A mixture of 34.25 moles of argon, 14.11 moles helium, 24.38 moles neon, and 40.39 moles krypton is contained in a 2930.17 L vessel at 148.45°C. Calculate the partial pressure of argon. Show the partial pressures of the other gases in your solution. Atomic Mass: Ar: 39.948 g/mol He: 4.003 g/mol Ne: 20.180 g/mol Kr: 83.798 g/mol

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Solve using dimensional analysis. Show the complete solution. Do not round off nonfinal answers.
A mixture of 34.25 moles of argon, 14.11 moles helium, 24.38 moles neon, and 40.39 moles
krypton is contained in a 2930.17 L vessel at 148.45°C. Calculate the partial pressure of argon.
Show the partial pressures of the other gases in your solution.
Atomic Mass:
Ar: 39.948 g/mol
He: 4.003 g/mol
Ne: 20.180 g/mol
Kr: 83.798 g/mol
Transcribed Image Text:A mixture of 34.25 moles of argon, 14.11 moles helium, 24.38 moles neon, and 40.39 moles krypton is contained in a 2930.17 L vessel at 148.45°C. Calculate the partial pressure of argon. Show the partial pressures of the other gases in your solution. Atomic Mass: Ar: 39.948 g/mol He: 4.003 g/mol Ne: 20.180 g/mol Kr: 83.798 g/mol
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