An ice cube of mass 10g at -10C is added to the beaker containing 150mL of water at 88.5C. Assuming no heat is lost to the surrounding; calculate the equilibrium temperature for the liquid after the ice melts.(Heat of fusion for H2O = 6.01 kJ/mol. Heat of vaporization 40.67kJ/mol. Density of H2O = 1.0g/mL.

Question

An ice cube of mass 10g at -10C is added to the beaker containing 150mL of water at 88.5C. Assuming no heat is lost to the surrounding; calculate the equilibrium temperature for the liquid after the ice melts.(Heat of fusion for H2O = 6.01 kJ/mol. Heat of vaporization 40.67kJ/mol. Density of H2O = 1.0g/mL. 
Given Table
H2O(s) = 37.1 J/mol^-1/K^-1
H2O(l) = 75.6 J/mol^-1/K^-1
H2O(g) = 33.6J/mol^-1/K^-1

DrBob222 · Answer

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