What gas is in a 1.66 m3 cylinder at a temperature of 280 K and a pressure of 2 * 10 (6) Pa, if its mass is 4.6 kg.

V = 1.66 m3.

T = 280 ° C.

P = 2 * 10 ^ 6 Pa.

m = 4.6 kg.

R = 8.31 m2 * kg / s2 * ° K * mol.

M -?

You can determine which gas is in the cylinder using the periodic table. For this, it is necessary to know its molar mass M.

Let us write down 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 = m * R * T / P * V.

M = 4.6 kg * 8.31 m2 * kg / s2 * ° K * mol * 280 ° K / 2 * 10 ^ 6 Pa * 1.66 m3 = 0.0032 kg / mol.

The molar mass of oxygen O2 is M = 0.0032 kg / mol.

Answer: there is oxygen in the cylinder.