Final answer:
The question is related to the decomposition and reaction rates of sucrose, which has a molecular formula of C12H22O11. Discussion includes first-order kinetics, rate laws, and the Arrhenius equation for determining kinetic parameters. Molarity calculations are also addressed for real-world application.
Step-by-step explanation:
Understanding Sucrose Decomposition
Honing in on the chemical properties of sucrose, which has the molecular formula C12H22O11, and considering its decomposition gives us insight into several chemical principles. Sucrose is a carbohydrate and yields about 4 kcal/g of energy upon metabolism, closely aligning with the expected value for sugars. When it comes to its decomposition, such as the hydrolysis of sucrose into glucose and fructose – both with the molecular formula of C6H12O6 but with different structural arrangements of atoms – we observe a first-order rate law governing the reaction.
The rate of reaction or decomposition can be affected by several factors including temperature. Using the Arrhenius equation, we can estimate changes in the rate constant, k, with changes in temperature. This allows for the determination of the activation energy and the frequency factor of the reaction.
In practical terms, such as determining the concentration of sucrose in a cup of tea after a teaspoon of sugar is dissolved, knowing the molarity of the solution is important. The molarity can be calculated by understanding the number of moles of sucrose and the volume of the solvent in which it is dissolved.