Dinitrogen monoxide gas is collected at-3.0 °c in an evacuated flask with a measured volume of 5.0 l. when all the gas has been collected, the press the flask is measured to be 0.100 atm . calculate the mass and number of moles of dinitrogen monoxide gas that were collected. round your answer to 2 significant digits. mass: mole: nol explanation check 2019 mcgraw-hill education all rights reserved

0.971 grams

Explanation:

Given:

Temperature = 3.0° C = 3 + 273 = 276 K

Volume, V = 5.0 L

Pressure, P = 0.100 atm

Now, from the relation

PV = nRT

where,

n is the number of moles,

R is the ideal gas constant  = 0.082057 L atm/mol.K

thus,

0.1 × 5 = n ×  0.082057 × 276

or

n = 0.022 moles

Also,

Molar mass of the Dinitrogen monoxide gas (N₂O)

= 2 × Molar mass of nitrogen + 1 × Molar mass of oxygen

= 2 × 14 + 16 = 44 grams/mol

Therefore, Mass of 0.022 moles of N₂O = 0.022 × 44 = 0.971 grams