It can be calculated that an air sample has an average molar mass of 28.82 g/mol. a. What is the total mass of air in a 1.5 L balloon in the mountains if the temperature = 23 ∘C and pressure = 0.68 atm? Assume the air behaves as an ideal gas
It can be calculated that an air sample has an average molar mass of 28.82 g/mol.
a. What is the total mass of air in a 1.5 L balloon in the mountains if the temperature = 23 ∘C and pressure = 0.68 atm? Assume the air behaves as an ideal gas
Given that: air sample has molar mass= 28.82 g/mol
Volume of balloon(V) = 1.5 L, Temperature(T)= 23⁰0C+ 273.15 =296.15 K, pressure(P)= 0.68 atm.
The air is behaving as an ideal gas.
Then from the ideal gas law:
PV=nRT
Where, P is pressure, V is volume, n is number of moles, R is universal gas constant and T is temperature.
The value of gas constant is taken as 0.08205 L.atm-1.K-1.mol-1.
Using all the values, the number of moles (n) is calculated as:
Hence the number of moles of air filled in balloon is 0.04197 mol.
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