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30 October, 20:28

If a gas has a volume of 1000 ML at a temperature of 23°C and a pressure of 100 mmhg, what is it's volume under standard conditions of temperature and pressure?

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  1. 30 October, 23:02
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    119.7 mL.

    Explanation:

    From the general law of ideal gases:

    PV = nRT.

    where, P is the pressure of the gas.

    V is the volume of the container.

    n is the no. of moles of the gas.

    R is the general gas constant.

    T is the temperature of the gas (K).

    For the same no. of moles of the gas at two different (P, V, and T):

    P₁V₁/T₁ = P₂V₂/T₂.

    P₁ = 100.0 mmHg, V₁ = 1000.0 mL, T₁ = 23°C + 273 = 296 K. P₂ = 1.0 atm = 760.0 mmHg (standard P), V₂ = ? mL, T₂ = 0.0°C + 273 = 273.0 K (standard T).

    ∴ V₂ = (P₁V₁T₂) / (T₁P₂) = (100.0 mmHg) (1000.0 mL) (273.0 K) / (296 K) (760.0 mmHg) = 121.4 mL.
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