Question

In the heating curve of water shown below, why is line \[WX\] longer than line \[YZ\]?

Answer 1

Hint: The above graph describes the change of phase of water from its solid form to liquid form and then to its gaseous form. Check the temperature and time required by each line to better understand how heat corresponds to the phase changes from ice to water and then to its vapour form. Then compare the molar enthalpy of both the phase change to explain the given question.

Complete step-by-step answer:
The above heating curve of water shows that water is first converted from its solid form to its liquid form by melting it. Then the liquid form is boiled to the gaseous form. The \[YZ\] line is at a constant temperature of \[0^\circ C\] which is also the melting point of ice. Hence, there is a melting phase transition of ice by heating it over time.

The \[WX\] line is at a constant temperature of \[100^\circ C\] which is also the boiling point of water. Hence, there is again a phase transition of water by boiling it over time. The molar enthalpy of ice at \[0^\circ C\] or \[273K\], \[\Delta {{\rm H}_{fusion}}\] is \[6.02kJ/mol\]at normal atmospheric pressure. Similarly, the molar enthalpy of vaporizing for water, \[\Delta {{\rm H}_{vaporisation}}\] is \[40.7kJ/mol\].

Here, the enthalpy of vaporizing for water is larger as compared to the enthalpy of fusion. This larger enthalpy indicates a larger amount of heat being applied at constant pressure in order to perform the phase transition. Since more heat is required to vaporize the water, hence, more time is required at the same constant heating rate to vaporize water. Thus, \[WX\] line is longer than \[YZ\] line.


Note: The value of molar enthalpy of ice has a constant value of \[6.02kJ/mol\] only at \[273K\] and at normal pressure. Similarly, the molar enthalpy of vaporization for water has a constant value of \[40.7kJ/mol\] at \[373K\] and at normal pressure. Any change in these conditions will also alter the values of enthalpy.