This question is from grade 12 university preparation level. The answer has to do something with rates of chemical reactions but I don't know what the answer is.

. When hydrogen peroxide H2O2 is used as an antiseptic on open wounds, bubbles form as a result of the following chemical reaction.

H2O2(aq) --------------> 2H2O(l) + O2(g)

This same hydrogen peroxide decomposes very slowly via the same chemical reaction when left in a bottle, even if temperature is increased to 36.8 oC (body temperature). Explain the two observations.

A coffee cup calorimeter contains 480.0 grams of water at 25.0 oC. To it are added: 380.0 grams of water at 53.5 oC 525 grams of water at 65.5 oC Consider the heat absorbed by the Styrofoam as negligible, calculate the expected final temperaturein oC

A. 38.2 oC
B. 88.7 oC
C. 67.6 oC
D. 48.2 oC
E. 94.4 oC
The correct answer should be D. I don't know how to do this question.

To explain the two observations, we need to understand the concept of reaction rates in chemical reactions. The reaction rate is a measure of how quickly a reaction occurs. Factors such as temperature, concentration, surface area, and the presence of catalysts can influence the rate of a chemical reaction.

Observation 1: Bubbles form when hydrogen peroxide is used as an antiseptic on open wounds.
When hydrogen peroxide is used as an antiseptic on open wounds, bubbles form because the hydrogen peroxide decomposes rapidly. The presence of an enzyme called catalase, naturally found in cells, catalyzes the breakdown of hydrogen peroxide into water (H2O) and oxygen gas (O2). This reaction occurs quickly in the presence of catalase, resulting in the formation of bubbles of oxygen gas.

Explanation 1: The rapid decomposition of hydrogen peroxide to produce bubbles is due to the presence of catalase, an enzyme that acts as a catalyst for the decomposition reaction.

Observation 2: Hydrogen peroxide decomposes slowly when left in a bottle, even at an increased temperature of 36.8 oC.
Even with an increased temperature of 36.8 oC (body temperature), hydrogen peroxide decomposes slowly when left in a bottle. This is because there is no catalase enzyme present in the bottle to catalyze the decomposition reaction. Without a catalyst, the decomposition of hydrogen peroxide proceeds at a much slower rate. As a result, the production of oxygen gas and the formation of bubbles occur at a much slower pace compared to when catalase is present.

Explanation 2: The slow decomposition of hydrogen peroxide in the absence of catalase enzyme accounts for the observed slow rate of reaction, even at an increased temperature of 36.8 oC.