Question

Sulfur hexafluoride, a dense gas, is held in two separate containers in a storage room at an atmospheric pressure of 755 mmHg and 20.3 °C. The volume of container 1 is 2.09 L, and it contains 7.61 mol of the gas. The volume of container 2 is 4.46 L. Determine the moles of F atoms in container 2 and the density of the gas at the conditions in the room

Answer 1

Step-by-step explanation:

As it is given that both the given containers are at same temperature and pressure, therefore they have the same density.

So, mass of
`SF_(6)` in container- 1 is as follows.

5.35 mol x molar mass of
`SF_(6)`

= 7.61 mol x 146.06 g/mol

= 1111.52 g

Therefore, density of
`SF_(6)` will be calculated as follows.

Density =
`(mass)/(volume)`

density =
`(1111.52 g)/(2.09 L * 1000 ml/L)`

= 0.532 g/mL

Now, mass of
`SF_(6)` in container- 2 is calculated as follows.

4.46 L x 1000 mL/L x 0.532 g/mL

= 2372.72 g

Hence, calculate the moles of moles
`SF_(6)` present in container 2 as follows.

No. of moles =
`\frac{mass}{\text{molar mass}}`

=
`(2372.72 g)/(146.06 g/mol)`

= 16.24 mol

Since, 1 mol
`SF_(6)` contains 6 moles F atoms .

So, 16.24 mol
`SF_(6)` contains following number of atoms.

=
`16.24 mol * 6`

= 97.46 mol

Thus, we can conclude that moles of F atoms in container 2 are 97.46 mol.