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27 May, 21:36

Will mark as Brainliest.

A 642 mL sample of oxygen gas at 23.5°C and 795 mm Hg, is heated to 31.7°C and the volume of the gas expands to 957 mL. What is the new pressure in atm?

A) 0.723 atm

B) 0.932 atm

C) 3.05 atm

D) 5.19 atm

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Answers (1)
  1. 27 May, 21:46
    0
    We can use combined gas law,

    PV/T = k (constant)

    Where, P is the pressure of the gas, V is volume of the gas and T is the temperature of the gas in Kelvin.

    For two situations, we can use that as,

    P₁V₁/T₁ = P₂V₂/T₂

    P₁ = 795 mm Hg

    V₁ = 642 mL

    T₁ = (273 + 23.5) K = 296.5 K

    P₂ = ?

    V₂ = 957 mL

    T₂ = (273 + 31.7) K = 304.7 K

    From substitution,

    795 mm Hg x 642 mL / 296.5 K = P₂ x 957 mL / 304.7 K

    P₂ = 548.072 mm Hg

    760 mmHg = 1 atm

    548.072 mm Hg = 1 atm x (548.072 mmHg / 760 mmHg)

    = 0.721 atm

    Pressure of Oxygen gas is 0.721 atm.

    Answer is "A"

    Here, we made an assumption that oxygen gas has an ideal gas behavior.
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