A scientist fills two test tubes with different aqueous solutions and adds different compounds to each solution. After the reactions are complete, the scientist measures the temperature of each solution. The table shows the results of the experiment.
Test Tube1 Test Tube2
Initial Temperature 20°C | 20°C
Final Temperature
25°C | 19°C

Which statement best explains the results?

A. The products in test tube 1 have a lower potential energy than the products in test tube 2.

B. The reaction in test tube 1 has a higher activation energy than the reaction in test tube 2.

C. Test tube 1 has a catalyst, and test tube 2 does not.

D. The reaction in test tube 1 is exothermic, and the reaction in test tube 2 is not.

The option that best explains the result is option D. That is, the reaction in test tube 1 is exothermic, and the reaction in test tube 2 is not.

Change in chemical reaction:

In a chemical reaction, heat is either absorbed or released.

In a reaction where there is absorption of heat from the surrounding is called an endothermic reaction.

While in a reaction where heat is released into the surrounding is called exothermic reaction.

From the experiment, there is increase in temperature, from 20 to 25°C, which shows the release of temperature to the surrounding.

Therefore, the reaction in test tube 1 is exothermic, and the reaction in test tube 2 is not.

Learn more about exothermic reaction here:

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