Question

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?

Answer 1

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

Step-by-step 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 =
`(0.228* 39.948)g=9.11g`

Volume of flask = 6.00 L

So, density of gas inside flask =
`(9.11g)/(6.00L)=1.52g/L`

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