A gas mixture for use in some lasers contains 5.00% by weight HCl, 1.00 % H2 and 94% Ne. The mix

step 1 This problem gives us a gas mixture at certain volume, certain pressure, and certain temperature

A gas mixture for use in some lasers contains 5.00% by...

A gas mixture for use in some lasers contains 5.00$\%$ by weight $\mathrm{HCl}, 1.00 \% \mathrm{H}_{2}$ and 94$\%$ Ne. The mixture is sold in cylinders that have a volume of 49.0 $\mathrm{L}$ and a pressure of $13,800 \mathrm{kPa}$ at $21.0^{\circ} \mathrm{C} .$ What is the partial pressure in kilo pascals of each gas in the mixture?

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 individual gases. It allows one to calculate the pressure contributed by each gas if its mole fraction or proportion is known, making it fundamental in analyzing gas mixtures.

Ideal Gas Law

The Ideal Gas Law, represented as PV = nRT, links the pressure, volume, temperature, and number of moles of a gas. This principle is used to determine the total moles of gas present in a given system and to relate these quantities under conditions where the behavior of gases approximates ideality.

Conversion from Weight Percentages to Mole Fractions

When gas mixtures are provided by weight percentages, converting these to mole fractions is essential since the partial pressures depend on the number of moles. This conversion involves using the molar mass of each component to convert from a weight basis to a mole basis, thereby allowing for proper application of Dalton's Law.

Units Conversion in Gas Calculations

Consistency and accuracy in gas law calculations depend on proper units conversion, such as converting temperatures to Kelvin or pressures into standard units. This ensures that the equations, like the Ideal Gas Law, yield correct and meaningful results in any analysis involving gases.

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