Endo vs Exo Which side will you take?

Introduction   

  

     In chemistry class you might of heard of the words "Endothermic" and "Exothermic". If you are like me you would of wondered what exactly did those words mean. I mean they sound similar, how much of a difference could there be? The answer Endothermic reactions and Exothermic reactions are night and day. The following will showcase the differences between the two words.

                                                   Endothermic                                       Exothermic 

     There are so many different types of learners in the world today. I for one learn best when I am able to experience or physically do something. So in this light the STEM academic strand students at SSIS Malarayat did an experiment focusing on the Endothermic and Exothermic reactions of Acids and Bases.


Procedures


Perform the following procedure, and identify each as either endothermic or exothermic, through temperature reading. For all procedures, take not of the initial temp. reading of the first solution/water, and then, the final temp. Draw a complete energy level diagram for each.

1. Mix 10 mL of dilute hydrochloric acid and 10 mL sodium hydroxide. Perform this cautiously by adding the acid TO the base in incremental amounts
2. Prepare 1 g of zinc dust in a test tube. Add 10 mL dilutated hydrochloric acid.
3. Dissolve 1 g of barium chloride in 150 mL water.
4. Dissolve 1 g of ammonium chloride in 150 mL water.
5. Dissolve 1 g of sodium hydroxide flakes in 150 mL water.
6. Dissolve 1 g of magnesium nitrate in 150 mL water.
7. Add 5 mL of potassium dichromate to 15 mL ethanol.
8. Add 1 g of anhydrous copper sulfate in 25 mL water

Experiment Proper

1. Mix 10 mL of dilute hydrochloric acid and 10 mL sodium hydroxide. Perform this cautiously by adding the acid TO the base in incremental amounts.

Figure 1.1

2. Prepare 1 g of zinc dust in a test tube. Add 10 mL dilutated hydrochloric acid.

Figure 1.2

3. Dissolve 1 g of barium chloride in 150 mL water.

Figure 1.3

4. Dissolve 1 g of ammonium chloride in 150 mL water.

Figure 1.4

5. Dissolve 1 g of sodium hydroxide flakes in 150 mL water.

Figure 1.5

6. Dissolve 1 g of magnesium nitrate in 150 mL water.

Figure 1.6

7. Add 5 mL of potassium dichromate to 15 mL ethanol.

Figure 1.7

8. Add 1 g of anhydrous copper sulfate in 25 mL water

Figure 1.8

Results 

Table 1.1 

Table 1.1 shows the differences in temperature of each reaction. 

Table 1.2 

Table 1.2 shows the type of reaction these acids and bases have displayed. 

Video