Ask Question
20 June, 16:37

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?

+3
Answers (1)
  1. 20 June, 17:04
    0
    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
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “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 ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers