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March 29, 2017

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When water freezes, the phase change that occurs is exothermic (DH = -6.02 kJ). Based on the change in enthalpy, you would expect that water would always freeze. Use the concepts of entropy and free energy to explain why this phase change is favourable only below o degrees Celsius

  • chemistry - ,

    I would look up delta S for ice and for liquid water and use that in DG = DH -TdeltsS to show that difference between 273 K and other temperatures.

  • chemistry - ,

    Calculate the standard Gibbs free energy


    NH3(g) + HCl(G) --> NH4Cl

    Ive tried but I keep getting a different answer

    How do I get to the correc tanswer which is -91.2 kJ?

  • chemistry - ,

    What numbers are you using. I looked up numbers and came up with -89.7 kJ. Close.

  • chemistry - ,

    Balanced equation

    NH3(g) + HCl(G) --> NH4Cl

    deltaH = (1 mol)(-314.4 kJ/mol) - (1 mol)(-45.9 kJ/mol) plus (1 mol)(-92.3 kJ/mol)

    =-176.2 kJ

    deltas = (1 mol)(94.6) - (1 mol)(192.78) plus (1 mol)(-186.90)

    = 0.00588

    DG = DH - TDS

    =176.2 kJ / 0.00588

    =29995

  • chemistry - ,

    I mean -176.2 -(278)(o.oo588)

    = -177.8

  • chemistry - ,

    Standard Gibbs free energy is DGfo.
    I looked up delta Gfo and found
    NH4Cl(s) = -201.5 kJ/mol
    NH3(g) =-16.5
    HCl(g) = -95.3
    Using those numbers I get =-89.7. Check to see what those numbers are in your text table. I think you are calculating G when you want Gof

  • chemistry - ,

    is this on a website?

  • chemistry - ,

    It may be but I picked these values out of a freshman college chemistry text.

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