Question

The density of air at 1.000 atm and 25 °C is 1.186 g/L. 9. Calculate the average molecular mass of air. a) From this value, and assuming that air contains only molecular nitrogen and b) molecular oxygen gases, cal culate the mass % of N2 and O2 in air.

Answer 1

Solhas givenis density of air = 1.000 atm Temperature = 25°c = (273+257 - 298k density = 1.186 g/L we know; PV=ART In= mass mass n=mass Plla mass RT Mo IPO = mass XRT volume density - mass V volume a [PMO=ORT] 1.000X Mo = 1.186 X 0.0821 X 298 I MO = 29 gm 191 Average molemlar mass of air = 29 gol mole

ibl let mass t of N₂ in air be dll. then mass f- of Oz in ain= (100-d) 7. molar mass of O2= 32gm/mol; mass of N2 =28 gminal Average 28x2 + 324 LUD–) = 29 (100T 100 28x+ 3200 - 32x = 2900 4x=300 1- 758 mass "/-07 N2 = 754. mass t. of O2 = 25%
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