Question

The enthalpy of vaporization for water is 40.67 kJ/mol and the enthalpy of fusion for water is

6.01 kJ/mol. What is the enthalpy of deposition?

Answer 1

`\Delta H_(dep)=-46.68kJ/mol`

Step-by-step explanation:

Hello!

In this case, since vaporization is the processes by which a liquid goes to the gas phase, fusion by which a solid goes to liquid and deposition by which a gas goes to solid; we infer that the following set up relates the enthalpies associated to each process:

`\Delta H_(fus)+\Delta H_(vap)=-\Delta H_(dep)`

Because deposition goes from a state with more energy to a state with less energy, therefore it is negative; in such a way, by plugging in we obtain:

`\Delta H_(dep)=-(\Delta H_(fus)+\Delta H_(vap))\\\\\Delta H_(dep)=-(6.01kJ/mol+40.67kJ/mol)\\\\\Delta H_(dep)=-46.68kJ/mol`

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