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29 November, 12:03

A gaseous mixture made from 37.14 g N2, 34.4 g C2H2, and 38.25 g of CO is placed in a 33.53 L vessel at 27.3 °C. What is the total pressure in the vessel?

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  1. 29 November, 15:59
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    Total pressure = 2.94 atm

    Explanation:

    Given dа ta:

    Mass of nitrogen = 37.14 g

    Mass of C₂H₂ = 34.4 g

    Mass of CO = 38.25 g

    Volume of vessel = 33.53 L

    Temperature = 27.3 °C (27.3 + 273 = 300.3 K)

    Solution:

    Number of moles of nitrogen:

    Number of moles = 37.14 g / 28 g/mol

    Number of moles = 1.3 mol

    PV = nRT

    P = nRT/V

    P = 1.3 mol * 0.0821 atm. L. mol⁻¹. K⁻¹ * 300.3 K / 33.53 L

    P = 32.1 atm / 33.53

    P = 0.96 atm

    Number of moles of C₂H₂:

    Number of moles = 34.4 g / 26.04 g/mol

    Number of moles = 1.32 mol

    PV = nRT

    P = nRT/V

    P = 1.32 mol * 0.0821 atm. L. mol⁻¹. K⁻¹ * 300.3 K / 33.53 L

    P = 32.54 atm / 33.53

    P = 0.97 atm

    Number of moles of CO:

    Number of moles = 38.25 g / 28 g/mol

    Number of moles = 1.37 mol

    PV = nRT

    P = nRT/V

    P = 1.37 mol * 0.0821 atm. L. mol⁻¹. K⁻¹ * 300.3 K / 33.53 L

    P = 33.8 atm / 33.53

    P = 1.008 atm

    Total pressure = P₁ + P₂ + P₃

    Total pressure = 1.008 atm + 0.97 atm + 0.96 atm

    Total pressure = 2.94 atm
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