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Hi, I see that these are the values for liquid water. Would it be different for water vapour, or water in gas state?
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- The enthalpy of solution of an ionic compound can be calculated from its lattice enthalpy and the enthalpies of hydration of the individual ions. Use the information shown below to complete the requested calculations. Quantity Lattice energy of solid ammonium chloride Lattice energy of solid ammonium nitrate Enthalpy of hydration of the gaseous ammonium ion Enthalpy of hydration of the gaseous chloride ion Enthalpy of hydration of the gaseous nitrate ion Enthalpy Change (kJ/mol) a. The enthalpy of solution of solid ammonium chloride (in kJ/mol) b. The enthalpy of solution of solid ammonium nitrate (in kJ/mol) 705 646 -307 -381 -314A student wants to determine the melting point of water as part of an investigation into the strength of electrostatic forces. The student considers determining the freezing point of water instead. Is this a valid option? O No, it is not because the freezing point is not related to electrostatic forces. O No, it is not because the freezing point is not related to the melting point. O Yes, it is; and determining the freezing point is likely to be more accurate. O Yes, it is; but determining the freezing point is likely to be more difficult.What can you conclude about the relative magnitudes of the lattice energy of ammonium chloride and its heat of hydration? The lattice energy is smaller greater in magnitude than the heat of hydration.
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