers on each of them.

00:11 So here is our first equation, and then our second equation.

00:18 And the coefficients really don't matter for labeling oxidation numbers, so i don't really need to be keeping track of that.

00:24 And then here's your third one.

00:28 And states of matter aren't going to affect this either.

00:34 So labeling oxidation numbers, any element by itself always gets zero.

00:38 Then when you start looking inside of compounds, h's will get plus ones, and oxygen's will get minus two.

00:45 So i'll go around and add those to each compound.

00:54 So that covers most of it.

00:55 After that, we start doing a little bit of math to try to figure out what's missing.

00:59 So like in the ammonia, if there's three plus ones, that means the nitrogen must be minus three to balance it.

01:05 In the no, the nitrogen must be plus two to balance that out.

01:09 Down here, same thing, plus two.

01:11 And for the no2, that's going to be plus four.

01:14 And again, we've got plus four for that n.

01:17 When we get over to the other side, it's going to be a plus five and a plus two.

01:23 So when it says, which ones are oxidation reduction reactions, if you can see only two things changing oxidation number, then you're an oxidation reduction reaction.

01:31 So in this first one, n and o are changing oxidation state...

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