At a temperature of 400K, the gas pressure is 166000Pa. Find the density of the gas if its paint mass is 0.032 kg / mol.

univerkov | September 4, 2021 | education

Given: T (temperature) = 400 K; P (taken gas pressure) = 166000 Pa.

Constants: R (universal gas constant) = 8.31 J / (mol * K); according to the condition M (molar mass) = 0.032 kg / mol (oxygen).

To find the density of the taken gas (oxygen) under the given conditions, we use the Mendeleev-Clapeyron law: P * V = m / M * R * T, whence P * M / (R * T) = m / V = ρ.

Calculation: ρ = 166000 * 0.032 / (8.31 * 400) = 1.598 kg / m3.

Answer: Oxygen under the given conditions has a density of 1.598 kg / m3.

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