A gas mixture with a total pressure of 745 mmHg contains each of the following gases at the indi

Name: Problem 62, Chapter 5: Chemistry A Molecular Approach
Uploaded: 2021-08-15T20:17:43-08:00
Duration: 2 min 36 s
Channel: Nicole Mabante
Description: A gas mixture with a total pressure of 745 mmHg contains each of the following gases at the indicated partial pressures: CO2, 125 mmHg ; Ar, 214 mmHg; and O2, 187 mmHg. The mixture also contains helium gas. What is the partial pressure of the helium gas? What mass of helium gas is present in a 12.0 L sample of this mixture at 273 K ?

step 1 Okay, so if the total pressure is 745 millimeters of mercury, that means that this pressure is g

Question

A gas mixture with a total pressure of $745 \mathrm{mmHg}$ contains each of the following gases at the indicated partial pressures: $\mathrm{CO}_{2}$, $125 \mathrm{mmHg} ;$ Ar, $214 \mathrm{mmHg}$; and $\mathrm{O}_{2}, 187 \mathrm{mmHg}$. The mixture also contains helium gas. What is the partial pressure of the helium gas? What mass of helium gas is present in a $12.0 \mathrm{~L}$ sample of this mixture at $273 \mathrm{~K}$ ?

   A gas mixture with a total pressure of $745 \mathrm{mmHg}$ contains each of the following gases at the indicated partial pressures: $\mathrm{CO}_{2}$, $125 \mathrm{mmHg} ;$ Ar, $214 \mathrm{mmHg}$; and $\mathrm{O}_{2}, 187 \mathrm{mmHg}$. The mixture
also contains helium gas. What is the partial pressure of the helium gas? What mass of helium gas is present in a $12.0 \mathrm{~L}$ sample of this mixture at $273 \mathrm{~K}$ ?

Chemistry A Molecular Approach

Nivaldo J. Tro 3rd Edition

Chapter 5, Problem 62

Instant Answer

Solved by Expert Nicole Mabante

08/15/2021

Step 1

This is the sum of the partial pressures of all the gases in the mixture. We are given the partial pressures of CO$_2$, Ar, and O$_2$ as 125 mmHg, 214 mmHg, and 187 mmHg respectively. We can find the partial pressure of helium (P$_{He}$) by subtracting the sum of Show more…

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A gas mixture with a total pressure of $745 \mathrm{mmHg}$ contains each of the following gases at the indicated partial pressures: $\mathrm{CO}_{2}$, $125 \mathrm{mmHg} ;$ Ar, $214 \mathrm{mmHg}$; and $\mathrm{O}_{2}, 187 \mathrm{mmHg}$. The mixture also contains helium gas. What is the partial pressure of the helium gas? What mass of helium gas is present in a $12.0 \mathrm{~L}$ sample of this mixture at $273 \mathrm{~K}$ ?

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Key Concepts

Dalton's Law of Partial Pressures

This principle states that in a mixture of non-reacting gases, the total pressure is equal to the sum of the individual partial pressures of each gas. Understanding this concept allows one to calculate the partial pressure of an unknown component by subtracting the known partial pressures from the total pressure.

Ideal Gas Law

This law, expressed as PV = nRT, relates the pressure, volume, temperature, and number of moles of an ideal gas. It is fundamental for calculating the amount of substance present in a gas sample when its pressure, volume, and temperature are known, which in turn helps to determine the mass of the gas using its molar mass.

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