A26 l flask at 224 k and 19 torr contains
nitrogen. what mass of nitrogen is present?

0.991 grams of N₂ are present in the flask

Explanation:

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

P . V = n . R .T

Previously we have to convert Torr to atm (because the units of R, Universal Gases Constant). Let's think the rule of three:

760 Torr is 1 atm

19 Torr is (19 . 1)/ 760 = 0.025 atm

0.025 atm . 26L = n . 0.082 L.atm/mol.K . 224K

(0.025 atm . 26L) / (0.082 L.atm/mol.K . 224K) = 0.035 moles

Molar mass N₂ = 28 g/m

Mol . molar mass = mass → 0.035 m . 28 g/m = 0.991 grams

idk what the question is about