A gas mixture contains O2, N2, and Ar at partial pressures of 125,175 , and 225 mm Hg , respect

Name: Problem 37, Chapter 7: General, Organic, and Biological Chemistry
Uploaded: 2021-04-05T08:09:20-08:00
Duration: 1 min 19 s
Channel: Shazia Naz
Description: A gas mixture contains O2, N2, and Ar at partial pressures of 125,175 , and 225 mm Hg , respectively. If CO2 gas is added to the mixture until the total pressure reaches 623 mm Hg , what is the partial pressure, in millimeters of mercury, of CO2 ?

step 1 solution for the given question here we have to determine the partial pressure from Dalton laws

Question

A gas mixture contains $\mathrm{O}_2, \mathrm{~N}_2$, and Ar at partial pressures of 125,175 , and 225 mm Hg , respectively. If $\mathrm{CO}_2$ gas is added to the mixture until the total pressure reaches 623 mm Hg , what is the partial pressure, in millimeters of mercury, of $\mathrm{CO}_2$ ?

   A gas mixture contains $\mathrm{O}_2, \mathrm{~N}_2$, and Ar at partial pressures of 125,175 , and 225 mm Hg , respectively. If $\mathrm{CO}_2$ gas is added to the mixture until the total pressure reaches 623 mm Hg , what is the partial pressure, in millimeters of mercury, of $\mathrm{CO}_2$ ?

General, Organic, and Biological Chemistry

H. Stephen Stoker 5th Edition

Chapter 7, Problem 37

Instant Answer

Solved by Expert Shazia Naz

04/05/2021

Step 1

The total pressure is the sum of the partial pressures of the individual gases. \[ P_{\text{total initial}} = P_{\mathrm{O}_2} + P_{\mathrm{N}_2} + P_{\mathrm{Ar}} = 125 \, \text{mm Hg} + 175 \, \text{mm Hg} + 225 \, \text{mm Hg} \] Show more…

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A gas mixture contains $\mathrm{O}_2, \mathrm{~N}_2$, and Ar at partial pressures of 125,175 , and 225 mm Hg , respectively. If $\mathrm{CO}_2$ gas is added to the mixture until the total pressure reaches 623 mm Hg , what is the partial pressure, in millimeters of mercury, of $\mathrm{CO}_2$ ?

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Key Concepts

Partial Pressure

Partial pressure refers to the pressure exerted by an individual gas in a mixture. In problem-solving, the partial pressure can be calculated by subtracting the combined pressures of the existing gases from the total pressure, which is a direct application of Dalton's Law.

Dalton's Law of Partial Pressures

This law states that in a mixture of non-reacting gases, the total pressure is equal to the sum of the pressures that would be exerted by each gas if it occupied the container alone. It is fundamental in calculating the contribution of each gas to the overall pressure, especially when additional gases are introduced.

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