Determine the temperature of oxygen which is under a pressure of 2.1 * 10 ^ 5 Pa

| May 6, 2021 | education

Determine the temperature of oxygen which is under a pressure of 2.1 * 10 ^ 5 Pa, if the volume is 0.02 m ^ 3 and the mass is 0.03 kg.

V = 0.02 m3.

m = 0.03 kg.

P = 2.1 * 10 ^ 5 Pa.

M (O2) = 0.032 kg / mol.

R = 8.31 m2 * kg / s2 * ° K * mol.

T -?

The molecular formula of oxygen has the form O2, therefore, its molar mass, according to the periodic table, will be M (O2) = 0.032 kg / mol.

We express the absolute gas temperature from the Mendeleev-Cliperon law: P * V = m * R * T / M, where P is the gas pressure, V is the gas volume, m is the gas mass, R is the universal gas constant, T is the absolute temperature, M is the molar mass of the gas.

T = P * V * M / R * m.

T = 2.1 * 10 ^ 5 Pa * 0.02 m3 * 0.032 kg / mol / 8.31 m2 * kg / s2 * ° K * mol * 0.03 kg = 539 ° K.

Answer: the oxygen temperature is T = 539 ° K.



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