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15 April, 09:21

A 3.00-l flask is filled with gaseous ammonia, nh3. the gas pressure measured at 15.0 ∘c is 2.15 atm. assuming ideal gas behavior, how many grams of ammonia are in the flask? express your answer to three significant figures and include the appropriate units.

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  1. 15 April, 09:50
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    We can find the mass of ammonia using the ideal gas law equation,

    PV = nRT

    where

    P - pressure - 2.15 atm x 101 325 = 2.18 x 10⁵

    V - volume - 3.00 x 10⁻³ m³

    n - number of moles

    R - universal gas constant - 8.314 Jmol⁻¹K⁻¹

    T - temperature in kelvin - 15.0 °C + 273 = 288 K

    substituting these values in the equation

    2.18 x 10⁵ Pa x 3.00 x 10⁻³ m³ = n x 8.314 Jmol⁻¹K⁻¹ x 288 K

    n = 0.273 mol

    number of moles of NH₃ is 0.273 mol

    molar mass of NH₃ - 17.0 g/mol

    mass pf ammonia present - 0.273 mol x 17.0 g/mol = 4.64 g

    mass of NH₃ present is 4.64 g
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