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

these nuts

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.