This means that you release 40.7 kJ for every mole of water that goes from steam at to liquid water at time, you have In water's case, #DeltaH_"vap"# is equal to 40.7 kJ/mol. The molar enthalpy of vaporization will tell you how much energy is absorbed when 1 mole of liquid water is converted to 1 mole of steam. This is used to show that heat is released, not absorbed, when condensation occurs. Notice that the equation has a negative sign this time. #DeltaH_"vap"# - the molar enthalpy of vaporization. Let's say that you need to determine how much heat is released when 5 moles of water condense from steam at to liquid at This time, the equation would be If you want to know how much heat would be needed to convert 3 moles of ice at its melting point to liquid water, you'd have This means that, in order to convert 1 mole of solid ice at to liquid water at you need to impart 6.02 kJ of heat. In water's case, the molar enthalpy of fusion is equal to 6.02 kJ/mol. #DeltaH_"fus"# - the molar enthlapy of fusion. #n# - the number of moles of a substance Let's say, for example, that you want to know how much heat is needed to melt 3 moles of ice at its melting temperature of equation will look like this This equation is used to establish a relationship between how much heat is involved when a number of moles of a substance undergoes a phase change.
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