The following diagram depicts a gaseous mixture of O2 (red spheres), N2 (blue spheres), and Cl2

Name: Problem 40, Chapter 7: General, Organic, and Biological Chemistry
Uploaded: 2021-03-07T20:54:32-08:00
Duration: 3 min 19 s
Channel: Ivan Kochetkov
Description: The following diagram depicts a gaseous mixture of O2 (red spheres), N2 (blue spheres), and Cl2 (yellow spheres). Assuming that the gases do not react with each other, what is the total pressure, in atm, in the container if the partial pressure of the O2 gas is 2.0 atm ?

step 1 Hello, here we have to calculate the pressure in the vessel to which oxygen and nitrogen were ad

Question

The following diagram depicts a gaseous mixture of $\mathrm{O}_2$ (red spheres), $\mathrm{N}_2$ (blue spheres), and $\mathrm{Cl}_2$ (yellow spheres). Assuming that the gases do not react with each other, what is the total pressure, in atm, in the container if the partial pressure of the $\mathrm{O}_2$ gas is 2.0 atm ?

   The following diagram depicts a gaseous mixture of $\mathrm{O}_2$ (red spheres), $\mathrm{N}_2$ (blue spheres), and $\mathrm{Cl}_2$ (yellow spheres).
Assuming that the gases do not react with each other, what is the total pressure, in atm, in the container if the partial pressure of the $\mathrm{O}_2$ gas is 2.0 atm ?

General, Organic, and Biological Chemistry

H. Stephen Stoker 5th Edition

Chapter 7, Problem 40

Instant Answer

Solved by Expert Ivan Kochetkov

03/07/2021

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The following diagram depicts a gaseous mixture of $\mathrm{O}_2$ (red spheres), $\mathrm{N}_2$ (blue spheres), and $\mathrm{Cl}_2$ (yellow spheres). Assuming that the gases do not react with each other, what is the total pressure, in atm, in the container if the partial pressure of the $\mathrm{O}_2$ gas is 2.0 atm ?

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Key Concepts

Dalton's Law of Partial Pressures

This principle states that the total pressure in a container holding a mixture of non-reacting gases is equal to the sum of the partial pressures of the individual gases. It provides a framework for analyzing how each gas contributes to the overall pressure.

Partial Pressure

Partial pressure refers to the pressure that one gas in a mixture would exert if it occupied the entire volume by itself at the same temperature. It is a key concept for understanding how the individual amounts of gases contribute to the total pressure.

Mole Fraction in Gas Mixtures

The mole fraction is the ratio of the number of moles of a particular gas to the total number of moles in the mixture. Since partial pressure is proportional to the mole fraction of a gas in a mixture, understanding this concept is essential for determining each gas’s contribution to the overall pressure.

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