A 26 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