Question

find the mass in grams of 1.00 x 10^23 molecules of N2

Answer 1

  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

Answer 2

The mass of $\rm 1.0\;\times\;10^2^3$ molecules of diatomic nitrogen has been 4.648 grams.

It has been known from the mole concept that 1 mole of a substance has $\rm 6.023\;\times\;10^2^3$ molecules.

So, $\rm 1.0\;\times\;10^2^3$ molecules of nitrogen gas have been consisted by:

$\rm 6.023\;\times\;10^2^3$ molecules = 1 mole

$\rm 1.0\;\times\;10^2^3$ molecules = $\rm \dfrac{1}{6.023\;\times\;10^2^3}\;\times\;1.0\;\times\;10^2^3$ mole

$\rm 1.0\;\times\;10^2^3$ molecules = 0.166 moles.

The  $\rm 1.0\;\times\;10^2^3$ molecules of nitrogen molecule has been consisted in 0.166 moles of gas.

The molecular weight of diatomic nitrogen is = 28 g/mole.

Mass = $\rm moles\;\times\;molecular\;weight$

Mass of diatomic nitrogen = 0.166 $\times$ 28

Mass of diatomic nitrogen  = 4.648 grams.

The mass of $\rm 1.0\;\times\;10^2^3$ molecules of diatomic nitrogen has been 4.648 grams.

For more information about the mass of molecules, refer to the link:

https://brainly.com/question/17756207