Extended post-lab (Thermochemistry) by Ronace Philip

QUESTION 1 : Reflect on what you observed during the experiment. Did the temperature of the reaction mixture increase or decrease?

xxronacexx — 2022-02-17 02:28:24 UTC

QUESTION 2 : Determine whether the reaction was exothermic or endothermic. Explain your reasoning, considering both the theoretical prediction and your experimental observations.

xxronacexx — 2024-05-06 16:24:20 UTC

QUESTION 3 : Another real-life scenario is self-inflating balloons that use the reaction between citric acid and baking soda to inflate. Explain how the process occurs and what type of reaction it is.

xxronacexx — 2024-05-06 16:24:39 UTC

ANSWER QUESTION 1

2024-07-03 17:10:16 UTC

The temperature rises for the baking soda and citric acid combinations. In contrast, the temperature drops for the baking soda and calcium chloride combinations.

ANSWER QUESTION 2

2024-07-03 17:12:36 UTC

i) Citric acid and baking soda (sodium bicarbonate) react endothermically. This conclusion is predicated on the idea that a chemical reaction is endothermic if it consumes more energy than it releases. Baking soda and citric acid react to generate sodium acetate, carbon dioxide gas, and water. An endothermic reaction is indicated by a drop in reaction mixture temperature, which is caused by the process of breaking the bonds in the reactants (citric acid and baking soda) requiring more energy than the production of bonds in the products.

ii) An exothermic reaction is the one that occurs when calcium and baking soda (sodium bicarbonate) interact. This indicates that as a result of the reaction, the surrounding air temperature rises. When new bonds are formed in the products of this reaction, more energy is produced than is consumed to break the bonds in the reactants. The reaction is exothermic due to this property.

ANSWER QUESTION 3

2024-07-03 17:13:57 UTC

A pill of baking soda and a sachet of citric acid are inside the balloon. The baking soda and citric acid combine when the packet bursts, releasing carbon dioxide gas. The balloon is inflated by this gas. Because of the endothermic nature of the reaction, more energy is needed to break the bonds in the reactants than is released during the formation of new bonds in the products.