The commercial production of nitric acid involves the following chemical reactions: 4 NH 3 (g) + 5 O 2 (g) → 4 NO(g) + 6 H 2 O(g) 2 NO(g) + O 2 (g) → 2 NO 2 (g) 3 NO 2 (g) + H 2 O(l) → 2 HNO 3 (aq) + NO(g) (b) Identify the element undergoing oxidation and the element undergoing reduction.

Hey everyone today, we're being asked to identify the reducing and oxidizing agents in the reaction between carbon and sulfuric acid to form carbon dioxide, sulfur dioxide and water. So, to identify the oxidation or oxidizing and reducing agents, we need to find out which molecules are being oxidized and reduced before and after the reaction has taken place. So let's go ahead and take a look at the react inside. First we have carbon and two sulfuric acids, H two, S. 04. So we need to find the oxidation states for these molecules. And for the carbon, it's pretty easy. Carbon is most stable. It is in its natural state alone. As C And recalling our oxidation rules, we know that a stable state element will have an oxidation state of zero An oxidation state of zero for sulfuric acid. However, it's a little more difficult. Now the molecule we wanted or elements that we need to pay attention to is the sulfur because it can have different oxidation states depending on what it is bonded to. Now recall, this is again a neutral element, which means it must counteract the some of the oxidation states of the other elements bonded to it in order for it to be neutral, recalling our oxidation rules, We know that oxygen unless it's bonded in hydrogen peroxide or bonded to a flooring, will have a charge of negative two. And since we have four oxygen's, that makes it a total charge of -8. Similarly, when hydrogen is bonded to a non metal in a molecule, it will have a charge of plus one an oxidation state of plus one. And since we have to hide regions that makes us plus two, therefore the total charge or or some of oxidation states in the molecule is negative six, it is negative eight plus two. So to counteract this, sulfur must have the oxidation state of plus six. So sulfur in sulfuric acid Has an oxidation state of Plus six. Taking a look at the reactant. Now we have a carbon dioxide C. 02, two, sulfur dioxides as 02 And two water molecules. Let's take a look at the carbon again. We remember our oxidation rules that oxygen has an oxidation state of negative two. And since we have two of those that makes us negative four. So the carbon must have an oxidation state of plus four. So it means it goes from 0 to Plus four. And sulfur similarly is also bonded to two oxygen's. So this is negative four, which means it also goes to plus four, but now it goes down from plus six to plus four. So what does this mean? Well, carbon lost electrons. It lost electrons. Meanwhile sulfur gained electrons after the reaction. And if we remember our oxidation and reduction rules for oil rig, let me write this. Better oil rig oxidation is losing and reduction is gaining which means carbon was oxidized it lost electrons and sulfur was reduced. It gained electrons. Which means that carbon here got oxidized oxidized and sulfuric acid got reduced. And because of this we know that carbon is therefore the reducing agent because it aids the reduction of sulfuric acid reducing agent, and sulfuric acid is the oxidizing agent as it aids the oxidation of carbon. I hope this helps, and I look forward to seeing y'all in the next one.

Ch.4 - Reactions in Aqueous Solution

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Brown 14th Edition

Ch.4 - Reactions in Aqueous Solution

Problem 96b

Chapter 4, Problem 96b

The commercial production of nitric acid involves the following chemical reactions:
4 NH₃(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g)
2 NO(g) + O₂(g) → 2 NO₂(g)
3 NO₂(g) + H₂O(l) → 2 HNO₃(aq) + NO(g)
(b) Identify the element undergoing oxidation and the element undergoing reduction.

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Identify the oxidation states of nitrogen in NO2, HNO3, and NO.

In NO2, nitrogen has an oxidation state of +4.

In HNO3, nitrogen has an oxidation state of +5.

In NO, nitrogen has an oxidation state of +2.

Determine which element is oxidized and which is reduced by comparing the changes in oxidation states.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Oxidation and Reduction

Oxidation and reduction are chemical processes that involve the transfer of electrons between substances. Oxidation refers to the loss of electrons, resulting in an increase in oxidation state, while reduction involves the gain of electrons, leading to a decrease in oxidation state. These processes are often summarized by the mnemonic 'OIL RIG' (Oxidation Is Loss, Reduction Is Gain). Understanding these concepts is crucial for identifying which elements are oxidized and reduced in a reaction.

Oxidation States

Oxidation states (or oxidation numbers) are a way to keep track of electron transfer in chemical reactions. Each element in a compound is assigned an oxidation state based on its electron configuration and bonding. In the context of redox reactions, changes in oxidation states help identify which elements are oxidized and reduced. For example, in the reaction provided, determining the oxidation states of nitrogen in NO2 and HNO3 is essential for identifying the changes occurring during the reaction.

Balancing Redox Reactions

Balancing redox reactions involves ensuring that the number of electrons lost in oxidation equals the number of electrons gained in reduction. This process often requires separating the reaction into half-reactions for oxidation and reduction, balancing them individually, and then combining them to form a balanced overall equation. This is important for accurately representing the stoichiometry of the reaction and understanding the conservation of mass and charge in chemical processes.