A problem in finding enthelpy of metal oxides

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SUMMARY

The discussion centers on the enthalpy changes associated with the hydration of metal oxides, specifically Magnesium Oxide, Calcium Oxide, Barium Oxide, and Strontium Oxide. It concludes that Calcium Oxide releases more energy upon hydration than Magnesium Oxide, despite the latter's stability due to Magnesium Hydroxide. The complexity arises from the interplay of large positive and negative enthalpy terms, which can lead to counterintuitive results in energy release during hydration.

PREREQUISITES
  • Understanding of enthalpy and thermodynamics
  • Familiarity with hydration reactions of metal oxides
  • Knowledge of stability concepts in chemical compounds
  • Basic grasp of energy balance in chemical processes
NEXT STEPS
  • Research the hydration enthalpy of Calcium Oxide using thermodynamic data
  • Study the stability of Magnesium Hydroxide and its implications on energy release
  • Explore the concept of enthalpy terms in chemical reactions
  • Investigate the hydration processes of other metal oxides for comparative analysis
USEFUL FOR

Chemistry students, chemical engineers, and researchers focusing on thermodynamics and hydration reactions of metal oxides.

vijayram
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Please post this type of questions in HW section using the template.
Arrange the energy released upon hydration of Magnesium Oxide,calcium oxide,barium oxide,strontium oxide.

I placed Magnesium oxide at the last,since magnesium hydroxide is a stable so lot of energy must be released in order to achieve that state,but the answer says calcium oxide.
 
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