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16 April, 22:10

How would I find the quantity of heat absorbed or released when 2.0g of LiOH is dissolved in 100g of H₂0 when the enthalpy of the solution is - 23.6KJ/mol?

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  1. 16 April, 23:54
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    1.97kJ of energy are released.

    Explanation:

    The dissolution of LiOH in water is:

    LiOH (s) → Li⁺ (aq) + OH⁻ (aq) ΔH = - 23.6kJ

    That means, when 1 mole of LiOH is dissolved, there are released (Because of the - in the enthalpy) 23.6kJ

    2.0 g of LiOH (Molar mass: 23.95g/mol) are:

    2.0g LiOH * (1 mol / 23.95g) = 0.0835 moles of LiOH.

    As 1 mole of LiOH release 23.6kJ, 0.0835moles release:

    0.0835moles * (-23.6kJ / 1mole) = 1.97kJ of energy are released
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