What is the mass of 1.81 x 10^23 molecules of nitrogen, N2?

Calculating the Mass of Nitrogen, N₂

From Avogadro's hypothesis:

6.02×10²³ molecules = 1 mole of nitrogen, N₂

1 mole of nitrogen, N₂ = 28.02 g

Therefore,

6.02×10²³ molecules = 28.02 g of nitrogen, N₂

Given that we need to find the mass of nitrogen, N₂ that contains 1.81×10²³ molecules:

1.81×10²³ molecules = (1.81×10²³ × 28.02) / 6.02×10²³

1.81×10²³ molecules = 8.42 g of nitrogen, N₂

Thus, the mass of nitrogen, N₂ containing 1.81×10²³ molecules is 8.42 g.

By using Avogadro's hypothesis and the molar mass of nitrogen, we can determine the mass of nitrogen molecules accurately.