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

Answer:

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 = $(0.228\times 39.948)g=9.11g$

Volume of flask = 6.00 L

So, density of gas inside flask = $\frac{9.11g}{6.00L}=1.52g/L$

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