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.

Question

Adelaide Buckley

Chemistry

29 October, 20:48

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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Ishaan Kidd · Answer 1

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