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Partial pressure of a gas by Dalton's law: mole fraction times total pressure

This type of question, asked 3 times: 15 May 2023 S1, 20 Apr 2025 S2, 20 Apr 2026 S2. All 3 questions below, oldest first.

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  1. Question 1

    15 May 2023 S1

    55
    Calculate the partial pressure exerted by dioxygen from a mixture of 32 g O2_2, 80 g Ar (mol. mass 40) and 4 g dihydrogen Ptotal=10P_{\text{total}} = 10 bar.

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  2. Question 2

    20 Apr 2025 S2

    61
    A container consisting mixture of 28 g N2,8 gHe28\text{ }g{\text{ }N}_{2},8\text{ }gHe and 40 g Ne at 25∘C25^{\circ}C. If the total pressure exerted by the gaseous mixture is 20 bar, what is the partial pressure exerted by N2N_{2} ?

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  3. Question 3

    20 Apr 2026 S2

    4
    A mixture of 0.5 mol N2\mathrm{N_2} gas, 1.0 mol O2\mathrm{O_2} gas and 1.5 mol H2\mathrm{H_2} gas exerts a total pressure of 18 bar. Find the partial pressure of O2(g)\mathrm{O_{2(g)}}.

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