Consider a chamber filled with gaseous N2 (molar mass 28.0 g/mol) and O2 (molar

Question

Consider a chamber filled with gaseous N2 (molar mass 28.0 g/mol) and O2 (molar mass 32.0 g/mol) which behave ideally (cv = (3/2)R). The chamber has a volume of 1.00 L and is initially at a temperature T = 25.0 OC ; the total initial pressure of all gases is ptot,i = 760. torr. The initial partial pressure of oxygen is pO2,i = 593. torr. A vacuum pump attached to the chamber is turned on. The total pressure inside the chamber is reduced to 35 mtorr (i.e. milli-torr) and the vacuum pump is turned off. You may assume that the temperature does not change as the pressure is reduced. What is the final partial pressure of O2: pO2,f?

Explanation / Answer

given

ptot,i = 760. torr.

pO2,i = 593

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