In this experiment, the reaction between vinegar (acetic acid) and baking soda (sodium bicarbonate) produces carbon dioxide gas, water, and sodium acetate. The relevant chemical reaction can be represented as:
\[ \text{NaHCO}_3 (s) + \text{CH}_3\text{COOH} (aq) \rightarrow \text{CO}_2 (g) + \text{H}_2\text{O} (l) + \text{CH}_3\text{COONa} (aq) \]
When vinegar is added to the mixture, the acetic acid reacts with the sodium bicarbonate, and this reaction is exothermic (it releases heat). Therefore, as more vinegar is added, more acetic acid reacts with the sodium bicarbonate, resulting in more heat being produced.
Consequently, the increase in the amount of reactants leads to a greater rate of reaction, which produces more carbon dioxide and releases more energy in the form of heat. This results in a more significant temperature change in the mixture of water, dish soap, and baking soda.
Overall, the greater temperature change observed with the addition of more vinegar is due to the increased amount of heat generated by the higher rate of reaction between acetic acid and sodium bicarbonate.