SUMMARY
The molar enthalpy of combustion of magnesium is calculated based on the energy released when burning a 1.0g sample, which is 25.5 kJ. Given that the molar mass of magnesium is approximately 24.31 g/mol, the molar enthalpy of combustion is determined to be -306.2 kJ/mol. This value indicates the energy released per mole of magnesium combusted, confirming option c) -306.2 kJ/mol as the correct answer. The reaction involved is 2Mg + O2 --> 2MgO.
PREREQUISITES
- Understanding of molar mass calculations
- Basic knowledge of thermodynamics and enthalpy
- Familiarity with calorimetry principles
- Ability to balance chemical equations
NEXT STEPS
- Study the concept of molar enthalpy and its applications in thermodynamics
- Learn about calorimetry and how to perform energy calculations
- Explore the combustion reactions of other metals for comparative analysis
- Investigate the implications of enthalpy changes in chemical reactions
USEFUL FOR
Chemistry students, educators, and professionals involved in thermodynamics and combustion analysis will benefit from this discussion.