Question

Compare 1 mole of H2, 1 mole of O2 and 1 mole of F2

Answer 1

Explanation:

(a)  As per the mole concept, one mole of any atom contains $6.022 \times 10^{23}$ atoms or molecules, that is, Avogadro's number of atoms.

Therefore, 1 mole of $H_{2}$ = $2 \times 6.022 \times 10^{23}$ molecules

                                           = $1.2044 \times 10^{23}$ molecules

   1 mole of $O_{2}$ = $2 \times 6.022 \times 10^{23}$ molecules

                                    = $1.2044 \times 10^{23}$ molecules

   1 mole of $F_{2}$ = $2 \times 6.022 \times 10^{23}$ molecules

                                    = $1.2044 \times 10^{23}$ molecules

Hence, there are equal number of molecules present in the given atoms.

(b)   Mass of each given atom will be calculated as follows.

                Mass = no. of moles × molar mass

As one molecule of $H_{2}$ contains 2 atoms of hydrogen.

So, mass of 1 mole of $H_{2}$ = $2 mol \times 1.008 g/mol$

                                                     = 2.016 g

      mass of 1 mole of $O_{2}$ = $2 mol \times 15.999 g/mol$

                                                     = 31.996 g

      mass of 1 mole of $F_{2}$ = $2 mol \times 18.998 g/mol$

                                                     = 37.996 g

Thus, we can conclude that $F_{2}$ has the greatest mass.