A mixture of three gases has a total pressure of 1380 mmhg at 298 k. The mixture is analyzed and is found to contain 1. 27 mol co2, 3. 04 mol co, and 1. 50 mol ar. What is the partial pressure of ar?.

According to Dalton's law of partial pressures, each gas in a mixture exerts the same amount of pressure as it would if it were the only one in the container.

Briefing:

Given ,a mixture of three gases has a total pressure of 1380 mm Hg (=1.81579 atm) at 298 K

Moles of CO2 = 1.27 moles

Moles of CO = 3.04 moles

Moles of Ar = 1.50 moles

Calculate total number of moles

Total number of moles = n(CO2)+ n(CO)+ n(Ar) = 1.27 mol+ 3.04 mol+ 1.50 mol = 5.81 moles

Calculate mol fraction Ar

Mol fraction Ar = 1.50 mol/5.81 mol = 0.258

Calculate partial pressure

1380 mm Hg * 0.258 moles Ar = 356.04 mm Hg = 0.4685 atm

The partial pressure of Ar is 356.04 mm Hg (= 0.4685 atm)

To know more about partial pressure visit:

https://brainly.com/question/14356335

#SPJ4