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question
what is the partial pressure in atmospheres of co₂ if a mixture has 5.0 moles of co₂, 3.0 moles of n₂, and 1.0 mole of h₂? the container has a total pressure of 1.05 atm. your answer should have two significant figures (round your answer to two decimal places).

Explanation:

Step1: Calculate the mole fraction of \(CO_2\)

The mole fraction \(X_{CO_2}=\frac{n_{CO_2}}{n_{total}}\), where \(n_{CO_2} = 5.0\) moles, \(n_{N_2}=3.0\) moles, \(n_{H_2}=1.0\) mole. Then \(n_{total}=n_{CO_2}+n_{N_2}+n_{H_2}=5.0 + 3.0+1.0=9.0\) moles. So \(X_{CO_2}=\frac{5.0}{9.0}\).

Step2: Calculate the partial pressure of \(CO_2\)

According to Dalton's law of partial pressures \(P_{CO_2}=X_{CO_2}\times P_{total}\). Given \(P_{total} = 1.05\) atm. Then \(P_{CO_2}=\frac{5.0}{9.0}\times1.05\) atm.

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Answer:

\(0.58\) atm