Practice Enthalpy Of Solution (5.5.e) - Thermodynamics

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8 questions

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Exercise
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6 sample questions

Question 1.
What is the enthalpy change when 1 mole of NaCl is dissolved in water?
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Remember the definitions of lattice energy and hydration energy.
Question 2.
Define hydration energy.
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Focus on the process of dissolution.
3Question 3.
Lattice energy refers to the energy required to:
- Dissolve a solute
- Break ionic bonds
- Hydrate ions
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Remember the role of lattice energy in dissolution.
4Question 4.
True or False: The enthalpy of solution can only be negative.
- True
- False
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Reflect on examples of both exothermic and endothermic dissolutions.
Question 5.
Given that the enthalpy change (∆solH⁰) for dissolving potassium bromide in water is +37.2 kJ/mol, explain how this could still occur despite the endothermic nature, using hydration reasoning.
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Consider temperature and solvation interactions.
Question 6.
Discuss the implications of enthalpy of solution on environmental chemistry, specifically in aquatic systems.
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Think about seasonal changes and reactions in natural waterways.

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