A 10.0-L flask contains 1.031gO2​ and 0.572gCO2​ at 18°C.

A 10.0-L flask contains 1.031gO2​ and 0.572gCO2​ at 18°C.

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September 3, 2023
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A 10.0-L flask contains 1.031gO2​ and 0.572gCO2​ at 18°C. What are the partial pressures of oxygen and carbon dioxide? What is the total pressure? What is the mole fraction of oxygen in the mixture?

Answer and ExplanationSolution by a verified expert

Explanation
First, calculate the number of moles of O2 and CO2.

Since the molar mass of each is not given, calculate using data from Periodic Table.

MMO2 = 32 g/mol

MMCO2 = 44 g/mol

nO2 = 1.031 g/32.0 g/mol

nO2 = 0.0322 mol

nCO2 = 0.572 g/44.0 g/mol

nO2 = 0.0130 mol

Calculate the total number of moles.

ntotal = 0.0322 mol + 0.0130 mol

ntotal = 0.0452 mol

In order to get the total pressure, you may use the ideal gas law.

PV = nRT

Ensure that units are converted correctly.

Ptotal = (ntotal x R x T)/V

Ptotal = [0.0452 mol x (0.08206 L-atm/mol-K) x (18 + 273.15 K)]/10 L

Ptotal = 0.108 atm

You can calculate the mole fraction, X, of O2 using the following formula.

XO2 = nO2/ntotal

XO2 = 0.0322 mol/0.0452 mol

XO2 = 0.712

Answer
Total pressure is 0.108 atm. Mole fraction of oxygen is 0.712.

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