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15 October, 21:14

A ballon is inflated with 2.42L of helium at a temperature of 27.0°C. When put in the freezer, the volume changes to 2.37L and - 8.8°C, and the pressure is measured to be 754torr. What was the initial pressure?

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  1. 15 October, 22:43
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    838 torr

    Step-by-step explanation:

    To solve this problem, we can use the Combined Gas Laws:

    p₁V₁/T₁ = p₂V₂/T₂ Multiply each side by T₁

    p₁V₁ = p₂V₂ * T₁/T₂ Divide each side by V₁

    p₁ = p₂ * V₂/V₁ * T₁/T₂

    dа ta:

    p₁ = ?; V₁ = 2.42 L; T₁ = 27.0 °C

    p₂ = 754 torr; V₂ = 2.37 L; T₂ = - 8.8 °C

    Calculations:

    (a) Convert temperatures to kelvins

    T₁ = (27.0 + 273.15) K = 300.15 K

    T₂ = (-8.8 + 273.15) K = 264.35 K

    (b) Calculate the pressure

    p₁ = 754 torr * (2.37 L/2.42) * (300.15/264.35)

    p₁ = 754 torr * 0.979 * 1.135

    p₁ = 838 torr
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