Learning objective
Convert calorimetry data into molar enthalpy changes.
Read the explanation, check the common trap, then practise with flashcards and questions.
At a glance
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Flashcards
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Questions
Topic
Energetics
Subtopic
Calorimetry and enthalpy measurements
Study support
Understand this objective
Quick explanation
Convert calorimetry data into molar enthalpy changes
- This point belongs to Energetics, especially Calorimetry and enthalpy measurements.
- You need to be able to convert calorimetry data into molar enthalpy changes.
- The key ideas to know are calorimetry and molar enthalpy.
- Use the linked flashcards and practice questions to check recall, then practise applying the idea in an exam-style answer.
Key concepts
Why it matters
This objective helps connect Calorimetry and enthalpy measurements to exam-style questions, flashcards, and revision notes for Energetics.
Quick student answer
What is the molar enthalpy change (ΔH) when 2.0 g of a substance is burned in excess oxygen, releasing 1500 J of energy? (Molar mass of the substance = 50 g/mol)
Direct answer
75 kJ/mol
Key terms
- Calorimeter: An instrument used to measure the amount of heat involved in a chemical reaction or physical process.
- Enthalpy change (ΔH): The heat content change of a system at constant pressure, typically measured in kJ/mol.
Common trap
Incorrect unit conversion: Always convert energy values to kJ by dividing by 1000 before performing calculations.
Related questions
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Flashcard prompts
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Revision tools
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Practice Questions0 linked questions
Revision notestopic notes
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Open revision notesRelated learning objectives
- Define enthalpy change under constant pressure.
Enthalpy change
- Distinguish exothermic and endothermic reactions using enthalpy change signs.
Enthalpy change
- Interpret reaction profile diagrams.
Enthalpy change
- Define standard enthalpy changes for formation, combustion and neutralisation where appropriate.
Enthalpy change
- Use q = mcΔT to calculate heat energy transferred.
Calorimetry and enthalpy measurements