Question

a mixture of three gases has a total pressure of 1380 mm hg at 298 k. the mixture is analysed and is found to contain 1.27 mol carbon dioxide, 3.04 mol carbon monoxide, and 1.50 mol argon. what is the partial pressure of argon? 0.258 mm hg 8020 mm hg 356 mm hg 301 mm hg 5345 mm hg

Explanation:

Step1: Calculate total moles

Total moles \(n_{total}=n_{CO_2}+n_{CO}+n_{Ar}\)
\(n_{total}=1.27 + 3.04+1.50=5.81\space mol\)

Step2: Calculate mole fraction of argon

Mole fraction \(X_{Ar}=\frac{n_{Ar}}{n_{total}}\)
\(X_{Ar}=\frac{1.50}{5.81}\approx0.258\)

Step3: Calculate partial pressure of argon

Using Dalton's law \(P_{Ar}=X_{Ar}\times P_{total}\)
\(P_{Ar}=0.258\times1380 = 356\space mm\space Hg\)

Answer:

356 mm Hg