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Calculation of entropy change for melting ice

  1. Nov 21, 2011 #1
    1. The problem statement, all variables and given/known data
    Calculate the entropy change when 1 mole of ice at 268 K is melted to form water at 323 K. The heat capacity of ice is 3.8 J K-1 kg-1 and that of water is 75 J K-1 kg-1. The enthalpy of fusion of ice at 273 K is 6.02 kJ mol-1.

    I know the entropy change by the melting of the ice is given by

    delta(S)=delta(Q)/T

    and that this is worked out by the enthalpy of fusion.

    My question is how do I calculate the entropy change caused by the change in temperature since it is not at a constant temperature does this mean the first equation cannot be used?

    Also this isn't a homework question it is an exam question from a previous year and my exam is tomorrow.
     
  2. jcsd
  3. Nov 24, 2011 #2
    Relate delta(Q) to temperature and integrate.
     
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