Question
Asked Oct 12, 2019
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A gas mixture is made by combining 7.5 g each of Ar, Ne, and an unknown diatomic gas. At STP, the mixture occupies a volume of 18.53 L.

What is the molar mass of the unknown gas?

Identify the unknown gas.

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Expert Answer

Step 1

Given,

Mass of Ar, Ne and an unknown diatomic gas = 7.5 g

Moles of Ar and Ne can be calculated as:

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7.5 g Mass of Ar Moles of Ar -0.1875 mol Molar mass of Ar 40 g/mol 7.5 g Mass of Ne Moles of Ne = 0.375 mol Molar mass of Ne 20 g/mol

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Step 2

Volume, V = 18.53 L

At STP: Pressure, P = 1 atm and temperature, T = 273 K

The total number of moles in the gas mixture can be calculated using the ideal gas equation as:

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PV nRT PV n RT 1 atm x 18.53 L Latm x 273 K 0.0821 mol K n 0.827 mol

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Step 3

The molar mass of the unknown g...

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Total moles Moles of Ar moles of Ne moles of unknown gas Moles of unknown gas = Total moles - (Moles of Ar Moles of Ne) Moles of unknown gas 0.827 mol (0.1875 mol 0.375 mol) Moles of unknown gas = 0.2645 mol 7.5 g Mass 28.35 g/mol Molar mass of unknown gas - Moles 0.2645 mol

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Tagged in
ScienceChemistry

Ideal gases

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