University:
North Central College
Course:
CHEM 121 | General Chemistry I
Academic year:

2022
Views:

482

Pages:

2
Author:

StellarStrategist

A student investigates the enthalpy of solution, Hsoln , for two alkali metal halides, LiCl and NaCl. In addition to the salts, the student has access to a calorimeter, a balance with a precision of ±0.1 g, and a thermometer with a precision of ±0.1C. (a) To measure Hsoln for LiCl, the student adds 100.0 g of water initially at 15.0C to a calorimeter and adds 10.0 g of LiCl(s), stirring to dissolve. After the LiCl dissolves completely, the maximum temperature reached by the solution is 35.6C. (i) Calculate the magnitude of the heat absorbed by the solution during the dissolution process, assuming that the specific heat capacity of the solution is 4.18 J/(g·°C). Include units with your answer. q = mcT = (110.0 g)(4.18 J/(g·°C))(35.6°C  15.0°C) 1 point is earned for the correct setup. 1 point is earned for the correct answer with units. = 9,470 J = 9.47 kJ (ii) Determine the value of Hsoln for LiCl in kJ/molrxn . 10.0 g LiCl  1 mol LiCl  0.236 mol LiCl 42.39 g LiCl 1 point is earned for the number of moles of LiCl. 1 point is earned for the correct Hsoln and the correct sign. -9.47 kJ = 40.1 kJ/molrxn 0.236 mol LiCl To explain why Hsoln for NaCl is different than that for LiCl, the student investigates factors that affect Hsoln and finds that ionic radius and lattice enthalpy (which can be defined as the H associated with the separation of a solid crystal into gaseous ions) contribute to the process. The student consults references and collects the data shown in the table below. Ion Li+ Na+ Ionic Radius (pm) 76 102 (b) Write the complete electron configuration for the Na+ ion in the ground state. 1s2 2s2 2p6 1 point is earned for the complete correct configuration. (c) Using principles of atomic structure, explain why the Na+ ion is larger than the Li+ ion. The valence electrons in the Na+ ion are in a higher principal energy level than the valence electrons in the Li+ ion. Electrons in higher principal energy levels are, on average, farther from the nucleus. 1 point is earned for a correct explanation based on occupied principal energy levels. (d) Which salt, LiCl or NaCl, has the greater lattice enthalpy? Justify your answer. LiCl. Because the Li+ ion is smaller than the Na+ ion, the Coulombic attractions between ions in LiCl are stronger than in NaCl. This results in a greater lattice enthalpy. 1 point is earned for the correct choice and justification. (e) Below is a representation of a portion of a crystal of LiCl. Identify the ions in the representation by writing the appropriate formulas ( Li+ or Cl ) in the boxes below. Cl  See diagram above. Li+ 1 point is earned for both identifications. (f) The lattice enthalpy of LiCl is positive, indicating that it takes energy to break the ions apart. in LiCl. However, the dissolution of LiCl in water is an exothermic process. Identify all particle-particle interactions that contribute significantly to the exothermic dissolution process being exothermic. For each interaction, include the particles that interact and the specific type of intermolecular force between those particles. There are interactions between Li+ ions and polar water molecules and between Cl ions and polar water molecules. These are ion-dipole interactions. 1 point is earned for identifying the particles that interact. 1 point is earned for correctly identifying the type of interaction.