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