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9 May, 19:51

Calculate the mass of 1.50 L of CH4 at STP

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  1. 9 May, 20:20
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    Let's assume that CH₄ has ideal gas behavior.

    Then we can use ideal gas formula,

    PV = nRT

    Where, P is the pressure of the gas (Pa), V is the volume of the gas (m³), n is the number of moles of gas (mol), R is the universal gas constant (8.314 J mol⁻¹ K⁻¹) and T is temperature in Kelvin.

    P = 1 atm = 101325 Pa

    V = 1.50 L = 1.50 x 10⁻³ m³

    n = ?

    R = 8.314 J mol⁻¹ K⁻¹

    T = 0 °C = 273 K

    By substitution,

    101325 Pa x 1.50 x 10⁻³ m³ = n x 8.314 J mol⁻¹ K⁻¹ x 273 K

    n = 0.0669 mol

    Hence, moles of CH₄ = 0.0669 mol

    Moles = mass / molar mass

    Molar mass of CH₄ = 16 g mol⁻¹

    Mass of CH₄ = moles x molar mass

    = 0.0669 mol x 16 g mol⁻¹

    = 1.0704 g

    Hence, mass of CH₄ in 1.50 L at STP is 1.0704 g
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