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For question 4.1 in the book, the question asks to calculate the energy needed to vaporize ice at -5.042 degrees C to a vapor at 150.33 degrees C. I understand how to calculate for the phases where the water is increasing in temperature, but for the phase changes, the solution book multiplies the moles of ice by 6.01KJ and the moles of water by 40.7KJ. Where did they get these KJ values for ice to water and water to vapor from?
They are most likely given in one of the tables in Chapter 4. However, on tests/midterm those values should be given if needed to solve a problem. So if a phase change is involved in figuring out the enthalpy of fusion and vaporization those values represent the amount of enthalpy required to change phases for every mol involved.
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