Thermochemistry is about studying heat changes during chemical reactions
Hey S3 click on ‘formal note’ below to get a copy of the unit notes. I’ve now coloured it and made it bold. I’ve put it between the dashed lines. What more can I do. Surely you can get it now! Doc F
1. Magnesium burning
A piece of magnesium was set alight.
It burned with a bright white flame.
The reaction is obviously producing heat and light energy.
2. Heat changes when substances dissolve
20cm3 of water were measured into a polystyrene cup and the temperature measured.
Two spatulas of solid were dissolved in it and the temperature measured again.
|solid||temperature 1 (ºC)||temperature 2 (ºC)||change (ºC)|
When substances dissolve they can give out, or take in heat.
3. The best fuel
An investigation was carried out to see which of two fuels had the greater heat output – petrol or methylated spirits.
A burner containing methylated spirits was weighed.
The burner was used to warm some water by about 40°C.
The burner was reweighed.
Using the difference in temperature and the difference in mass the heat produce by the burner was calculated.
|Fuel||Mass (g)||Temperature (°C)||Heat|
4. The bomb calorimeter
The bomb calorimeter is used to measure heat produced from combustion reactions.
5. Exothermic and Endothermic Reactions – an investigation
The reactions were carried out in a poly-cup as shown. The temperature change was followed using a temperature probe connected to a Logit Datameter 1000. This was linked to a PC and the data captured.
Here is sodium bicarbonate (baking soda) being reacted with citric acid.
And a screen shot of the data being captured.
The experiment was repeated reacting magnesium powder with hydrochloric acid. A printout was obtained and temperatures worked out.
|Sodium bicarbonate + citric acid||18||12||-6|
|Magnesium + hydrochloric acid||18||45||+27|
So the reaction between sodium bicarbonate and citric acid is endothermic. The temperature falls as heat is taken in from the surroundings.
The reaction between magnesium and hydrochloric acid is exothermic. The temperature rises as heat is given out.
Chemiluminescence is the production of light using a cold chemical reaction.
Luminol produces light in the presence of certain oxidisers.
Here luminol is reacted with sodium hypochlorite.
Solution 1 – 0.02 g of luminol and 15 ml of 0.1 M sodium hydroxide are made up to 200 ml with water.
Solution 2 – 7 ml of stock sodium hypochlorite are made up to 25 ml with water
3 ml of solution 2 are added with a dropper to 50 ml of solution 1 in a beaker.
[pro-player type=’video’ image=’http://hferrier.co.uk/school/wp-content/uploads/2013/04/image.jpeg’]http://hferrier.co.uk/school/wp-content/uploads/2013/03/luminol1.flv[/pro-player]
This time luminol is reacted with hydrogen peroxide
Solution 1 – 4 g sodium carbonate, 0.2 g luminol, 24 g sodium bicarbonate, 0.5 g ammonium bicarbonate and 0.4 g copper II sulphate made up to 1 l with water
Solution 2 – 50 ml of 10 vol hydrogen peroxide made up to 1 l with water
20 ml of solution 1 are added to 20 ml of solution 2 in beakers
[pro-player type=’video’ image=’http://hferrier.co.uk/school/wp-content/uploads/2013/04/image1.jpeg’]http://hferrier.co.uk/school/wp-content/uploads/2013/03/luminol2.flv[/pro-player]
An internet research was carried on Chemiluminescence by answering some questions
I can collect and analyse experimental data on chemical reactions that result in an obvious change in energy. I can apply my findings to explain the significance of the energy changes associated with chemical reactions.
Energy changes of chemical reactions
Recognition and uses of exothermic and endothermic reactions.
Reactions can be exothermic or endothermic. This is dependent on the overall energy change taking place.
Energy from fuels
Different fuels provide different quantities of energy and this can be measured experimentally and calculated