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26 December, 20:14

How many moles of air are in 1.00 L at - 23 C anf 101 KPa?

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  1. 26 December, 23:27
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    0.041 mol.

    Explanation:

    To solve this problem, we can use the general law of ideal gases:

    PV = nRT,

    where, P is the pressure of the air = 101 kPa = 0.9967 atm.

    V is the volume of the air = 1.00 L.

    n is the no. of moles of air = ? mol.

    R is the general gas constant = 0.082 L. atm/mol. K.

    T is the temperature of the air = 23 °C + 273 = 296.0 K.

    ∴ n (no. of moles of air) = PV/RT = (0.9967 atm) (1.00 L) / (0.082 L. atm/mol. K) (296.0 K) = 0.041 mol.
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