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Consider the calculation of the pressure in kilopascals exerted by 1.25 g of nitrogen gas in a flask of volume 250 mL (0.250 dm3) at 20°C. The amount of N2 molecules (of molar mass M  28.02 g mol 1) present is

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The amount of the nitrogen gas, N₂ molecules present is 2.68×10²² molecules

Avogadro's hypothesis

1 mole of N₂ = 6.02×10²³ molecules

How to determine the mole of N₂

We'll begin by calculating the number of mole of N₂. This can be obtained as follow:

  • Mass of N₂ = 1.25 g
  • Molar mass of N₂ = 28.02 g/mol
  • Mole of N₂ =?

Mole = mass / molar mass

Mole of N₂ = 1.25 / 28.02

Mole of N₂ = 0.0446 mole

How to determine the molecules of N₂ present

From Avogadro's hypothesis,

1 mole of N₂ = 6.02×10²³ molecules

Therefore,

0.0446 mole N₂ = 0.0446 × 6.02×10²³

0.0446 mole N₂ = 2.68×10²² molecules

Thus, the molecules of N₂ present is 2.68×10²² molecules

Learn more about Avogadro's number:

https://brainly.com/question/26141731

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