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Assuming ideal gas behavior, we know that

P = ρRT

So,

ρ=P/RT

where P (atm) is pressure, ρ is molar density (mol L-1), R is a constant (0,082 atm L mol-1 K-1), and T is temperature (K)

10 bar are 9.87 atm.

Therefore, assuming ambient temperature 25°C (298 K):

ρ=(9.87)/(0,082*298) = 0.404 mol/L

Oxygen (O2) has a molecular weight of 32g/mol so:

ρ= 0.404 mol/L * 32g/mol * (1 Lt/1000 cm3) = 0.013 g/cm3

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