Temperature = 26.4oC (299.4 K)
Pressure = 798 mmHg (1.05 atm)
Volume = 475 cm3 (0.475 L)
R = 0.082057 atm L mol-1K-1
So, PV= nRT
1.05*0.475= n *0.082057* 299.4
Moles of air = 0.49875/24.5678
Moles of air = 0.0203
Moles of oxygen = 0.21* moles of air
Moles of oxygen = 0.21*0.0203
Moles of oxygen= 0.004263
So, mass of oxygen = moles of oxygen* molecular weight of oxygen
Mass of oxygen = 0.004263*1 6
Mass of oxygen in balloon = 0.068208g
A balloon contains 475 cm of air at 798 mmHg and 26.4 °C. How many grams...
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