Find the mass in grams of 1.00 x 10^23 molecules of n2

  the mass  in grams  of  1.00 x 10^23  molecules of N2 is 4.648  g

 calculation

Step  1:  use  the Avogadro's  constant   to determine  the moles of N2

According  to Avogadro's  law    1   mole  =  6.02 x 10 ^23  molecules

                                                       ?  moles  = 1.00 x 10 ^23  molecules

      by  cross  multiplication

 = (1  mole  x 1.00  x10^23  molecules)  / (  6.02  x 10^23  molecules)

        =0.166 moles  of  N2

Step 2 :  find  mass  of N2

Mass =  moles x molar  mass

From  periodic  table the molar  mass  of N2  = 14 x2  = 28 g/mol

mass = 0.166  moles  x   28  g/mol   = 4.648  g

here are some of the ways in which chemical and nuclear reactions differ.

explanation: