Energetics
5.1 Measuring energy changes SL
• Heat is a form of energy.
• Temperature is a measure of the average kinetic energy of the particles.
• Total energy is conserved in chemical reactions.
• Chemical reactions that involve transfer of heat between the system and the surroundings are described as endothermic or exothermic.
• The enthalpy change (∆H) for chemical reactions is indicated in kJ mol-1.
• ∆H values are usually expressed under standard conditions, given by ∆H°, including standard states.
• Calculation of the heat change when the temperature of a pure substance is changed using q=mc∆T.
• A calorimetry experiment for an enthalpy of reaction should be covered and the results evaluated.
• Heat is a form of energy.
• Temperature is a measure of the average kinetic energy of the particles.
• Total energy is conserved in chemical reactions.
• Chemical reactions that involve transfer of heat between the system and the surroundings are described as endothermic or exothermic.
• The enthalpy change (∆H) for chemical reactions is indicated in kJ mol-1.
• ∆H values are usually expressed under standard conditions, given by ∆H°, including standard states.
• Calculation of the heat change when the temperature of a pure substance is changed using q=mc∆T.
• A calorimetry experiment for an enthalpy of reaction should be covered and the results evaluated.
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The difference between temperature and heat, how to draw enthalpy diagrams. How to measure heat change Q and determine the enthalpy of a reaction using calorimetry and Q=mcdT with practice problems
1:03 Enthalpy H 1:47 dH exothermic and endothermic reactions 2:56 Enthalpy diagrams 5:06 Examples of exothermic reactions 5:49 Measuring heat energy change Q 6:22 Calorimetry 8:07 Calculations for calorimetry 9:24 Example problem 1 10:27 Example problem 2 |
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What triggers a chemical reaction? - Teacher Sep
Chemicals are in everything we see, and the reactions between them can look like anything from rust on a spoon to an explosion on your stovetop. But why do these reactions happen in the first place? Kareem Jarrah answers this question by examining the two underlying forces that drive both endothermic and exothermic chemical reactions: enthalpy and entropy.