A 0.228 mol sample of Ar gas is contained in a 6.00 L flask at room temperature and pressure. What is the density of the gas, in grams/liter, under these conditions?

Density of Ar gas under the given condition is 1.52 g/L

Explanation:

Density in grams/liter = (mass of Ar gas present in flask)/(volume of flask)

We know, number of moles = (mass)/(molar mass)

Molar mass of Ar = 39.948 g/mol

So, mass of 0.228 mol of Ar =

Volume of flask = 6.00 L

So, density of gas inside flask =

Hence, density of Ar gas under the given condition is 1.52 g/L

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