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Dinitrogen difluoride gas is collected at 5.0 °C in an evacuated flask with a measured volume of 50.0 L. When all the gas has ben collected, the pressure in the flask is measured to be 0.070 atm: Calculate the mass and number of moles of dinitrogen difluoride gas that were collected.

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Answer:

0.153 moles with a mass of 10.09 grams of dinitrogen difluoride gas were collected

Explanation:

Let's apply the Ideal Gases Law to solve this:

P . V = n . R .T

0.070 atm . 50L = n . 0.082L.atm / mol.K . 278K

(0.070 atm . 50L) / (0.082L.atm / mol.K . 278K) = n

0.153 moles = n

Molar Mass N₂F₂ = 66.01 g/m

Molar mass . moles = mass

66.01 g/m . 0.153moles = 10.09 g