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Assuming ideal gas behavior, we know that
P = ÏRT
So,
Ï=P/RT
where P (atm) is pressure, Ï 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):
Ï=(9.87)/(0,082*298) = 0.404 mol/L
Oxygen (O2) has a molecular weight of 32g/mol so:
Ï= 0.404 mol/L * 32g/mol * (1 Lt/1000 cm3) = 0.013 g/cm3
Wiki User
∙ 11y ago
Wiki User
∙ 12y agoaccording to density=P/RT
density at 10 bar=1e6 Pa
is 11.6 Kg/M3
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