Melting x moles of ice reversibly at 273 K and 1 atm increases entropy by 28.80 cal/K. Heat of fusion is 80 cal/g and water molar mass 18 g/mol. Find x (two decimal places).
For reversible melting at the transition temperature, ΔS=Qrev/T=x(18)(80)/273. Therefore $x=28.80(273)/(18\times80)=5.46$ mol. Convert the mass-specific latent heat to a molar quantity before using the mole count.
More Equilibrium: Laws of thermodynamics. Standard states. Thermochemistry. Thermodynamic functions and their relationships: Gibbs-Helmholtz and Maxwell relations, Gibbs-Duhem equation, Van’t Hoff equation. Criteria of spontaneity and equilibrium. Absolute entropy. Partial molar quantities. Thermodynamics of mixing. Chemical potential. Fugacity, Activity and Activity coefficient. Chemical equilibria. Dependence of equilibrium constant on temperature and pressure. questions
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