A gas mixture with a total pressure of 755 mmHg contains each of the following gases at the indi

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

A gas mixture with a total pressure of 755 mmHg contains...

A gas mixture with a total pressure of $755 \mathrm{mmHg}$ contains each of the following gases at the indicated partial pressures: $\mathrm{CO}_{2}, 255$ $\mathrm{mmHg}_{\text {i }}$ Ar, $124 \mathrm{mmHg}$; and $\mathrm{O}_{2}, 167 \mathrm{mmHg}$. The mixture also contains helium gas. What is the partial pressure of the helium gas? What mass of helium gas is present in a $10.0$ -L sample of this mixture at $273 \mathrm{~K} ?$

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Dalton's Law of Partial Pressures

This law states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases. This concept is essential because it allows the calculation of an unknown gas pressure in a mixture by subtracting the known partial pressures from the total system pressure.

Ideal Gas Law

The ideal gas law, expressed as PV = nRT, relates the pressure, volume, temperature, and number of moles of a gas. It is crucial in this context for determining the number of moles of a gas present in a given volume and temperature, which can subsequently be used for mass calculations.

Molar Mass Conversion

Once the number of moles of a gas is known, converting this value to a mass requires the use of the gas's molar mass. This step links the microscopic amount of substance (moles) to a measurable macroscopic quantity (mass), facilitating practical applications and quantitative analysis in chemistry.

Transcript

Please give Ace some feedback