Demonstration and Observation of How an Endothermic Reaction Works
9A
Endothermic
Bilal Ali
Aim: To demonstrate and observe how an endothermic reaction works.
Hypothesis: In these practical’s there were a lot of observations:
1) Magnesium and Hydrochloric Acid: what I observed was at the start it was 20.5oc then when I added hydrochloric acid it increased 23.7oc and there was steam coming out.
2) Hydrochloric Acid and Sodium Hydroxide: the initial temp was 20oc then when I added Sodium hydroxide it went up to 29℃. But there was no visual reaction.
3) Anhydrous Copper (II) Sulfate and Water: the initial temperature was 21℃ but when we added the water it was 30℃ so it went 9℃ high the visual change was that the water was ocean blue.
4) Sodium Theosulfate And Water: initial temperature is 23℃ when we added the water it was 14℃ It got deducted 9℃ no visual change only white water.
5) Potassium Nitrate and Water: initial temperature was 10℃ then when we added water to the substance it dropped 4℃ no visual change only white water.
Prediction: My prediction was that they were going to all get cold and crack or just too hot and explode like glass bursting.
Materials: * Balance * Spatula and watch glass. * Stirring rod. * Potassium nitrate * Sodium thiosulfate
Method:
Potassium nitrate in water 1. Add 10mL of water into a test tube 2. Then add 2g of potassium nitrate 3. Place thermometer into the test tube 4. Stir well 5. Then record final results
Dissolving sodium thiosulfate in water 1. Add 10mL of water into a test tube 2. Then add 2g of sodium thiosulfate 3. Stir well 4. Place thermometer into the test tube 5. Then record final results
Results/Observations:
Table #2: Endothermic Chemical Process | Initial Temperature | Final Temperature | Decreasing In Temperature | Potassium nitrate | 20.5℃ | 14℃ | 9℃ | Sodium thiosulfate | 10℃ | 6℃ | 2℃ |
Discussion: The results in this practical are very interesting as it shows that the endothermic
Endothermic
Bilal Ali
Aim: To demonstrate and observe how an endothermic reaction works.
Hypothesis: In these practical’s there were a lot of observations:
1) Magnesium and Hydrochloric Acid: what I observed was at the start it was 20.5oc then when I added hydrochloric acid it increased 23.7oc and there was steam coming out.
2) Hydrochloric Acid and Sodium Hydroxide: the initial temp was 20oc then when I added Sodium hydroxide it went up to 29℃. But there was no visual reaction.
3) Anhydrous Copper (II) Sulfate and Water: the initial temperature was 21℃ but when we added the water it was 30℃ so it went 9℃ high the visual change was that the water was ocean blue.
4) Sodium Theosulfate And Water: initial temperature is 23℃ when we added the water it was 14℃ It got deducted 9℃ no visual change only white water.
5) Potassium Nitrate and Water: initial temperature was 10℃ then when we added water to the substance it dropped 4℃ no visual change only white water.
Prediction: My prediction was that they were going to all get cold and crack or just too hot and explode like glass bursting.
Materials: * Balance * Spatula and watch glass. * Stirring rod. * Potassium nitrate * Sodium thiosulfate
Method:
Potassium nitrate in water 1. Add 10mL of water into a test tube 2. Then add 2g of potassium nitrate 3. Place thermometer into the test tube 4. Stir well 5. Then record final results
Dissolving sodium thiosulfate in water 1. Add 10mL of water into a test tube 2. Then add 2g of sodium thiosulfate 3. Stir well 4. Place thermometer into the test tube 5. Then record final results
Results/Observations:
Table #2: Endothermic Chemical Process | Initial Temperature | Final Temperature | Decreasing In Temperature | Potassium nitrate | 20.5℃ | 14℃ | 9℃ | Sodium thiosulfate | 10℃ | 6℃ | 2℃ |
Discussion: The results in this practical are very interesting as it shows that the endothermic