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Entropy change

  1. Dec 21, 2011 #1

    RCB

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    1. The problem statement, all variables and given/known data
    "Which of SrSO4 and BaSO4 is more soluble. Justify your answer using the following data to calculate the difference between ΔS total:

    ΔHsolution SrSO4 (s) = -9 kJ/mol
    ΔHsolution BarSO4 (s) = +19 kJ/mol

    S Sr2+ = -33 kJ/mol
    S Ba2+ = +10 kJ/mol


    2. Relevant equations



    3. The attempt at a solution
    So the difference in ΔH solution is 28 kJ/mol
    this equates to a difference of 93.6 J/K/mol (finding ΔS surrounding)

    ΔS total = ΔS surr + ΔS system

    ΔS system = S(products) - S(reactants)

    I can understand why I don't need the entropy for the SO42- ion BUT how can I find ΔS total if I dont have S(products)

    Once I have this it is obvious how to continue

    thanks
     
  2. jcsd
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