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10 February, 13:48

A gas is found to occupy a volume of 38.2 mL at 25.0ºC and an unknown

pressure. If this same gas occupies 37.5 mL at STP, determine what its unknown original pressure was in mm Hg.

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Answers (1)
  1. 10 February, 17:27
    0
    836 mmHg

    Explanation:

    Given dа ta:

    Initial volume = 38.2 mL

    Initial temperature = 25°C (25+273=298 k)

    Final volume = 37.5 mL

    Final temperature = standard = 273 K

    Final pressure = standard = 1 atm

    Initial pressure = ?

    Solution:

    Formula:

    P₁V₁/T₁ = P₂V₂/T₂

    P₁ = Initial pressure

    V₁ = Initial volume

    T₁ = Initial temperature

    P₂ = Final pressure

    V₂ = Final volume

    T₂ = Final temperature

    Solution:

    P₁ = P₂V₂T₁ / T₂ V₁

    P₁ = 1 atm * 37.5 mL * 298 K / 273 K * 38.2 mL

    P₁ = 11175 atm / 10428.6

    P₁ = 1.1 atm

    atm to mmHg

    1.1 atm * 760 mmHg / 1 atm

    836 mmHg
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