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Demos

Demos. How would you sort these?. Year 12 Chemistry. Topic 8 Energetics 1 Text book page 237 Enthalpy Introduction. Topic 8 Energetics 1. Lesson 1: Enthalpy Introduction Success criteria

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Demos

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  1. Demos

  2. How would you sort these?

  3. Year 12 Chemistry Topic 8 Energetics 1 Text book page 237 Enthalpy Introduction

  4. Topic 8 Energetics 1 Lesson 1: Enthalpy Introduction Success criteria • explain that some chemical reactions are accompanied by enthalpy changes, exothermic (ΔH, negative) or endothermic ΔH, positive) • Know that enthalpy change is the heat energy change measured at constant pressure • construct a simple enthalpy level diagrams for a reaction to show the difference in the enthalpy of the reactants compared with that of the products • explain qualitatively, using reaction profile diagrams, the term activation energy

  5. Practical We will do two simple test-tube experiments, in each case we add a solid to a liquid: • Hydrochloric acid plus magnesium ribbon. • Water plus ammonium nitrate For each case, write a prediction of what will happen.

  6. Practical Practical 1: • Put 5 cm depth of hydrochloric acid in a test tube. • Add a piece of magnesium ribbon. • Write down ALL your observations. • Write an equation for what happened. Practical 2: • Put 5 cm depth of water in a test tube. • Add a spatula of ammonium nitrate. • Write down ALL your observations. • Write an equation for what happened.

  7. Definitions NOW write definitions of: • Exothermic reaction • Endothermic reaction • Enthalpy

  8. Enthalpy Definitions: • Enthalpy, H, is the heat content that is stored in a system. • Chemical system is the reactants and the products • Surroundings is whatever is outside the chemical system.

  9. Enthalpy • It is impossible for us to actually measure how much heat energy is in a system. • What can we measure? • We can measure the energy that is given out or absorbed by a chemical system during a chemical change. • We are actually measuring the heat exchange between the chemical system and its surroundings.

  10. The law of conservation of energy The law of conservation of energy states… …that energy cannot be created or destroyed, only moved from one place to another. So if a chemical system releases energy, the surroundings must gain exactly the same amount of energy.

  11. Conservation of Energy Heat loss in a chemical system = heat gain in the surroundings We see this as a _________ in temperature Heat gain in a chemical system = heat loss from the surroundings We see this as a _________ in temperature n increase decrease

  12. Enthalpy Changes • In a chemical reaction, either the products or the reactants will have more energy. • An enthalpy change, ΔH is: • The heat exchange with the surroundings during a reaction, at constant pressure. • The difference between enthalpy of the products and enthalpy of the reactants: ΔH = Hproducts - Hreactants

  13. Activity • Cut out the boxes and stick in place on the diagram to explain exothermic and endothermic reactions. • Don’t stick them down yet. • Place them where you think they go • We will cover more of the topic and continue to look back at this

  14. Exothermic & Endothermic We now need better definitions of exothermic and endothermic reactions. For each type of reaction: • Is heat lost to or gained from the surroundings? • Which has the smaller enthalpy, reactants or products? • Is ΔH negative or positive?

  15. Exothermic • Heat is lost to the surroundings? • The enthalpy of the products is smaller than the enthalpy of the reactants. • H products < H reactants • ΔH is negative.

  16. Self heating cans use exothermic reactions

  17. Endothermic • Heat is gained from the surroundings? • The enthalpy of the products is larger than the enthalpy of the reactants. • H products > H reactants • ΔH is positive.

  18. Exothermic Reactions The most exploited exothermic reaction in the world is… …combustion of fuels • Write an equation for burning methane (natural gas) in oxygen. • Which have more enthalpy, products or reactants? • Is ΔH positive or negative?

  19. Exothermic Reactions Combustion of Fuels Burning methane in oxygen: CH4(g) + 2O2(g)  CO2(g) + 2H2O(l)ΔH = -890kJ.mol-1 The units are kJ.mol-1 so it is the amount of energy per mole.

  20. Exothermic Reactions Respiration Probably the most important reaction for living things, it gives out energy so is exothermic: Glucose + Oxygen  Carbon dioxide + Water C6H12 O6 (aq) + 6O2(g)  6CO2(g) + 6H2O(l)ΔH = -2801kJ.mol-1

  21. Endothermic Reactions Thermal decomposition of limestone Endothermic reactions require energy input for them to take place. CaCO3 (s)  CaO(s) + CO2(g)ΔH = +178 kJ.mol-1

  22. Endothermic Reactions Photosynthesis Probably the most important endothermic reaction for living things, it requires energy: 6CO2(g) + 6H2O(l)  C6H12 O6 (aq) + 6O2(g)ΔH = +2801kJ.mol-1 What type of energy does it take in?

  23. Topic 8 Energetics 1 Lesson 1: Enthalpy Introduction Success criteria • explain that some chemical reactions are accompanied by enthalpy changes, exothermic (ΔH, negative) or endothermic ΔH, positive) • Know that enthalpy change is the heat energy change measured at constant pressure • construct a simple enthalpy level diagrams for a reaction to show the difference in the enthalpy of the reactants compared with that of the products • explain qualitatively, using reaction profile diagrams, the term activation energy

  24. Enthalpy Level Diagram • A simple enthalpy level diagram shows: • the symbols and enthalpy of products • the symbols and enthalpy of reactants • the enthalpy change • You need to be able to draw them and include all the features.

  25. Enthalpy Level Diagram • A simple enthalpy level diagram: Exothermic

  26. Enthalpy Level Diagram • A simple enthalpy level diagram: Endothermic

  27. Activation Energy • Why doesn’t magnesium spontaneously burn in air? • It’s products have less energy than it’s reactants so there is no reason they can’t form? • Yes there is – Activation energy! • We need an input of energy in the first place to break the bonds and allow the reaction to start.

  28. Activation Energy • Once the reaction has been started it is giving out energy so the activation energy can continue to be overcome and the reaction is self-sustaining. • This reaction profile diagram shows the activation energy

  29. Activation Energy • An endothermic reaction has activation energy too.

  30. Now • Check you have all of the enthalpy mind map complete • Complete the following questions • Draw reaction profile diagrams for the following reactions 1) You are given the data for the following reaction CO(g) + NO2 (g)  CO2 (g) + NO (g) ΔH = -226 kJ mol-1 Ea = + 134 kJ mol-1 2) You are given the data for the following reaction H2 (g) + I2 (g)  2HI (g) ΔH = +53 kJ mol-1 Ea = + 183 kJ mol-1 More questions a) What does enthalpy mean? b) What decides if a reaction is endothermic or exothermic?

  31. Topic 8 Energetics 1 Lesson 1: Enthalpy Introduction Success criteria • explain that some chemical reactions are accompanied by enthalpy changes, exothermic (ΔH, negative) or endothermic ΔH, positive) • Know that enthalpy change is the heat energy change measured at constant pressure • construct a simple enthalpy level diagrams for a reaction to show the difference in the enthalpy of the reactants compared with that of the products • explain qualitatively, using reaction profile diagrams, the term activation energy

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