Reacting oxygen with white phosphorus can form either P4 O6 or P4 O10. State the conditions that

Name: Problem 59, Chapter 24: Chemistry A Molecular Approach
Uploaded: 2020-02-11T02:38:28-08:00
Duration: 42 s
Channel: Amy Jiang
Description: Reacting oxygen with white phosphorus can form either P4 O6 or P4 O10. State the conditions that determine which product forms.

step 1 So for this question, we're asked, reacting oxygen with white phosphorus can form either P4 .06

Question

Reacting oxygen with white phosphorus can form either $\mathrm{P}_{4} \mathrm{O}_{6}$ or $\mathrm{P}_{4} \mathrm{O}_{10}$. State the conditions that determine which product forms.

   Reacting oxygen with white phosphorus can form either $\mathrm{P}_{4} \mathrm{O}_{6}$ or $\mathrm{P}_{4} \mathrm{O}_{10}$. State the conditions that determine which product forms.

Chemistry A Molecular Approach

Nivaldo J. Tro 5th Edition

Chapter 24, Problem 59

Instant Answer

Solved by Expert Amy Jiang

02/11/2020

Step 1

The reactants are oxygen ($\mathrm{O}_2$) and white phosphorus ($\mathrm{P}_4$). The possible products are $\mathrm{P}_4\mathrm{O}_6$ and $\mathrm{P}_4\mathrm{O}_{10}$. Show more…

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Reacting oxygen with white phosphorus can form either $\mathrm{P}_{4} \mathrm{O}_{6}$ or $\mathrm{P}_{4} \mathrm{O}_{10}$. State the conditions that determine which product forms.

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Key Concepts

Reaction Stoichiometry

This concept involves understanding how the molar ratios of reactants control the extent of a reaction. In oxidation reactions, the proportion of oxygen to the substance being oxidized determines whether the oxidation is partial or complete. When the oxygen supply is limited relative to the reactive species, the reaction proceeds only partially, leading to a lower oxidation state, while an excess of oxygen leads to full oxidation and a higher oxidation state.

Controlled Oxidation Conditions

Controlled oxidation refers to the deliberate adjustment of reaction conditions such as the availability of oxygen, temperature, and pressure to direct the reaction toward a desired product. By limiting oxygen, one can achieve partial oxidation, resulting in a less oxidized product, whereas providing an excess of oxygen results in complete oxidation. This control is crucial in synthesizing specific compounds with targeted chemical properties.

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