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8 February, 22:20

A particular sample of pantothenic acid, a B vitamin, gives off 72.6 mL of nitrogen gas at 23 degrees c and 795 torr. What is the volume of the nitrogen at STP?

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  1. 9 February, 00:12
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    70.04 mL.

    Explanation:

    We can use the general law of ideal gas: V = nRT.

    where, P is the pressure of the gas in atm.

    V is the volume of the gas in L.

    n is the no. of moles of the gas in mol.

    R is the general gas constant,

    T is the temperature of the gas in K.

    If n is constant, and have two different values of V, P and T:

    P₁V₁T₂ = P₂V₂T₁

    P₁ = 795 torr, V₁ = 72.6 mL, T₁ = 23.0 °C + 273 = 296 K.

    P₂ = 760 torr (standard pressure = 1 atm = 760 torr), V₂ = ? mL, T₂ = 0.0 °C + 273 = 273 K (standard T).

    ∴ V₂ = P₁V₁T₂/P₂T₁ = (795 torr) (72.6 mL) (273 K) / (760 torr) (296 K) = 70.04 mL.
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