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17 February, 12:31

8.98 dm3 of hydrogen gas is collected at 38.8 °C. Find the volume the gas will occup at - 39.9 °C if the pressure remains constant.

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  1. 17 February, 13:27
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    V₂ = 6.7 dm³

    Explanation:

    Given dа ta:

    Volume of hydrogen = 8.98 dm³

    Initial temperature = 38.8 °C

    Final volume of hydrogen gas = ?

    Final volume = - 39.9°C

    Solution:

    Initial temperature = 38.8 °C (38.8 + 273 = 311.8 K)

    Final volume = - 39.9°C (-39.9 + 273 = 233.1 k)

    The given problem will be solve through the Charles Law.

    According to this law, The volume of given amount of a gas is directly proportional to its temperature at constant number of moles and pressure.

    Mathematical expression:

    V₁/T₁ = V₂/T₂

    V₁ = Initial volume

    T₁ = Initial temperature

    V₂ = Final volume

    T₂ = Final temperature

    Now we will put the values in formula.

    V₁/T₁ = V₂/T₂

    V₂ = V₁T₂/T₁

    V₂ = 8.98 dm³ * 233.1 K / 311.8 K

    V₂ = 2093.238 dm³. K / 311.8 K

    V₂ = 6.7 dm³
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