This page contains the detailed and easy notes for GCSE CCEA Chemistry Energy Changes in Chemistry for revision and understanding Energy Changes in Chemistry .
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Law of conservation of energy states that energy is neither created nor destroyed. It just converts from one form to another.
| Exothermic Reactions | ENDOTHERMIC REACTIONS |
| Reactions that releases heat to the surroundings. | Reactions that takes in heat from the surroundings |
| The reaction is accompanied by increase in temperature of the surroundings as the heat is released. | The reaction is accompanied by decrease in temperature of the surroundings as the heat is absorbed. |
| The product have the lower energy than the reactants. | The products have higher energy than the reactants. |
| Example: Combustion reaction and Respiration | Example: Thermal decomposition and -Photosynthesis |
| In terms of bond breaking the energy released in making the product is more than energy used up in breaking the reactants. | In terms of bond breaking the energy used in breaking the bonds of reactants is more than the energy released in making up of the products. |
| Used in self heating cans and hand warmers | Used in Ice packs made for sports injuries |
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Exothermic Reaction
Endothermic Reaction
Defining Exothermic and Endothermic in terms of Bond making and Breaking
| Reactants | Products | ||
| Bonds are always broken in a reaction | Bonds are always made in a reaction. | ||
| Endothermic | Breaking of bonds of the reaction takes in heat | > | Making of bonds of the products Releases heat. |
| Exothermic | Breaking of bonds of the reaction takes in heat | < | Making of bonds of the products releases heat. |
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A2 + B2 2AB
A-A + B-B 2[A-B]
221+ 325 2 x 425
546 850
| Bond | Energy |
| A-A | 221 |
| B-B | 325 |
| A-B | 425 |
Energy used in breaking the bonds – 546 KJ/mol
Energy released in making the bonds – 850KJ/mol
Energy associated in overall reaction – 546- 850 = -304 KJ/mol
Is it Exothermic or Endothermic – Exothermic as energy is released in products is greater
At the Negative Electrode
2H2(g) + 4OH–(aq) 4H2O(l) + 4e–
At the Positive Electrode
O2 + 2H2O + 4e– 4 OH–(aq)
Overall – 2H2(g) + O2 (g) 2H2O(l)
ADVANTAGES
DISADVANTAGES
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Exothermic Reaction – The reaction which gives out heat to the surroundings. Example: Respiration or Combustion
Endothermic Reaction – The reactions which taken in heat from the surrounding. Example: Photosynthesis or Thermal decomposition
Reaction Profile – Diagramatic representation showing the relative energies of reactants and products in a reaction.
Activation – Minimum energy required to start a reaction.
Bond Energy – Heat energy contained in a bond between two atoms.
Chemical Cells – A device that converts chemical energy into electrical energy.
Fuel Cells – A chemical cells that uses a reaction between hydrogen and oxygen to form water and energy.
Batteries – collection of cells.
Label the reaction profile and classify it as Exothermic or Endothermic
ADVANTAGES
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DISADVANTAGES
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Disclaimer:
I have tried my level best to cover the maximum of your specification. But this is not the alternative to the textbook. You should cover the specification or the textbook thoroughly. This is the quick revision to help you cover the gist of everything. In case you spot any errors then do let us know and we will rectify it.
References:
BBC Bitesize
Wikipedia
Wikimedia Commons
Image Source:
Wikipedia
Wikimedia
Commons
Flickr
Pixabay
Make sure you have watched the above videos and are familiar with the key definations before trying these questions. It is also good to time yourself while doing these questions so that you can work on the speed as well.