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

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 in container- 1 is as follows.

    5.35 mol x molar mass of

            = 7.61 mol x 146.06 g/mol

             = 1111.52 g

Therefore, density of will be calculated as follows.

            Density =  

         density =

                       = 0.532 g/mL

Now, mass of 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 present in container 2 as follows.

  No. of moles =  

                        =

                        = 16.24 mol

Since, 1 mol contains 6 moles F atoms .

So, 16.24 mol   contains following number of atoms.

                =

                = 97.46 mol

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

periodic trends is an atom that gets larger as the number of electronic shells increase, the radius of atoms increases as you go down a certain group in the periodic table of elements. in general, the size of an atom will decrease as you move from left to right of a certain period.

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