1. a) “super-cool” water, which is liquid water that exists below the freezing point of water at 1 atm. The molar enthalpy of fusion of ice at 0◦C is 6.01 kJ mol−1 and molar heat capacity of liquid water between −5◦C and 0◦C is 75.3 J K−1 mol−1 and expected to be constant. One mole of supercooled water at −5◦C is induced to crystallize in an insulated vessel.The result is a mixture of ice and water at 0◦C. What fraction of this mixture is ice?
1. a) “super-cool” water, which is liquid water that exists below the freezing point of water at 1 atm. The molar enthalpy of fusion of ice at 0◦C is 6.01 kJ mol−1 and molar heat capacity of liquid water between −5◦C and 0◦C is 75.3 J K−1 mol−1 and expected to be constant. One mole of supercooled water at −5◦C is induced to crystallize in an insulated vessel.The result is a mixture of ice and water at 0◦C. What fraction of this mixture is ice?
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Changes in entropy have often been described in terms of order and disorder. For example, a process that leads to an increase in order has a negative ∆S. For the freezing of the supercooled water discussed above, two things are obvious. First, the process is spontaneous. Second, the formation of solid ice from liquid water is accompanied by an increase in order. How would you account for the apparent contradiction that in a spontaneous process such as this, ∆S is negative? To bolster your answer, calculate the ∆S for this process
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