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24 November, 21:01

What pressure will 2.6 x 1023 molecules of h2 exert in a 3.9 l container at 45°c?

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  1. 24 November, 21:16
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    We can use the ideal gas law equation to find the pressure

    PV = nRT

    where;

    P - pressure

    V - volume - 3.9 x 10⁻³ m³

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

    T - temperature - 45 °C + 273 = 318 K

    n - number of moles

    there are 6.022 x 10²³ molecules in 1 mol of H₂

    Therefore when theres 2.6 x 10²³ H₂ molecules - 1 / (6.022 x 10²³) x 2.6 x 10²³

    Number of H₂ moles - 0.43 mol

    substituting these values in the equation,

    P x 3.9 x 10⁻³ m³ = 0.43 mol x 8.314 Jmol⁻¹K⁻¹ x 318 K

    P = 291.5 kPa
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