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Chapter 4: Problem 53

On the basis of oxidation number considerations, one of the following oxides would not react with molecular oxygen: \(\mathrm{NO}, \mathrm{N}_{2} \mathrm{O}, \mathrm{SO}_{2}, \mathrm{SO}_{3}, \mathrm{P}_{4} \mathrm{O}_{6}\) Which one is it? Why?

Short Answer

Expert verified
The oxide that would not react with molecular oxygen is \(\mathrm{SO}_{3}\) because sulfur in this compound is already in its highest oxidation state (+6), thus it cannot be further oxidized.

Step by step solution

01

Recall the Oxidation Numbers

An oxidation number is a measure of the degree of oxidation of an atom in a substance. For example, the oxidations states for nitrogen can range from -3 to +5, sulfur from -2 to +6 and phosphorus from -3 to +5.
02

Apply the Oxidation Numbers

Let's take a look at the given substances: \(\mathrm{NO}\) has nitrogen at +2, \(\mathrm{N}_{2} \mathrm{O}\) has nitrogen at +1, \(\mathrm{SO}_{2}\) has sulfur at +4, \(\mathrm{SO}_{3}\) has sulfur at +6 and \(\mathrm{P}_{4}\mathrm{O}_{6}\) has phosphorus at +3.
03

Determine the Highest Oxidation State

Among the substances given, sulfur in \(\mathrm{SO}_{3}\) is already at its highest oxidation state of +6. This means that it cannot be further oxidized by molecular oxygen.

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Most popular questions from this chapter

Chemical tests of four metals \(\mathrm{A}, \mathrm{B}, \mathrm{C},\) and \(\mathrm{D}\) show the following results. (a) Only \(\mathrm{B}\) and \(\mathrm{C}\) react with \(0.5 \mathrm{M} \mathrm{HCl}\) to give \(\mathrm{H}_{2}\) gas. (b) When \(\mathrm{B}\) is added to a solution containing the ions of the other metals, metallic \(\mathrm{A}, \mathrm{C},\) and \(\mathrm{D}\) are formed. (c) A reacts with \(6 M \mathrm{HNO}_{3}\) but \(\mathrm{D}\) does not. Arrange the metals in the increasing order as reducing agents. Suggest four metals that fit these descriptions.

What are the similarities and differences between acid-base titrations and redox titrations?

You have \(505 \mathrm{~mL}\) of a \(0.125 \mathrm{M} \mathrm{HCl}\) solution and you want to dilute it to exactly \(0.100 \mathrm{M}\). How much water should you add? Assume volumes are additive.

A 22.02-mL solution containing \(1.615 \mathrm{~g} \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\) is mixed with a 28.64-mL solution containing \(1.073 \mathrm{~g}\) \(\mathrm{NaOH}\). Calculate the concentrations of the ions remaining in solution after the reaction is complete. Assume volumes are additive.

Phosphoric acid \(\left(\mathrm{H}_{3} \mathrm{PO}_{4}\right)\) is an important industrial chemical used in fertilizers, in detergents, and in the food industry. It is produced by two different methods. In the electric furnace method, elemental phosphorus \(\left(\mathrm{P}_{4}\right)\) is burned in air to form \(\mathrm{P}_{4} \mathrm{O}_{10},\) which is then reacted with water to give \(\mathrm{H}_{3} \mathrm{PO}_{4} .\) In the wet process, the mineral phosphate rock fluorapatite \(\left[\mathrm{Ca}_{5}\left(\mathrm{PO}_{4}\right)_{3} \mathrm{~F}\right]\) is reacted with sulfuric acid to give \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (and \(\mathrm{HF}\) and \(\mathrm{CaSO}_{4}\) ). Write equations for these processes and classify each step as precipitation, acid-base, or redox reaction.
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