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21 March, 01:57

To what temperature was 32.0L of gas at 2°C be heated for it to occupy 1.00*10^2L at the same pressure?

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  1. 21 March, 02:22
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    T₂ = 859.4 K

    Explanation:

    Given dа ta:

    Initial volume of gas = 32.0 L

    Initial temperature = 2°C (2 + 273 = 275 k)

    Final temperature = ?

    Final volume = 1.00 * 10²L

    Solution:

    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

    T₂ = V₂T₁ / V₁

    T₂ = 1.00 * 10²L * 275 K / 32.0 L

    T₂ = 27500 L. K / 32.0 L

    T₂ = 859.4 K
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