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.

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

answer:

the answer is 6 valence electrons.

explanation:

valence is the # of electrons on the outer most shell of an atom.

oxygen has 6.

although, the valency of oxygen is 2, because it only needs to make 2 covalent bonds, or gain 2 electrons, to achieve the stable octet configuration of a noble gas.

that's it!

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explanation:

because it is